Chemicals

35% Food Grade Hydrogen Peroxide This is the highest concentration of hydrogen peroxide we offer.   Our food-grade peroxide is clear, colorless, and free of any stabilizers or additives.  Peroxide is one of the most effective oxidizers and may be applied to food directly to food products.  Our peroxide is certified FCC (Food Chemical Codex).  It has been tested and verified for its quality and purity.  35% Food Grade Hydrogen Peroxide Certificate of Analysis 35% Food Grade Hydrogen Peroxide Safety Data Sheet Our food-grade hydrogen peroxide is 12x strength, when diluted you can make a remarkably large volume of 3% hydrogen peroxide that can be used for a wide variety of applications.   1 Quart 35% Makes 4.2 Gallons of 3% 1 Gallon 35% Makes 11.5 Gallons of 3% 5 Gallon 35% Makes 57.8 Gallons of 3% 55 Gallon 35% Makes 634 Gallons of 3%   Some applications include... Elevating Plant Growth: Diluted hydrogen peroxide supports healthy roots and elevated oxygen availability in the soil. Excellent Cleaner for Food Prep Environments: Hydrogen peroxide is a disinfectant, that kills viruses and various forms of bacteria. Bleaching: Diluted hydrogen peroxide is a mild bleaching agent that can be used to clean stains.  Cleansing Fresh Produce: Diluted hydrogen peroxide can be used to clean fruits and vegetables.  Mold and Mildew Removal: Hydrogen peroxides strong oxidative qualities breakdown mold and mildew with ease.  How to Dilute 35% Hydrogen Peroxide to 3% Hydrogen Peroxide: 35% food-grade hydrogen peroxide Deionized distilled water A clean, empty Gallon bottle for the final 3% hydrogen peroxide solution Measuring cup Funnel Safety goggles Rubber gloves Apron or old clothes Steps to perform dilution: Wear safety goggles, rubber gloves, an apron or old clothing to protect yourself from spills and splashes.  Choose a well-ventilated space. Mix 1 part 35% hydrogen peroxide with 11 parts distilled water. Example: Mix 1 cup hydrogen peroxide, with 11 cups of distilled water.  To be exact, this will make a slightly less than 3% solution of hydrogen peroxide – 2.92%. What Is Hydrogen Peroxide? Hydrogen peroxide (H2O2) is a chemical compound composed of two hydrogen atoms and two oxygen atoms. It is a clear, colorless liquid with a slightly more viscous consistency than water. Hydrogen peroxide is commonly used for its powerful oxidizing properties and has a wide range of applications in various industries and household settings. What Are The Properties Of Hydrogen Peroxide? Hydrogen peroxide (H2O2) is a clear, colorless liquid with several notable properties: Chemical Formula: H2O2 - It consists of two hydrogen atoms (H) and two oxygen atoms (O) linked by a single covalent bond, as well as a second oxygen atom connected to one of the hydrogen atoms by a single covalent bond. Molecular Weight: Approximately 34.01 grams per mole. Physical State: Hydrogen peroxide is a liquid at room temperature and pressure (25°C or 77°F). Odor: It has a slightly sharp and distinctive odor. Solubility: Hydrogen peroxide is miscible (mixes completely) with water in all proportions. Density: The density of hydrogen peroxide varies with concentration. A common concentration of 3% hydrogen peroxide has a density of approximately 1.01 grams per milliliter (g/mL). Boiling Point: The boiling point of hydrogen peroxide is approximately 150.2°C (302.4°F). Melting Point: Pure hydrogen peroxide does not have a distinct melting point because it decomposes before reaching a stable liquid state at atmospheric pressure. Reactivity: Hydrogen peroxide is a powerful oxidizing agent and is highly reactive with various substances, including organic compounds and some metals. It readily decomposes into water and oxygen when exposed to heat, light, or certain catalysts. Concentration: Hydrogen peroxide is available in various concentrations, with common household solutions typically being around 3%. Higher concentrations, such as 30% or 35%, are used in industrial and laboratory applications. pH: The pH of hydrogen peroxide solutions varies with concentration but is typically slightly acidic. Stability: Hydrogen peroxide solutions are not indefinitely stable and can decompose over time, especially when exposed to light, heat, or contaminants. Storing hydrogen peroxide in a cool, dark place in a well-sealed container helps preserve its stability. Safety: Concentrated hydrogen peroxide solutions can be hazardous and should be handled with care. Contact with skin or eyes should be avoided, and protective equipment may be required when working with high-concentration solutions. These properties make hydrogen peroxide a versatile chemical with various applications in industries ranging from healthcare and cosmetics to water treatment and rocket propulsion. The concentration and handling precautions should be considered based on the specific use and requirements of the application. What Is Hydrogen Peroxide Used For? Hydrogen peroxide (H2O2) is used for a wide range of purposes in various industries and household settings due to its versatile properties. Some common uses of hydrogen peroxide include: Disinfectant and Antiseptic: Hydrogen peroxide is a common disinfectant and antiseptic agent. It is used to clean wounds, cuts, and minor injuries to prevent infection. In lower concentrations (typically 3%), it can be safely applied to the skin. Hair Bleaching and Dyeing: Many hair bleaching and hair dyeing products contain hydrogen peroxide as it can help break down the natural pigments in hair, lightening its color. Teeth Whitening: Hydrogen peroxide is used in some teeth whitening products and dental treatments to remove stains and discoloration from teeth. Cleaning Agent: It is used as a cleaning agent for surfaces, fabrics, and contact lenses due to its ability to break down and remove organic stains and deposits. Water Treatment: In water treatment processes, hydrogen peroxide can be used to remove contaminants, oxidize organic matter, and disinfect water supplies. Rocket Propellant: In the aerospace industry, highly concentrated hydrogen peroxide (usually around 90% purity) is used as a rocket propellant. Chemical Synthesis: Hydrogen peroxide is used in the synthesis of various chemicals and pharmaceuticals. Environmental Applications: It can be employed for soil and groundwater remediation, helping to break down pollutants and contaminants. Food Industry: In the food industry, hydrogen peroxide can be used for cleaning and disinfection of equipment and packaging materials. Cosmetics: It is used in some cosmetic and personal care products, such as hair dyes, hair bleaches, and skin creams. Textiles: Hydrogen peroxide is used in the textile industry to bleach fabrics and remove stains. Paper and Pulp Industry: It is used for bleaching paper pulp and improving the quality of paper products. Agriculture: In agriculture, hydrogen peroxide can be used as an oxygen source in soil, promoting plant growth. Medical and Laboratory Use: It is utilized for cleaning and sterilizing medical equipment and laboratory instruments. First Aid: Hydrogen peroxide is a household item for treating minor cuts and scrapes. The specific application and concentration of hydrogen peroxide used can vary depending on the intended purpose. Higher concentrations are typically used in industrial and chemical applications, while lower concentrations are common in household and personal care products. It's important to handle hydrogen peroxide with care, follow safety guidelines, and use the appropriate concentration for a given task. How Is Hydrogen Peroxide Produced? Hydrogen peroxide (H2O2) is typically produced through one of two main methods: the anthraquinone process and the direct synthesis process. Both processes involve the reaction of hydrogen and oxygen in the presence of a catalyst to form hydrogen peroxide. Here's an overview of these two methods: Anthraquinone Process: This is the most common method for commercial hydrogen peroxide production. It involves a series of chemical reactions that use anthraquinone derivatives as catalysts. The process typically consists of the following steps: Hydrogenation: Anthraquinone derivatives are hydrogenated with hydrogen gas (H2) to form hydroquinone derivatives. Autoxidation: The hydroquinone derivatives react with oxygen (O2) to form anthraquinone derivatives again, while producing hydrogen peroxide in the process. Extraction: The hydrogen peroxide is then extracted from the reaction mixture. Oxidation of Anthraquinone: The anthraquinone derivatives are oxidized back to their original form for reuse in the process. Direct Synthesis Process: In this method, hydrogen and oxygen are directly combined to produce hydrogen peroxide using a catalyst. The reaction typically occurs in a gas-phase reactor, and the process is often referred to as the "direct synthesis" or "hydrogenation-oxygenation" process. Common catalysts used in this process include palladium or platinum on a support material. While these are the main methods for hydrogen peroxide production, there are other less common methods as well. The choice of production method depends on factors such as the desired concentration of hydrogen peroxide, production scale, and cost considerations. It's worth noting that hydrogen peroxide is a sensitive compound and can decompose over time, especially when exposed to heat, light, or contaminants. Therefore, it requires careful handling and storage to maintain its stability and effectiveness. Does Hydrogen Peroxide Expire? Hydrogen peroxide can degrade over time and may lose its effectiveness, so it can be said to have a shelf life rather than a strict expiration date. The shelf life of hydrogen peroxide depends on several factors, including its