Acids and Bases

Acids

• Definition: Substances that donate protons (H⁺ ions) in a chemical reaction.
• Properties:
  • Sour taste
  • Conduct electricity in solution
  • Turn blue litmus paper red
  • React with metals to produce hydrogen gas
• Examples:
  • Hydrochloric acid (HCl)
  • Sulfuric acid (H₂SO₄)
  • Acetic acid (CH₃COOH)

Bases

• Definition: Substances that accept protons or donate hydroxide ions (OH⁻) in a reaction.
• Properties:
  • Bitter taste
  • Slippery feel
  • Conduct electricity in solution
  • Turn red litmus paper blue
• Examples:
  • Sodium hydroxide (NaOH)
  • Potassium hydroxide (KOH)
  • Calcium carbonate (CaCO₃)

Salts

• Definition: Ionic compounds formed from the neutralization reaction between an acid and a base.
• Properties:
  • Usually crystalline at room temperature
  • High melting and boiling points
  • Can conduct electricity when dissolved in water
• Examples:
  • Sodium chloride (NaCl) - common table salt
  • Calcium sulfate (CaSO₄)
  • Ammonium nitrate (NH₄NO₃)

pH Scale

• Range: 0 to 14
• Acidic: pH < 7
• Neutral: pH = 7 (pure water)
• Basic: pH > 7
• Significance: Indicates the concentration of H⁺ ions in a solution; lower pH means higher acidity, higher pH means higher alkalinity.

Neutralization Reaction

• Definition: A chemical reaction between an acid and a base producing salt and water.
• General Equation:
  • Acid + Base → Salt + Water
• Importance: Used in various applications, including antacid formulations and in treating acidic soils.

Common Uses

• Acids: Food preservation, battery production, cleaning agents.
• Bases: Cleaning products, antacids, soap making.
• Salts: Food seasoning, fertilizers, water softeners.

Acids

• Acids are substances that donate protons (H⁺ ions) during chemical reactions.
• Characteristic properties include a sour taste, the ability to conduct electricity in solution, turning blue litmus paper red, and reacting with metals to release hydrogen gas.
• Notable examples include hydrochloric acid (HCl), sulfuric acid (H₂SO₄), and acetic acid (CH₃COOH).

Bases

• Bases are substances that either accept protons or donate hydroxide ions (OH⁻) in reactions.
• They are identified by their bitter taste, slippery texture, ability to conduct electricity in solution, and their capacity to turn red litmus paper blue.
• Common bases include sodium hydroxide (NaOH), potassium hydroxide (KOH), and calcium carbonate (CaCO₃).

Salts

• Salts are ionic compounds produced through the neutralization of an acid and a base.
• They typically form crystalline structures at room temperature, possess high melting and boiling points, and can conduct electricity when dissolved in water.
• Examples of salts are sodium chloride (NaCl), calcium sulfate (CaSO₄), and ammonium nitrate (NH₄NO₃).

pH Scale

• The pH scale ranges from 0 to 14, measuring the acidity or alkalinity of a solution.
• Solutions with a pH less than 7 are classified as acidic, a pH of 7 indicates neutrality (like pure water), and a pH greater than 7 indicates basicity.
• The pH value reflects the concentration of H⁺ ions; lower pH indicates stronger acidity, while higher pH indicates stronger alkalinity.

Neutralization Reaction

• A neutralization reaction occurs when an acid reacts with a base to produce salt and water.
• The general equation for this reaction is: Acid + Base → Salt + Water.
• This type of reaction is vital in various applications such as antacid production and acidic soil treatment.

Common Uses

• Acids are commonly used in food preservation, battery production, and as cleaning agents.
• Bases find applications in cleaning products, antacids, and soap manufacturing.
• Salts are widely used for seasoning food, in fertilizers, and as water softeners.