Reactions of Acids with Metals and Metal Oxides

Reactions of Acids with Metals

• Acids are reactive with metals, producing hydrogen gas and a salt.

Example 1: Calcium and Hydrochloric Acid

• Reaction: Calcium (Ca) + Hydrochloric Acid (HCl) → Hydrogen Gas (H₂) + Calcium Chloride (CaCl₂)
• Balanced Equation:
  • Unbalanced: Ca + 2 HCl → H₂ + CaCl₂
  • To balance:
  • 1 Calcium on both sides
  • Initially, 1 Hydrogen on the left; 2 on the right. Add coefficient of 2 to HCl. Now, 2 Chloride on both sides.
• Final Balanced Equation:
  • Ca + 2 HCl → H₂ + CaCl₂

Example 2: Iron and Sulfuric Acid

• Reaction: Iron (Fe) + Sulfuric Acid (H₂SO₄) → Hydrogen Gas (H₂) + Iron(II) Sulfate (FeSO₄)
• Given Product: Iron (II) Sulfate (Fe²⁺)
• Balanced Equation:
  • Unbalanced: Fe + H₂SO₄ → H₂ + FeSO₄
  • Balancing checks:
  • 1 Iron on both sides
  • 2 Hydrogen on both sides
  • 1 Sulfate on both sides
• Final Balanced Equation:
  • Fe + H₂SO₄ → H₂ + FeSO₄

Reactions of Acids with Metal Oxides

• Acids react with metal oxides, producing water and a salt.

Example 3: Hydrobromic Acid and Lithium Oxide

• Reaction: Hydrobromic Acid (HBr) + Lithium Oxide (Li₂O) → Water (H₂O) + Lithium Bromide (LiBr)
• Balanced Equation:
  • Unbalanced: HBr + Li₂O → H₂O + LiBr
  • Balancing checks:
  • 2 Lithium on left; add coefficient of 2 to the product side (LiBr)
  • This means 2 Bromide on left; add coefficient of 2 to HBr.
  • Hydrogen and Oxygen are balanced.
• Final Balanced Equation:
  • 2 HBr + Li₂O → H₂O + 2 LiBr

Summary of Common Reactions

• **Types of Reactions: **

  • Metals with acids yield hydrogen gas and salts.
  • Metal oxides with acids yield water and salts.

• Importance of Balancing:

  • Essential for reactions to follow the law of conservation of mass.
  • Indicates correct proportions for the reactants and products in a chemical reaction.