concentration, exposure to light, temperature, and how well it's stored. Here are some general guidelines: Concentration: Higher concentrations of hydrogen peroxide (e.g., 30% or 35%) tend to be more stable and have a longer shelf life compared to lower concentrations (e.g., 3% or 6%). Exposure to Light: Hydrogen peroxide is light-sensitive, and exposure to ultraviolet (UV) light can accelerate its decomposition. It is typically sold in brown or opaque containers to protect it from light. Temperature: Storage at higher temperatures can also speed up the decomposition of hydrogen peroxide. It should be stored at a cool, dry place away from heat sources. Contaminants: Contaminants or impurities can catalyze the decomposition of hydrogen peroxide. It's essential to keep the container tightly sealed and free from any potential contaminants. Age: Hydrogen peroxide degrades slowly over time, even when stored correctly. The rate of degradation is higher for lower concentrations. To maximize the shelf life and potency of hydrogen peroxide, follow these recommendations: Store it in its original, tightly sealed container. Keep it in a cool, dark place away from direct sunlight and heat sources. Check the expiration date on the container, if available. If you're unsure about the potency of an old bottle of hydrogen peroxide, consider testing it on a small, non-critical area before using it for medical or cleaning purposes. It's important to note that even if hydrogen peroxide has degraded, it may still be useful for some applications, such as cleaning and disinfecting surfaces. However, for medical or first-aid use, it's best to use hydrogen peroxide that is within its recommended shelf life to ensure its effectiveness. Is Hydrogen Peroxide Safe As Mouthwash? Hydrogen peroxide can be used as a mouthwash, but it should be used with caution and in a diluted form. Here are some important considerations: Dilution: Never use undiluted hydrogen peroxide as a mouthwash. It's too concentrated at its full strength and can cause irritation, burning, and tissue damage. Instead, dilute it with water. A common recommendation is to use a 3% hydrogen peroxide solution, which is typically sold in drugstores. Frequency: Do not use hydrogen peroxide as a mouthwash too frequently. Using it daily or excessively can lead to oral issues, including irritation and disruption of the natural balance of oral bacteria. Duration: When using hydrogen peroxide as a mouthwash, swish it around your mouth for a brief period, typically about 30 seconds, and then spit it out. Do not swallow it. Rinse Thoroughly: After using hydrogen peroxide as a mouthwash, rinse your mouth thoroughly with water to remove any residual hydrogen peroxide. Avoid Ingestion: Do not swallow hydrogen peroxide, even when diluted. Swallowing hydrogen peroxide can lead to stomach upset and other health issues. Consultation: Before using hydrogen peroxide as a mouthwash, it's a good idea to consult with your dentist or oral healthcare provider. They can provide guidance on its safe and appropriate use based on your specific oral health needs. Hydrogen peroxide can help kill harmful bacteria in the mouth and may be used as a short-term remedy for issues like canker sores or minor gum irritations. However, it is not a substitute for regular oral hygiene practices such as brushing, flossing, and using a fluoride-based mouthwash. If you experience any adverse reactions, such as severe irritation, burning, or pain, discontinue use immediately and consult a healthcare professional. It's important to use hydrogen peroxide as a mouthwash cautiously and in accordance with recommended guidelines to avoid potential side effects or harm to oral tissues. What Are The Hazards Of Hydrogen Peroxide? Hydrogen peroxide, while commonly used for various purposes, can pose certain hazards if mishandled or used improperly. Here are some of the potential hazards associated with hydrogen peroxide: Irritation and Burns: Hydrogen peroxide is a strong oxidizing agent and can cause skin and eye irritation upon contact. In higher concentrations or with prolonged exposure, it can lead to chemical burns. Ingestion: Ingesting concentrated hydrogen peroxide can be harmful and even life-threatening. It can cause gastrointestinal irritation, stomach pain, vomiting, and, in severe cases, internal burns or damage. Inhalation: Inhalation of hydrogen peroxide vapors can irritate the respiratory tract, leading to coughing, shortness of breath, and throat irritation. Explosive Hazards: Concentrated hydrogen peroxide solutions can be sensitive to shock, heat, or contamination with organic materials. This can lead to the potential for explosions or fires if mishandled. Skin Sensitization: Prolonged or repeated contact with hydrogen peroxide can lead to skin sensitization, where the skin becomes more sensitive or allergic to the chemical. Environmental Impact: Hydrogen peroxide can be harmful to aquatic life and the environment if not properly disposed of. It should not be released into natural waterways. hydrogen peroxide, consider the following precautions: Dilution: When using hydrogen peroxide, dilute it to the appropriate concentration for the intended purpose. Most household hydrogen peroxide solutions are 3%, while higher concentrations are used for industrial or medical applications. Protective Equipment: When handling concentrated hydrogen peroxide, wear appropriate personal protective equipment, including gloves and safety goggles. Ventilation: Use hydrogen peroxide in well-ventilated areas to minimize inhalation risks. First Aid: In case of skin or eye contact, rinse immediately with plenty of water. If ingested, seek medical attention. Storage: Store hydrogen peroxide in a cool, dark place away from flammable materials and heat sources. Dispose Properly: Dispose of hydrogen peroxide in accordance with local regulations. Do not pour it down drains or release it into the environment. Always follow the safety guidelines and instructions provided on the product label or by the manufacturer. If you have specific concerns or questions about handling hydrogen peroxide for a particular application, it's advisable to consult with a safety professional or chemical expert for guidance. How Can I Use Hydrogen Peroxide Safely? Using hydrogen peroxide safely involves taking appropriate precautions to minimize the risk of accidents or harm. Here are some guidelines for safe handling and use of hydrogen peroxide: Read the Label: Always read and follow the instructions and safety precautions provided on the hydrogen peroxide product label. Different concentrations may have different recommended uses and safety guidelines. Personal Protective Equipment (PPE): Wear appropriate personal protective equipment, including safety goggles or a face shield to protect your eyes. Use gloves made of materials that are compatible with hydrogen peroxide, such as nitrile or latex gloves. Ventilation: Use hydrogen peroxide in a well-ventilated area to minimize exposure to vapors. If you're using it in a confined space, consider using a fume hood or working near an open window or door. Concentration: Ensure that you are using the correct concentration of hydrogen peroxide for your specific application. Most household hydrogen peroxide solutions are typically 3%, but higher concentrations are available for industrial or medical use. Dilution: When diluting concentrated hydrogen peroxide, always add the hydrogen peroxide to water, not the other way around. This helps prevent splattering and potential reactions. Avoid Contaminants: Keep hydrogen peroxide away from organic materials (e.g., paper, cloth) and flammable substances, as it can react with them and potentially cause fires or explosions. Avoid Mixing: Do not mix hydrogen peroxide with other chemicals unless you are following a specific recipe or procedure that requires it. Mixing hydrogen peroxide with certain substances can be dangerous. First Aid: In case of skin contact, immediately rinse the affected area with plenty of water. If hydrogen peroxide comes into contact with your eyes, flush them with water for at least 15 minutes and seek medical attention if irritation persists. If ingested, do not induce vomiting. Seek medical attention immediately. Storage: Store hydrogen peroxide in a cool, dark place, away from direct sunlight and heat sources. Keep the container tightly closed when not in use. Disposal: Dispose of hydrogen peroxide in accordance with local regulations. Do not pour it down drains or release it into the environment. Emergency Response: Have access to an emergency eyewash station and safety shower if you are working with concentrated hydrogen peroxide. Keep a spill kit and appropriate cleanup materials on hand in case of accidents. Training: Ensure that individuals handling hydrogen peroxide are trained in its safe use and understand the potential hazards. If you are unsure about how to use hydrogen peroxide safely for a specific application, consider seeking guidance from a safety professional or chemical expert. Always exercise caution and pr

