Introduction to Acids, Bases, and Alkalis

Key Concepts

• Acid: A substance that produces hydrogen ions (H⁺) in aqueous solutions.
• Base: A chemical that can neutralize acids, usually metal oxides or metal hydroxides.
• Alkali: A base that is soluble in water, producing hydroxide ions (OH⁻).

Common Acids

• Hydrochloric Acid (HCl)
  • Produces hydrogen ions (H⁺) and chloride ions (Cl⁻) in aqueous solutions.
• Sulfuric Acid (H₂SO₄)
  • Produces hydrogen ions (H⁺) and sulfate ions (SO₄²⁻) in aqueous solutions.
• Nitric Acid (HNO₃)
  • Produces hydrogen ions (H⁺) and nitrate ions (NO₃⁻) in aqueous solutions.

Properties of Acids

• Acids produce hydrogen ions (H⁺) in aqueous solutions.

Bases and Alkalis

• Bases: Neutralize acids to produce a salt and water.
  • Examples: Copper oxide, iron(III) hydroxide, sodium hydroxide.
• Alkalis: Bases that are soluble in water.
  • Example: Sodium hydroxide (NaOH)
  • Produce sodium ions (Na⁺) and hydroxide ions (OH⁻) in aqueous solutions.

pH Scale

• Acidity and Alkalinity Measurement
  • Acids: pH between 0 and 6.
  • Neutral Solutions: pH of 7.
  • Alkaline Solutions: pH between 8 and 14.
• Measuring pH
  • pH Probe: Determines pH electronically.
  • Universal Indicator: Changes color to indicate pH level.
    • Green: Neutral (pH 7)
    • Red: Very acidic
    • Purple: Very alkaline

Neutralization Reaction

• Process: Reaction between hydrogen ions (H⁺) from acids and hydroxide ions (OH⁻) from alkalis to produce water.
• Equation: H⁺ + OH⁻ → H₂O

Additional Resources

• Practice questions available in the provided workbook link.

Ensure to review these notes and understand the equations and chemical reactions as they are fundamental in chemistry. Utilize the workbook for further practice and understanding.