Laboratory Acids

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1. Purpose: Nitric acid is used as a common laboratory reagent and an important industrial chemical.
2. Composition: It has the chemical formula HNO₃.
3. Appearance: Nitric acid is a colorless liquid, but samples tend to acquire a yellow cast over time due to decomposition into oxides of nitrogen.
4. Concentration: Most commercially available nitric acid has a concentration of 68% in water.
5. Forms:
   • Fuming Nitric Acid: Refers to solutions with more than 86% HNO₃. It can be further characterized as red fuming nitric acid (above 86%) or white fuming nitric acid (above 95%).

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• Chemical Formula: Sulfuric acid has the formula H₂SO₄.
• Appearance: It is a colorless, odorless, and viscous liquid.
• Uses:
  • Industrial: Widely used in various industries, including fertilizers, batteries, and metallurgy.
  • Dehydrating Agent: At higher concentrations, it acts as a dehydrating agent.
  • Oxidizing Agent: Also functions as an oxidizing agent.
• Hazards: Extremely corrosive and should be handled with care

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• Chemical Name: Sulphuric acid (H₂SO₄)
• CAS Number: 7664-93-9
• Molar Mass: 98.08 g/mol
• Appearance: Clear, colorless to brown liquid
• Common Uses:
  • Used in battery manufacturing (lead-acid batteries)
  • Essential in industrial processes (e.g., fertilizer production, petroleum refining)
  • Diluted forms used as drain cleaners
  • Catalyst in chemical reactions
• Physical Properties:
  • Density: 1.84 g/cm³ (concentrated)
  • Boiling Point: 337 °C (concentrated)
  • Solubility: Miscible with water
  • Odor: Pungent and acrid
• Safety Information:
  • Hazard Class: Corrosive (Category 1)
  • Eye Damage/Irritation: Category 1
  • Skin Corrosion/Irritation: Category 1A
  • Storage: Store in a cool, well-ventilated area away from incompatible materials

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1. Structure and Properties:

   • Sodium hydroxide is a white, translucent crystalline solid.
   • It is highly corrosive and can cause severe skin burns and irritation to the eyes and other body parts.
   • The compound absorbs moisture from the air.
   • It is highly soluble in water and consists of sodium cations (Na⁺) and hydroxide anions (OH⁻).
   • Sodium hydroxide generates a high level of heat and should always be created by mixing the compound into water, not vice versa.

2. Uses:

   • Soap and Detergent Production: Sodium hydroxide reacts with fats and oils in a process called saponification, creating soap. It transforms triglycerides into glycerol and fatty acid salts, which act as cleansing agents in soaps and detergents.
   • Bleach Production: It is used in the production of bleach (chlorine).
   • Drain Cleaners: Sodium hydroxide is an ingredient in drain cleaners.
   • Water Treatment: Municipal water treatment facilities use it to remove heavy metals from water.
   • Food Preservatives: It prevents bacteria and mold growth in food.
   • Papermaking and Recycling: Sodium hydroxide is used in papermaking and paper recycling processes.

3. Health Hazards:

   • Sodium hydroxide is highly corrosive and can cause chemical burns.
   • It decomposes proteins at room temperature.
   • Safety precautions are essential when handling sodium hydroxide.