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BVV™ High Purity Sodium Hydroxide 99% NSF Certified (Food Safe Chemical) Sodium Hydroxide is a highly versatile compound that finds extensive use in various applications, including acid-base extractions. As a strong base, Sodium Hydroxide is used to adjust the pH of aqueous solutions, making it an ideal choice for separating acidic and basic compounds during extraction. Also known as caustic soda, Sodium Hydroxide is a highly alkaline compound that is used in a wide range of applications beyond extraction including manufacturing, cleaning, and water treatment. At BVV, we pride ourselves on offering only the highest-quality chemicals and compounds, including Sodium Hydroxide. Our Sodium Hydroxide is a premium-grade product that is manufactured to the highest standards, ensuring exceptional quality and performance for your pH adjustment needs.  Our Sodium Hydroxide is NSF certified as a food safe chemical, which means it can be used in a variety of applications including drinking water and is evaluated safe for consumption.Our product is available in a range of sizes and quantities to suit your needs, and our team is always on hand to provide expert advice and support. High Purity Sodium Hydroxide Safety Data Sheet SDS High Purity Sodium Hydroxide Certificate of Analysis COA Chemical Formula: NaOH Molecular Weight: 39.9971 g/mol CAS Registry Number: 1310-73-2 Appearance White, hard (when pure), opaque crystals Odor: Odorless Density 2.13 g/cm3 Boiling Point: 1388°C / 2530°F Solubility in water: 418 g/L (0 °C)1000 g/L (25 °C)3370 g/L (100 °C) GHS Pictograms:   GHS Signal Word: Danger GHS Hazard Statements: H290, H302, H314 GHS Precautionary Statements P280, P305+P351+P338, P310 UN Identification Number: 1823 Proper Shipping Name: Sodium Hydroxide, solid Transport Hazard Class: 8 Packing Group: II DOT Placard: What Is Sodium Hydroxide? Sodium hydroxide, commonly known as lye or caustic soda, is a highly versatile and strong alkaline compound. It is represented by the chemical formula NaOH and consists of one sodium (Na+) ion, one hydrogen (H+) ion, and one hydroxide (OH-) ion. Sodium hydroxide is a white, odorless solid at room temperature and is highly soluble in water, producing a highly alkaline solution. It is widely used in various industries and applications, including manufacturing, chemical processes, cleaning agents, soap production, food processing, and more. What Is Sodium Hydroxide Used For? Sodium hydroxide (NaOH), commonly known as caustic soda or lye, has a wide range of industrial, commercial, and household uses due to its strong alkaline properties. Some of the common uses of sodium hydroxide include: Chemical Manufacturing: Sodium hydroxide is a key component in the production of various chemicals, including detergents, soaps, textiles, paper, and synthetic materials. Soap and Detergent Production: It is used in the saponification process to make soap and is also a crucial ingredient in many household and industrial cleaning products. Food Processing: Sodium hydroxide is used to process and refine certain foods, such as in the preparation of olives, cocoa, and chocolate. It is also used for peeling fruits and vegetables. Water Treatment: In water treatment, sodium hydroxide is used to adjust pH levels, remove acidity, and precipitate metals from wastewater. Petroleum Industry: It is used in refining petroleum products, including the removal of impurities from crude oil. Aluminum Production: Sodium hydroxide is employed in the extraction of alumina from bauxite ore and as an electrolyte in the aluminum extraction process. Pulp and Paper Industry: It is used in the pulping and bleaching processes of paper manufacturing. Textile Industry: Sodium hydroxide is utilized to process and dye textiles and fabrics. Pharmaceuticals: It is used in the manufacture of certain drugs and pharmaceutical products. Biodiesel Production: Sodium hydroxide is used as a catalyst in the transesterification process to produce biodiesel from vegetable oils or animal fats. Hydrogen Production: Sodium hydroxide is used to produce hydrogen gas through the electrolysis of water. Cleaning and Degreasing: It is used as a strong cleaning agent for surfaces, equipment, and industrial machinery due to its ability to dissolve oils, fats, and grease. Drain Cleaning: Sodium hydroxide-based drain cleaners are used to unclog and clean drains. pH Adjustment: In laboratories and industrial processes, sodium hydroxide is used to adjust the pH of solutions. It's important to note that sodium hydroxide is a highly caustic and reactive substance, and its use should be handled with care and appropriate safety measures. Is Sodium Hydroxide Lye? Yes, sodium hydroxide is commonly known as lye. Lye is a strong alkaline substance that is often used in various industrial, commercial, and household applications, as mentioned earlier. It is important to handle sodium hydroxide with caution, as it can cause severe burns and irritation if it comes into contact with skin or eyes. Proper safety measures should be taken when working with sodium hydroxide or lye. Are  Sodium Hydroxide and Caustic Soda The Same Thing? Yes, sodium hydroxide and caustic soda are the same thing. Caustic soda is a common name for sodium hydroxide, which is a strong alkaline chemical compound. Both terms refer to the same chemical substance with the chemical formula NaOH. It is used in various industrial, commercial, and household applications, including cleaning, manufacturing, and chemical processes. What Is Sodium Hydroxide Structure?   Sodium hydroxide (NaOH) has a simple molecular structure consisting of one sodium (Na) atom, one oxygen (O) atom, and one hydrogen (H) atom. The structure of sodium hydroxide can be visualized as follows: In this structure, the sodium atom (Na) is bonded to the oxygen atom (O) through an ionic bond, and the oxygen atom is bonded to the hydrogen atom (H) through a covalent bond. The hydroxide ion (OH-) is formed by the combination of the oxygen and hydrogen atoms, and it is the key component that gives sodium hydroxide its strong alkaline properties. What Is The pH of Sodium Hydroxide? The pH of sodium hydroxide (NaOH) is very high and strongly alkaline. Sodium hydroxide is a strong base and is commonly used to raise the pH of solutions. In its pure form, sodium hydroxide has a pH of approximately 14, which is the highest value on the pH scale. When dissolved in water, it dissociates into hydroxide ions (OH-) and sodium ions (Na+), resulting in a highly alkaline solution with a pH greater than 14. The exact pH of a sodium hydroxide solution will depend on its concentration and the amount dissolved in the solventWhat Are The Hazards of Sodium Hydroxide? Is Sodium Hydroxide A Weak or Strong Base? Sodium hydroxide (NaOH) is considered a strong base. It is highly soluble in water and dissociates completely into sodium ions (Na+) and hydroxide ions (OH-) when dissolved. This complete dissociation results in a high concentration of hydroxide ions in the solution, making sodium hydroxide a strong and effective source of hydroxide ions for chemical reactions. Strong bases like sodium hydroxide have a high tendency to accept protons (H+) from other substances, leading to the characteristic properties of strong bases, such as high alkalinity and the ability to neutralize acids.What Is Sodium Hydroxide? What Are The Hazards of Sodium Hydroxide? Sodium hydroxide (NaOH) is a caustic and highly reactive compound, and its use should be handled with care due to the following hazards: Corrosive to Skin and Tissues: Sodium hydroxide is highly corrosive and can cause severe burns upon contact with the skin, eyes, and mucous membranes. It can damage and destroy living tissue upon contact, leading to chemical burns and tissue damage. Inhalation Hazard: Inhaling sodium hydroxide dust, fumes, or mists can irritate the respiratory tract and cause coughing, shortness of breath, and lung irritation. Prolonged exposure to airborne sodium hydroxide particles can lead to more serious respiratory effects. Eye Irritation: Contact with sodium hydroxide can cause irritation, redness, and damage to the eyes. Severe exposure can lead to permanent eye damage or blindness if not promptly treated. Reactivity: Sodium hydroxide is highly reactive and can react violently with certain substances, especially acids. Mixing sodium hydroxide with acids can result in rapid heat generation, spattering, and potentially explosive reactions. Environmental Impact: Sodium hydroxide is harmful to aquatic life and can lead to water pollution if released into the environment. It is important to properly dispose of sodium hydroxide-containing solutions and prevent their release into water systems. Corrosion of Materials: Sodium hydroxide can corrode metals and other materials, causing structural damage and weakening of containers, pipes, and equipment. Toxicity: Ingesting sodium hydroxide can cause severe internal burns, damage to the digestive system, and even death. Ingestion can lead to life-threatening medical emergencies and requires immediate medical attention. To mitigate these hazards, it is essential to handle sodium hydroxide with proper protective equipment, such as gloves, goggles, and lab coats, in a well-ventilated area. Proper storage, labeling, and disposal procedures should also be followed to prevent accidents and environmental contamination. How Do I Use Sodium Hydroxide Safely? Sodium hydroxide, also known as caustic soda or lye, is a highly caustic and potentially dangerous chemical. It's essential to handle and use it safely to prevent accidents or injuries. Here are guidelines for safely using sodium hydroxide: Protective Equipment: Wear appropriate personal protective equipment (PPE), including chemical-resistant gloves, safety goggles or a full-face shield, a lab coat or chemical-resistant apron, and closed-toe shoes with chemical-resistant soles. Work in a Controlled Environment: Work in a well-ventilated area, such as a fume hood, to minimize exposure to fumes. Adequate ventilation helps disperse any fumes produced during handling. Avoid Skin Contact: In case of skin contact, immediately flush the affected area with plenty of water for at least 15 minutes. Remove contaminated clothing and seek medical attention if irritation or burns occur. Prevent Eye Contact: Wear chemical-resistant safety goggles or a full-face shield to protect your eyes from splashes. If sodium hydroxide comes into contact with your eyes, rinse them immediately with water for at least 15 minutes and seek medical attention. Use Appropriate Containers: Use containers made of materials that are compatible with sodium hydroxide, such as glass or certain types of plastic. Avoid using aluminum or reactive metals. Dilution Procedure: When diluting sodium hydroxide in water, always add the chemical to the water, not the other way around. Stir gently while adding to prevent splashing. Label Containers: Properly label containers holding sodium hydroxide solutions with appropriate hazard warnings and information. Handling Crystals or Pellets: Handle sodium hydroxide crystals or pellets with dry hands or appropriate gloves to avoid skin contact. Always use tools (e.g., scoops or spatulas) to handle solid sodium hydroxide. Do Not Inhale Fumes: Avoid inhaling sodium hydroxide fumes. Work in a well-ventilated area, and if working with large quantities or generating fumes, use a fume hood or wear a chemical-resistant mask with appropriate filters. Emergency Equipment: Have access to emergency equipment, such as eye wash stations and safety showers, in case of accidental exposure. Know the location of fire extinguishers and fire alarm systems. Spill Response: In case of a sodium hydroxide spill, follow your organization's spill response procedures. Typically, this involves containing the spill, neutralizing with an acid if appropriate, and safely cleaning it up. Storage: Store sodium hydroxide in a cool, dry, well-ventilated area, away from incompatible substances (e.g., acids, organic materials). Keep containers tightly closed when not in use. Dispose of Waste Properly: Dispose of sodium hydroxide waste in accordance with local, state, and federal regulations. It is considered hazardous waste and should be handled and disposed of as such. Training and Knowledge: Ensure that personnel working with sodium hydroxide are adequately trained in its safe handling, storage, and disposal. Training should include hazard recognition, first aid procedures, and emergency response protocols. First Aid: Familiarize yourself with the appropriate first aid measures for sodium hydroxide exposure, including how to treat skin contact, eye exposure, and ingestion. Medical Monitoring: If workers are regularly exposed to sodium hydroxide, consider implementing a medical monitoring program to track their health and detect early signs of exposure-related issues. Always follow the safety guidelines and procedures established by your organization or regulatory authorities when working with sodium hydroxide. Remember that sodium hydroxide is a highly caustic substance, and improper handling can result in severe burns or other injuries. Prioritize safety and take appropriate precautions to protect yourself and others from potential hazards associated with sodium hydroxide.

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34% Technical Industrial Grade Hydrogen Peroxide Our Technical-grade 34% peroxide tests at 34.1%.  Technical is also what is referred to as Industrial grade.  Our peroxide is clear, colorless, and free of any stabilizers or additives.  Peroxide is one of the most effective oxidizers and may be applied to food directly to food products.  Our peroxide is certified FCC (Food Chemical Codex).  It has been tested and verified for its quality and purity.  34% Food Grade Hydrogen Peroxide Certificate of Analysis 34% Food Grade Hydrogen Peroxide Safety Data Sheet Our 34% hydrogen peroxide when diluted you can make a remarkably large volume of 3% hydrogen peroxide that can be used for a wide variety of applications.   1 Quart 34% Makes 4.36 Gallons of 3% 1 Gallon 34% Makes 11.37 Gallons of 3% 5 Gallon 34% Makes 56.83 Gallons of 3% 55 Gallon 34% Makes 625.17 Gallons of 3%   Some applications include... Elevating Plant Growth: Diluted hydrogen peroxide supports healthy roots and elevated oxygen availability in the soil. Excellent Cleaner for Food Prep Environments: Hydrogen peroxide is a disinfectant, that kills viruses and various forms of bacteria. Bleaching: Diluted hydrogen peroxide is a mild bleaching agent that can be used to clean stains.  Cleansing Fresh Produce: Diluted hydrogen peroxide can be used to clean fruits and vegetables.  Mold and Mildew Removal: Hydrogen peroxides strong oxidative qualities breakdown mold and mildew with ease.  How to Dilute 34% Hydrogen Peroxide to 3% Hydrogen Peroxide: 34% food-grade hydrogen peroxide Deionized distilled water A clean, empty Gallon bottle for the final 3% hydrogen peroxide solution Measuring cup Funnel Safety goggles Rubber gloves Apron or old clothes Steps to perform dilution: Wear safety goggles, rubber gloves, an apron or old clothing to protect yourself from spills and splashes.  Choose a well-ventilated space. Mix 1 part 34.1% hydrogen peroxide with 10 parts distilled water. Example: Mix 1 cup hydrogen peroxide, with 10 cups of distilled water.  To be exact, this will make slightly more than 3% solution of hydrogen peroxide – 3.10%. What Is Hydrogen Peroxide? Hydrogen peroxide (H2O2) is a chemical compound composed of two hydrogen atoms and two oxygen atoms. It is a clear, colorless liquid with a slightly more viscous consistency than water. Hydrogen peroxide is commonly used for its powerful oxidizing properties and has a wide range of applications in various industries and household settings. What Are The Properties Of Hydrogen Peroxide? Hydrogen peroxide (H2O2) is a clear, colorless liquid with several notable properties: Chemical Formula: H2O2 - It consists of two hydrogen atoms (H) and two oxygen atoms (O) linked by a single covalent bond, as well as a second oxygen atom connected to one of the hydrogen atoms by a single covalent bond. Molecular Weight: Approximately 34.01 grams per mole. Physical State: Hydrogen peroxide is a liquid at room temperature and pressure (25°C or 77°F). Odor: It has a slightly sharp and distinctive odor. Solubility: Hydrogen peroxide is miscible (mixes completely) with water in all proportions. Density: The density of hydrogen peroxide varies with concentration. A common concentration of 3% hydrogen peroxide has a density of approximately 1.01 grams per milliliter (g/mL). Boiling Point: The boiling point of hydrogen peroxide is approximately 150.2°C (302.4°F). Melting Point: Pure hydrogen peroxide does not have a distinct melting point because it decomposes before reaching a stable liquid state at atmospheric pressure. Reactivity: Hydrogen peroxide is a powerful oxidizing agent and is highly reactive with various substances, including organic compounds and some metals. It readily decomposes into water and oxygen when exposed to heat, light, or certain catalysts. Concentration: Hydrogen peroxide is available in various concentrations, with common household solutions typically being around 3%. Higher concentrations, such as 30% or 35%, are used in industrial and laboratory applications. pH: The pH of hydrogen peroxide solutions varies with concentration but is typically slightly acidic. Stability: Hydrogen peroxide solutions are not indefinitely stable and can decompose over time, especially when exposed to light, heat, or contaminants. Storing hydrogen peroxide in a cool, dark place in a well-sealed container helps preserve its stability. Safety: Concentrated hydrogen peroxide solutions can be hazardous and should be handled with care. Contact with skin or eyes should be avoided, and protective equipment may be required when working with high-concentration solutions. These properties make hydrogen peroxide a versatile chemical with various applications in industries ranging from healthcare and cosmetics to water treatment and rocket propulsion. The concentration and handling precautions should be considered based on the specific use and requirements of the application. What Is Hydrogen Peroxide Used For? Hydrogen peroxide (H2O2) is used for a wide range of purposes in various industries and household settings due to its versatile properties. Some common uses of hydrogen peroxide include: Disinfectant and Antiseptic: Hydrogen peroxide is a common disinfectant and antiseptic agent. It is used to clean wounds, cuts, and minor injuries to prevent infection. In lower concentrations (typically 3%), it can be safely applied to the skin. Hair Bleaching and Dyeing: Many hair bleaching and hair dyeing products contain hydrogen peroxide as it can help break down the natural pigments in hair, lightening its color. Teeth Whitening: Hydrogen peroxide is used in some teeth whitening products and dental treatments to remove stains and discoloration from teeth. Cleaning Agent: It is used as a cleaning agent for surfaces, fabrics, and contact lenses due to its ability to break down and remove organic stains and deposits. Water Treatment: In water treatment processes, hydrogen peroxide can be used to remove contaminants, oxidize organic matter, and disinfect water supplies. Rocket Propellant: In the aerospace industry, highly concentrated hydrogen peroxide (usually around 90% purity) is used as a rocket propellant. Chemical Synthesis: Hydrogen peroxide is used in the synthesis of various chemicals and pharmaceuticals. Environmental Applications: It can be employed for soil and groundwater remediation, helping to break down pollutants and contaminants. Food Industry: In the food industry, hydrogen peroxide can be used for cleaning and disinfection of equipment and packaging materials. Cosmetics: It is used in some cosmetic and personal care products, such as hair dyes, hair bleaches, and skin creams. Textiles: Hydrogen peroxide is used in the textile industry to bleach fabrics and remove stains. Paper and Pulp Industry: It is used for bleaching paper pulp and improving the quality of paper products. Agriculture: In agriculture, hydrogen peroxide can be used as an oxygen source in soil, promoting plant growth. Medical and Laboratory Use: It is utilized for cleaning and sterilizing medical equipment and laboratory instruments. First Aid: Hydrogen peroxide is a household item for treating minor cuts and scrapes. The specific application and concentration of hydrogen peroxide used can vary depending on the intended purpose. Higher concentrations are typically used in industrial and chemical applications, while lower concentrations are common in household and personal care products. It's important to handle hydrogen peroxide with care, follow safety guidelines, and use the appropriate concentration for a given task. How Is Hydrogen Peroxide Produced? Hydrogen peroxide (H2O2) is typically produced through one of two main methods: the anthraquinone process and the direct synthesis process. Both processes involve the reaction of hydrogen and oxygen in the presence of a catalyst to form hydrogen peroxide. Here's an overview of these two methods: Anthraquinone Process: This is the most common method for commercial hydrogen peroxide production. It involves a series of chemical reactions that use anthraquinone derivatives as catalysts. The process typically consists of the following steps: Hydrogenation: Anthraquinone derivatives are hydrogenated with hydrogen gas (H2) to form hydroquinone derivatives. Autoxidation: The hydroquinone derivatives react with oxygen (O2) to form anthraquinone derivatives again, while producing hydrogen peroxide in the process. Extraction: The hydrogen peroxide is then extracted from the reaction mixture. Oxidation of Anthraquinone: The anthraquinone derivatives are oxidized back to their original form for reuse in the process. Direct Synthesis Process: In this method, hydrogen and oxygen are directly combined to produce hydrogen peroxide using a catalyst. The reaction typically occurs in a gas-phase reactor, and the process is often referred to as the "direct synthesis" or "hydrogenation-oxygenation" process. Common catalysts used in this process include palladium or platinum on a support material. While these are the main methods for hydrogen peroxide production, there are other less common methods as well. The choice of production method depends on factors such as the desired concentration of hydrogen peroxide, production scale, and cost considerations. It's worth noting that hydrogen peroxide is a sensitive compound and can decompose over time, especially when exposed to heat, light, or contaminants. Therefore, it requires careful handling and storage to maintain its stability and effectiveness. Does Hydrogen Peroxide Expire? Hydrogen peroxide can degrade over time and may lose its effectiveness, so it can be said to have a shelf life rather than a strict expiration date. The shelf life of hydrogen peroxide depends on several factors, including its concentration, exposure to light, temperature, and how well it's stored. Here are some general guidelines: Concentration: Higher concentrations of hydrogen peroxide (e.g., 30% or 35%) tend to be more stable and have a longer shelf life compared to lower concentrations (e.g., 3% or 6%). Exposure to Light: Hydrogen peroxide is light-sensitive, and exposure to ultraviolet (UV) light can accelerate its decomposition. It is typically sold in brown or opaque containers to protect it from light. Temperature: Storage at higher temperatures can also speed up the decomposition of hydrogen peroxide. It should be stored at a cool, dry place away from heat sources. Contaminants: Contaminants or impurities can catalyze the decomposition of hydrogen peroxide. It's essential to keep the container tightly sealed and free from any potential contaminants. Age: Hydrogen peroxide degrades slowly over time, even when stored correctly. The rate of degradation is higher for lower concentrations. To maximize the shelf life and potency of hydrogen peroxide, follow these recommendations: Store it in its original, tightly sealed container. Keep it in a cool, dark place away from direct sunlight and heat sources. Check the expiration date on the container, if available. If you're unsure about the potency of an old bottle of hydrogen peroxide, consider testing it on a small, non-critical area before using it for medical or cleaning purposes. It's important to note that even if hydrogen peroxide has degraded, it may still be useful for some applications, such as cleaning and disinfecting surfaces. However, for medical or first-aid use, it's best to use hydrogen peroxide that is within its recommended shelf life to ensure its effectiveness. Is Hydrogen Peroxide Safe As Mouthwash? Hydrogen peroxide can be used as a mouthwash, but it should be used with caution and in a diluted form. Here are some important considerations: Dilution: Never use undiluted hydrogen peroxide as a mouthwash. It's too concentrated at its full strength and can cause irritation, burning, and tissue damage. Instead, dilute it with water. A common recommendation is to use a 3% hydrogen peroxide solution, which is typically sold in drugstores. Frequency: Do not use hydrogen peroxide as a mouthwash too frequently. Using it daily or excessively can lead to oral issues, including irritation and disruption of the natural balance of oral bacteria. Duration: When using hydrogen peroxide as a mouthwash, swish it around your mouth for a brief period, typically about 30 seconds, and then spit it out. Do not swallow it. Rinse Thoroughly: After using hydrogen peroxide as a mouthwash, rinse your mouth thoroughly with water to remove any residual hydrogen peroxide. Avoid Ingestion: Do not swallow hydrogen peroxide, even when diluted. Swallowing hydrogen peroxide can lead to stomach upset and other health issues. Consultation: Before using hydrogen peroxide as a mouthwash, it's a good idea to consult with your dentist or oral healthcare provider. They can provide guidance on its safe and appropriate use based on your specific oral health needs. Hydrogen peroxide can help kill harmful bacteria in the mouth and may be used as a short-term remedy for issues like canker sores or minor gum irritations. However, it is not a substitute for regular oral hygiene practices such as brushing, flossing, and using a fluoride-based mouthwash. If you experience any adverse reactions, such as severe irritation, burning, or pain, discontinue use immediately and consult a healthcare professional. It's important to use hydrogen peroxide as a mouthwash cautiously and in accordance with recommended guidelines to avoid potential side effects or harm to oral tissues. What Are The Hazards Of Hydrogen Peroxide? Hydrogen peroxide, while commonly used for various purposes, can pose certain hazards if mishandled or used improperly. Here are some of the potential hazards associated with hydrogen peroxide: Irritation and Burns: Hydrogen peroxide is a strong oxidizing agent and can cause skin and eye irritation upon contact. In higher concentrations or with prolonged exposure, it can lead to chemical burns. Ingestion: Ingesting concentrated hydrogen peroxide can be harmful and even life-threatening. It can cause gastrointestinal irritation, stomach pain, vomiting, and, in severe cases, internal burns or damage. Inhalation: Inhalation of hydrogen peroxide vapors can irritate the respiratory tract, leading to coughing, shortness of breath, and throat irritation. Explosive Hazards: Concentrated hydrogen peroxide solutions can be sensitive to shock, heat, or contamination with organic materials. This can lead to the potential for explosions or fires if mishandled. Skin Sensitization: Prolonged or repeated contact with hydrogen peroxide can lead to skin sensitization, where the skin becomes more sensitive or allergic to the chemical. Environmental Impact: Hydrogen peroxide can be harmful to aquatic life and the environment if not properly disposed of. It should not be released into natural waterways. hydrogen peroxide, consider the following precautions: Dilution: When using hydrogen peroxide, dilute it to the appropriate concentration for the intended purpose. Most household hydrogen peroxide solutions are 3%, while higher concentrations are used for industrial or medical applications. Protective Equipment: When handling concentrated hydrogen peroxide, wear appropriate personal protective equipment, including gloves and safety goggles. Ventilation: Use hydrogen peroxide in well-ventilated areas to minimize inhalation risks. First Aid: In case of skin or eye contact, rinse immediately with plenty of water. If ingested, seek medical attention. Storage: Store hydrogen peroxide in a cool, dark place away from flammable materials and heat sources. Dispose Properly: Dispose of hydrogen peroxide in accordance with local regulations. Do not pour it down drains or release it into the environment. Always follow the safety guidelines and instructions provided on the product label or by the manufacturer. If you have specific concerns or questions about handling hydrogen peroxide for a particular application, it's advisable to consult with a safety professional or chemical expert for guidance. How Can I Use Hydrogen Peroxide Safely? Using hydrogen peroxide safely involves taking appropriate precautions to minimize the risk of accidents or harm. Here are some guidelines for safe handling and use of hydrogen peroxide: Read the Label: Always read and follow the instructions and safety precautions provided on the hydrogen peroxide product label. Different concentrations may have different recommended uses and safety guidelines. Personal Protective Equipment (PPE): Wear appropriate personal protective equipment, including safety goggles or a face shield to protect your eyes. Use gloves made of materials that are compatible with hydrogen peroxide, such as nitrile or latex gloves. Ventilation: Use hydrogen peroxide in a well-ventilated area to minimize exposure to vapors. If you're using it in a confined space, consider using a fume hood or working near an open window or door. Concentration: Ensure that you are using the correct concentration of hydrogen peroxide for your specific application. Most household hydrogen peroxide solutions are typically 3%, but higher concentrations are available for industrial or medical use. Dilution: When diluting concentrated hydrogen peroxide, always add the hydrogen peroxide to water, not the other way around. This helps prevent splattering and potential reactions. Avoid Contaminants: Keep hydrogen peroxide away from organic materials (e.g., paper, cloth) and flammable substances, as it can react with them and potentially cause fires or explosions. Avoid Mixing: Do not mix hydrogen peroxide with other chemicals unless you are following a specific recipe or procedure that requires it. Mixing hydrogen peroxide with certain substances can be dangerous. First Aid: In case of skin contact, immediately rinse the affected area with plenty of water. If hydrogen peroxide comes into contact with your eyes, flush them with water for at least 15 minutes and seek medical attention if irritation persists. If ingested, do not induce vomiting. Seek medical attention immediately. Storage: Store hydrogen peroxide in a cool, dark place, away from direct sunlight and heat sources. Keep the container tightly closed when not in use. Disposal: Dispose of hydrogen peroxide in accordance with local regulations. Do not pour it down drains or release it into the environment. Emergency Response: Have access to an emergency eyewash station and safety shower if you are working with concentrated hydrogen peroxide. Keep a spill kit and appropriate cleanup materials on hand in case of accidents. Training: Ensure that individuals handling hydrogen peroxide are trained in its safe use and understand the potential hazards. If you are unsure about how to use hydrogen peroxide safely for a specific application, consider seeking guidance from a safety professional or chemical expert. Always exercise caution and pr

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BVV™ Food & Lab Grade Glacial Acetic Acid 99.8% pH: 2.4 Looking for a food-grade acid for your acid-base extraction? Our premium Glacial Acetic Acid is precisely what you need! As a leading supplier of high-purity solvents & chemicals, we provide the purest Glacial Acetic Acid available for your acid-base extraction and pH adjustment needs, ensuring exceptional results every time. Acetic acid, also known as ethanoic acid, is a versatile organic compound that plays a significant role in various industries and everyday life. It is a colorless liquid with a pungent, vinegar-like odor. Acetic acid  (CH3COOH) is a weak acid that is highly soluble in water and many organic solvents. Due to its unique properties, acetic acid is widely used as a solvent, preservative, and flavoring agent in the food and beverage industry. It is also a key component in the production of vinyl acetate, which is used in the manufacturing of adhesives, coatings, and textiles. Furthermore, acetic acid is utilized in the synthesis of numerous chemicals, including pharmaceuticals, dyes, and plastics. Its diverse range of applications makes acetic acid an essential compound in many industrial processes, where it contributes to the creation of countless products that we encounter in our daily lives. Glacial Acetic Acid, also known as ethanoic acid, is a highly concentrated and pure form of acetic acid.  Its name, "glacial," refers to its ability to freeze at a relatively low temperature (16.6C/61.9F). This characteristic sets it apart from other forms of acetic acid, making it ideal for various industrial applications, including acid-base extraction. Our Glacial Acetic Acid contains less than 1% water and is also considered water-free anhydrous acetic acid.   In acid-base extraction, Glacial Acetic Acid serves as an essential component due to its unique properties. It acts as a weak acid, enabling the extraction of alkaline compounds from organic mixtures. With our premium Glacial Acetic Acid, you can achieve efficient separation of target compounds by adjusting the pH and facilitating the formation of soluble salts. In addition to its use in acid-base extraction, our Glacial Acetic Acid finds widespread application in various industries, including pharmaceuticals, textiles, and food processing. It is also known for its ability to dissolve and remove mineral deposits, making it an excellent choice for descaling and cleaning applications. At BVV, we take pride in delivering premium solvents, chemicals, and adsorbents that exceed customer expectations. Our team of experts is always available to provide personalized support and guidance, ensuring that you find the right solution for your needs. With our high-purity Glacial Acetic Acid & Sodium Hydroxide, you can optimize your acid-base extraction processes and pH adjustment needs to achieve exceptional results. Ready to elevate your acid-base extraction procedures? Order our High Purity Glacial Acetic Acid & Sodium Hydroxide today and experience its superior quality and performance firsthand. Contact us now to learn more and take advantage of our competitive prices and prompt delivery. Unlock the potential of your acid-base extractions with BVV!   Flashpoint: 102°F Molecular Formula: C2H4O2 CAS No.: 64-19-7 UN 2789 Freezing Point: 16.6°C (61.9°F) Boiling Point: 117.9°C (244.2°F) Density: 1.05 g/cm3 @ 25°C (77°F) Water Solubility: 602.9 g/l completely Soluble @ 25°C (77°F) Acetic Acid Glacial 99.8% Certificate of Analysis (COA) Acetic Acid Glacial 99.8% Safety Data Sheet (SDS) Chemical Formula: CH3COOH Molecular Weight: 60.052 g·mol−1 CAS Registry Number: 64-19-7 Appearance Colorless, transparent liquid,  Odor: Heavily vinegar-like Density 1.049 g/cm3 (liquid); 1.27 g/cm3 (solid) Boiling Point: 16 °C / 61°F GHS Pictograms: GHS Signal Word: Danger GHS Hazard Statements: H226, H314 GHS Precautionary Statements P280, P305+P351+P338, P310 UN Identification Number: 2789 Proper Shipping Name: Acetic Acid, Glacial Transport Hazard Class: 8 Packing Group: II DOT Placard: What is Acetic Acid? Acetic acid, also known as ethanoic acid, is a colorless liquid organic compound with a distinct sour taste and pungent smell. It is a member of the carboxylic acid family and is classified as a weak acid due to its partial ionization in aqueous solutions. Acetic acid is a fundamental building block in various chemical reactions and is commonly found in vinegar, giving it its characteristic sour taste. Chemically represented as CH3COOH, acetic acid consists of two main components: a carboxyl group (-COOH) and a methyl group (-CH3). It is produced naturally through fermentation processes, where bacteria convert ethanol into acetic acid. Additionally, acetic acid can be synthesized through various chemical methods for industrial applications. Acetic acid is widely utilized in various industries, including food, pharmaceuticals, textiles, and chemicals. It serves as a crucial ingredient in the production of plastics, solvents, dyes, and synthetic fibers. Its versatile nature makes it an essential component in countless products and processes, contributing to a wide range of applications across different sectors. What Is Acetic Acids Formula? Chemically represented as CH3COOH, acetic acid consists of two main components: a carboxyl group (-COOH) and a methyl group (-CH3). It is produced naturally through fermentation processes, where bacteria convert ethanol into acetic acid. Additionally, acetic acid can be synthesized through various chemical methods for industrial applications. What is Acetic Acids Structure? The structure of acetic acid consists of two carbon atoms (C), four hydrogen atoms (H), and two oxygen atoms (O) arranged in a specific pattern. It forms a molecule with a central carbon atom bonded to two oxygen atoms: one oxygen atom is double-bonded to the carbon (C=O) and the other is bonded via a single bond (C-OH). This arrangement creates a carboxyl group (COOH) at one end of the molecule. The remaining carbon and hydrogen atoms are bonded in a linear chain, resulting in the overall molecular structure of CH3COOH. What Is Acetic Acids Molar Mass? The molar mass of a chemical compound is a measure of the mass of one mole of that substance, expressed in grams per mole (g/mol). For acetic acid (CH3COOH), which is a simple organic compound, the molar mass is calculated by adding up the atomic masses of all the individual atoms in its chemical formula. Let's break down the components of acetic acid: Carbon (C) - Atomic mass: 12.01 g/mol Hydrogen (H) - Atomic mass: 1.01 g/mol (there are 2 hydrogen atoms) Oxygen (O) - Atomic mass: 16.00 g/mol (there are 2 oxygen atoms) Another Oxygen (O) - Atomic mass: 16.00 g/mol Hydrogen (H) - Atomic mass: 1.01 g/mol (there is 1 hydrogen atom) Now, add up the atomic masses: 12.01 g/mol (C) + 1.01 g/mol (H) + 1.01 g/mol (H) + 16.00 g/mol (O) + 16.00 g/mol (O) + 1.01 g/mol (H) = 60.05 g/mol Therefore, the molar mass of acetic acid is approximately 60.05 g/mol. This value is crucial for various chemical calculations and reactions involving acetic acid, including determining quantities in chemical reactions or preparing solutions with specific concentrations. What is the PKA of Acetic Acid? The pKa of acetic acid (CH3COOH) is approximately 4.75. The pKa value represents the acidity of a compound and indicates the strength of its dissociation in aqueous solution. Acetic acid is a weak acid, meaning that it does not completely dissociate into ions in water and has a relatively low tendency to donate protons (H+ ions). Is Acetic Acid A Weak or Strong Acid? Acetic acid (CH3COOH) is considered a weak acid. Weak acids are substances that only partially dissociate into ions when dissolved in water. In the case of acetic acid, it releases a limited number of hydrogen ions (H+) and acetate ions (CH3COO-) in water. This is in contrast to strong acids, which completely dissociate into ions and release a higher concentration of hydrogen ions in solution. What Is The Boiling Point of Acetic Acid? The boiling point of acetic acid is approximately 118.1 degrees Celsius (244.5 degrees Fahrenheit) at standard atmospheric pressure. However, this value can vary slightly depending on factors such as atmospheric pressure and impurities present in the acetic acid. What Is The Density of Acetic Acid? The density of acetic acid is approximately 1.049 grams per cubic centimeter (g/cm³) at 20 degrees Celsius (68 degrees Fahrenheit). Keep in mind that the density of acetic acid can vary slightly with temperature and concentration. What Is Glacial Acetic Acid? Glacial acetic acid, also known as anhydrous acetic acid, is a highly concentrated and pure form of acetic acid. The term "glacial" is used to describe its appearance, as it solidifies into ice-like crystals at room temperature due to its high freezing point. Glacial acetic acid typically has a concentration of around 99-100%, making it one of the purest forms of acetic acid available. This highly concentrated form of acetic acid is commonly used in various industrial, laboratory, and chemical applications. It is often utilized as a solvent, reagent, or catalyst in chemical reactions, as well as in the production of various chemicals, plastics, textiles, and pharmaceuticals. Glacial acetic acid's high purity and reactivity make it a valuable component in many manufacturing processes and scientific experiments. It's important to handle glacial acetic acid with care due to its corrosive and strong acidic properties. Proper safety precautions should be taken when working with this substance, including using appropriate protective equipment and following recommended handling procedures. What Is Acetic Acid Used For? Acetic acid is a versatile chemical compound with a wide range of applications across various industries. Here are some common uses of acetic acid: Food and Beverage Industry: Acetic acid is a key component in the production of vinegar, which is used as a condiment, flavor enhancer, and food preservative. It is also used in the production of pickles, sauces, and dressings. Chemical Industry: Acetic acid is used as a chemical intermediate in the production of various chemicals, including acetate esters, acetic anhydride, and vinyl acetate monomer. These chemicals are used in the manufacturing of plastics, synthetic fibers, dyes, and pharmaceuticals. Cleaning and Disinfecting: Acetic acid is commonly used as an environmentally friendly cleaning agent due to its mild acidity and disinfectant properties. It can effectively remove mineral deposits, stains, and mold from surfaces. Textile Industry: Acetic acid is used in the production of acetate fibers, which are used to make fabrics, textiles, and clothing items. It is also employed in dyeing and finishing processes. Photography: Acetic acid is used in photographic processes, including film development and as a fixing agent for prints. Preservation: Acetic acid is used to preserve and prevent spoilage in various agricultural products, such as fruits and vegetables. Laboratory and Research: Acetic acid is commonly used in laboratories for various purposes, including chemical analysis, pH adjustment, and buffer preparation. Medicine and Pharmaceuticals: Acetic acid is used in the synthesis of pharmaceutical compounds and as a solvent for certain medications and ointments. Wastewater Treatment: Acetic acid is used in wastewater treatment processes to adjust pH levels and promote the growth of beneficial microorganisms. Tanning Industry: Acetic acid is used in leather tanning processes to adjust the pH of the solutions and aid in the removal of unwanted substances. Plastics and Polymers: Acetic acid is a precursor in the production of polyvinyl acetate (PVA) and other polymer materials used in adhesives, coatings, and paints. Oil and Gas Industry: Acetic acid is employed in the oil and gas industry for processes such as well drilling, acidizing, and corrosion inhibition. Electronics Industry: Acetic acid is used for cleaning and etching electronic components and printed circuit boards. These are just a few examples of the diverse applications of acetic acid. Its chemical properties make it a valuable ingredient in numerous industrial and consumer products, contributing to various processes and sectors. What Are The Hazards of Acetic Acid? Acetic acid is generally considered safe when used properly and handled with care. However, like any chemical compound, it can pose certain hazards if not used and managed correctly. Here are some potential hazards associated with acetic acid: Corrosive Nature: Acetic acid is a corrosive substance, and concentrated solutions can cause severe irritation or burns to the skin, eyes, and respiratory tract upon direct contact. Prolonged exposure to the skin or eyes can result in chemical burns and tissue damage. Inhalation Risks: Inhaling acetic acid vapors or mists can irritate the respiratory system, causing symptoms such as coughing, shortness of breath, and throat irritation. Prolonged or intense exposure to vapors can lead to more severe respiratory effects. Fire and Explosion Hazard: Acetic acid is flammable, with a low flashpoint. Concentrated vapors or mists can ignite and potentially cause fires or explosions when exposed to an open flame, spark, or heat source. Incompatibility: Acetic acid may react with certain chemicals and substances, resulting in potentially hazardous reactions or releases of toxic gases. Proper storage and handling procedures are essential to prevent such interactions. Toxicity: Ingesting or consuming concentrated acetic acid can lead to serious health issues, including chemical burns in the digestive tract, internal injuries, and other toxic effects. Ingestion should be avoided. Environmental Impact: Improper disposal or release of acetic acid into the environment can harm aquatic life and ecosystems. It can also contribute to air pollution when released into the atmosphere. Sensitization: Prolonged or repeated exposure to acetic acid can lead to sensitization, where an individual becomes more susceptible to adverse effects upon subsequent exposures. To mitigate these hazards and ensure safe handling of acetic acid, it's important to follow proper safety guidelines and precautions How Do I Use Glacial Acetic Acid Safely? Using glacial acetic acid safely is essential due to its corrosive and strong acidic properties. Follow these guidelines to ensure safe handling and use: Personal Protective Equipment (PPE): Wear appropriate PPE, including chemical-resistant gloves, safety goggles, a lab coat or protective clothing, and closed-toe shoes to prevent contact with the skin, eyes, and clothing. Well-Ventilated Area: Work in a well-ventilated area or use a fume hood to minimize inhalation exposure. Ensure proper ventilation to prevent the buildup of fumes. Avoid Contact: Avoid direct skin contact with glacial acetic acid. In case of accidental skin contact, immediately rinse the affected area with copious amounts of water and seek medical attention if irritation persists. Eye Protection: Wear safety goggles or a face shield to protect your eyes from potential splashes or fumes. In case of eye contact, rinse the eyes thoroughly with water and seek immediate medical assistance. Handling and Pouring: When handling glacial acetic acid, use chemical-resistant containers and utensils. Pour slowly to avoid splashing and minimize the release of fumes. Always use a chemical-resistant funnel for transferring the acid. Dilution: If dilution is required, always add glacial acetic acid to water, never the other way around. Adding water to the acid can cause a violent reaction. Storage: Store glacial acetic acid in a cool, dry, and well-ventilated area, away from direct sunlight and incompatible substances. Ensure proper labeling of containers and keep them tightly sealed to prevent evaporation and fume release. First Aid: Have an eyewash station and safety shower readily accessible in case of accidental exposure. Know the location of emergency exits and procedures. Emergency Response: In case of spills or leaks, contain and absorb the acid using appropriate absorbent materials. Neutralize any spilled acid with a suitable neutralizing agent under proper ventilation. Dispose of contaminated materials as hazardous waste. Training: Ensure that personnel handling glacial acetic acid are trained in its proper handling, storage, and emergency response procedures. Regularly review safety protocols. Medical Attention: If you experience skin contact, eye exposure, or inhalation of fumes, seek medical attention immediately. Provide medical professionals with accurate information about the substance involved. Always refer to the Material Safety Data Sheet (MSDS) or Safety Data Sheet (SDS) provided by the manufacturer for specific safety information and handling guidelines for the glacial acetic acid product you are using. Following proper safety protocols and practices is crucial to prevent accidents and ensure the well-being of individuals working with glacial acetic acid.

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Hydrochloric Acid 37% ACS Reagent Grade HCL pH: 1.1 Hydrochloric acid, solution is a colorless watery liquid with a sharp, irritating odor. Consists of hydrogen chloride, a gas, dissolved in water. Sinks and mixes with water.  HCL vapors are heavier than air.  It is classified as a Strong Acid and is used in many types of laboratory preparations.     Chemical Formula: HCl Molecular Weight: 36.46 CAS Registry Number:  7647-01-0 Appearance Colorless, transparent liquid, fumes in air if concentrated Odor: Pungent characteristic Density 0.81 g/cm3 Boiling Point: 61C @ 36% Concentration GHS Pictograms: GHS Signal Word: Danger GHS Hazard Statements: H290, H314, H335 GHS Precautionary Statements P210, P233, P240, P305+P351+P338, P403+P23 P260, P280, P303+P361+P353, P305+P351+P338 UN Identification Number: 1789 Proper Shipping Name: Hydrochloric acid solution Transport Hazard Class: 8 Packing Group: II DOT Placard:    What Is Hydrochloric Acid? Hydrochloric acid (HCl) is a strong, highly corrosive acid that is widely used in various industrial, commercial, and laboratory applications. It is a solution of hydrogen chloride gas dissolved in water, forming a clear, colorless liquid with a sharp, pungent odor. Chemically, hydrochloric acid is composed of hydrogen (H) and chlorine (Cl) atoms, with a chemical formula of HCl. In aqueous solution, hydrochloric acid dissociates into hydrogen ions (H⁺) and chloride ions (Cl⁻), making it a strong acid. How Is Hydrochloric Acid Produced? Hydrochloric acid (HCl) is typically produced on an industrial scale through the chemical reaction between hydrogen gas (H2) and chlorine gas (Cl2). This reaction is exothermic and requires the presence of a suitable catalyst to proceed efficiently. The primary method for producing hydrochloric acid involves the following steps: Preparation of Hydrogen: Hydrogen gas (H2) is produced through various methods, such as steam reforming of natural gas (methane), electrolysis of water, or as a byproduct of certain chemical processes. Steam reforming is the most common method for large-scale hydrogen production, where methane is reacted with steam in the presence of a nickel-based catalyst to produce hydrogen gas and carbon monoxide: CH4 + H2O → CO + 3H2 The produced hydrogen gas is then purified to remove impurities before use in the hydrochloric acid production process. Preparation of Chlorine: Chlorine gas (Cl2) is typically produced by the electrolysis of sodium chloride (table salt) solution, known as the chlor-alkali process. In this process, an electric current is passed through a brine solution (sodium chloride dissolved in water), resulting in the decomposition of water and the formation of chlorine gas at the anode: 2Cl⁻ → Cl2 + 2e⁻ The chlorine gas is then purified and dried to remove any water vapor before use in the hydrochloric acid production process. Hydrogen-Chlorine Reaction: Once hydrogen and chlorine gases are prepared, they are combined and reacted in a controlled manner. The reaction typically occurs in a reactor vessel equipped with a suitable catalyst, such as platinum or rhodium, to facilitate the reaction: H2 + Cl2 → 2HCl This reaction produces hydrochloric acid gas (HCl), which is then cooled and condensed to form a liquid solution of hydrochloric acid. Dissolution in Water: The hydrochloric acid gas is dissolved in water to produce a concentrated solution of hydrochloric acid. This solution can be further diluted to the desired concentration for various industrial, commercial, or laboratory applications. Overall, the production of hydrochloric acid involves the controlled reaction of hydrogen and chlorine gases in the presence of a catalyst, followed by the dissolution of the resulting hydrochloric acid gas in water. The process is typically carried out in specialized chemical plants equipped with the necessary infrastructure and safety measures to handle corrosive and hazardous materials. What Is Hydrochloric Acid Used for? Hydrochloric acid (HCl) is a versatile and widely used chemical with numerous industrial, commercial, and laboratory applications. Some common uses of hydrochloric acid include: Chemical Manufacturing: Hydrochloric acid is used in the production of a wide range of chemicals, including chlorine, vinyl chloride (used to make PVC), and various pharmaceuticals, dyes, and pigments. Steel Pickling: Hydrochloric acid is commonly used for pickling or cleaning steel surfaces to remove rust, scale, and other impurities before further processing, such as galvanizing or coating. pH Control: Hydrochloric acid is used as a pH adjuster or neutralizer in various industrial processes, wastewater treatment, and swimming pool maintenance. Food Processing: Hydrochloric acid is used in the food industry for various purposes, including adjusting acidity, flavor enhancement, and food preservation (in accordance with regulatory guidelines). Laboratory Applications: Hydrochloric acid is commonly used in laboratories for chemical analysis, titrations, and as a reagent in various chemical reactions. Household Cleaning Products: Dilute hydrochloric acid solutions are used in household cleaning products, such as toilet bowl cleaners and descaling agents. Oil and Gas Production: Hydrochloric acid is used in the oil and gas industry for various applications, including well acidization to enhance the productivity of oil and gas wells. Water Treatment: Hydrochloric acid is used in water treatment processes to control pH, remove mineral scale deposits, and neutralize alkaline substances. Textile and Leather Processing: Hydrochloric acid is used in textile and leather processing industries for desizing, bleaching, and pH adjustment. Metal Cleaning and Etching: Hydrochloric acid is used for cleaning and etching metals, such as aluminum, copper, and brass, in various manufacturing processes. Chemical Synthesis: Hydrochloric acid is used as a reactant or catalyst in various chemical synthesis processes, including the production of pharmaceuticals, plastics, and synthetic rubber. These are just a few examples of the diverse range of applications for hydrochloric acid. Its versatility, corrosive properties, and ability to adjust pH make it an essential chemical in many industries and processes. However, it's important to handle hydrochloric acid with care due to its corrosive nature and potential health hazards. Proper safety precautions, such as wearing protective equipment and following appropriate handling and storage procedures, should be observed when working with hydrochloric acid. What Are The Hazards of Hydrochloric Acid? Hydrochloric acid (HCl) is a highly corrosive and hazardous chemical that can pose several risks to human health, safety, and the environment. Some of the main hazards associated with hydrochloric acid include: Corrosive Properties: Hydrochloric acid is highly corrosive to skin, eyes, respiratory tract, and mucous membranes. Contact with concentrated hydrochloric acid can cause severe chemical burns, irritation, and tissue damage. Inhalation of hydrochloric acid vapors or mists can also cause irritation and damage to the respiratory system. Acute Toxicity: Exposure to high concentrations of hydrochloric acid vapor or mist can cause acute toxicity, leading to symptoms such as coughing, difficulty breathing, chest pain, and throat irritation. Severe exposure may result in pulmonary edema (fluid buildup in the lungs) and respiratory distress. Environmental Hazards: Spills or releases of hydrochloric acid can have adverse effects on the environment, including contamination of soil, water bodies, and aquatic ecosystems. Hydrochloric acid can be corrosive to metals and may cause damage to infrastructure and equipment if not properly contained and managed. Reactivity: Hydrochloric acid is reactive with a wide range of substances, including metals, alkalis, and organic materials. It can release hazardous gases (such as hydrogen gas) when reacting with certain metals, posing fire and explosion hazards in confined spaces. Storage and Handling Risks: Hydrochloric acid must be stored and handled with care due to its corrosive and reactive nature. Improper storage, handling, or mixing with incompatible substances can lead to accidents, spills, and exposure incidents. Health Effects: Prolonged or repeated exposure to hydrochloric acid vapor or mist may cause chronic respiratory effects, such as bronchitis, asthma, or chronic obstructive pulmonary disease (COPD). Individuals with pre-existing respiratory conditions or sensitivities may be more susceptible to the effects of hydrochloric acid exposure. Skin and Eye Damage: Contact with hydrochloric acid can cause severe chemical burns and damage to the skin and eyes. Eye contact may result in irritation, redness, and blurred vision, while skin contact may cause pain, redness, and blistering. Ingestion Hazards: Ingestion of hydrochloric acid can cause severe burns to the mouth, throat, esophagus, and stomach, leading to tissue damage, perforation, and internal bleeding. Ingestion of even small amounts of concentrated hydrochloric acid can be life-threatening and requires immediate medical attention. Overall, the hazards associated with hydrochloric acid underscore the importance of proper handling, storage, and use of this chemical in industrial, commercial, and laboratory settings. Employers and workers should be trained on the safe handling procedures, use of personal protective equipment, and emergency response protocols to minimize the risks associated with hydrochloric acid exposure. Additionally, regulatory guidelines and safety standards should be followed to ensure compliance and protect human health and the environment.

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