Reactions of acids with metals

• What is the purpose of indicators in chemistry?

  Indicators are used to determine whether a solution is acidic or alkaline.
• What do acids produce when they react with metals, bases, and carbonates?

  Acids produce salts when they react with metals, bases, and carbonates.
• What is neutralisation in chemistry?

  Neutralisation is the reaction between an acid and a base.
• What are the products of the reaction of acids with metals?

  • A salt
  • Hydrogen gas
• What is the general equation for the reaction of an acid with a metal?

  Acid + metal → salt + hydrogen.
• Write the equation for the reaction of hydrochloric acid with magnesium.

  2HCl(aq) + Mg(s) → MgCl₂(aq) + H₂(g).
• Which metals react with hydrochloric acid?

  Magnesium, zinc, and iron react with hydrochloric acid.
• What are the products of the reaction of sulfuric acid with iron?

  The products are iron(II) sulfate and hydrogen.
• Write the equation for the reaction of sulfuric acid with zinc.

  H₂SO₄(aq) + Zn(s) → ZnSO₄(aq) + H₂(g).
• What type of reactions occur when acids react with metals?

  The reactions of acids with metals are redox reactions.
• What is a redox reaction?

  A redox reaction is when reduction and oxidation take place at the same time.
• What is an ionic equation?

  An ionic equation shows how positively charged ions join with negatively charged ions to make a compound.
• Write the ionic equation for the reaction of magnesium with hydrochloric acid.

  2H⁺(aq) + Mg(s) → Mg²⁺(aq) + H₂(g).
• What happens to magnesium atoms during the reaction with hydrochloric acid?

  Magnesium atoms lose electrons and are oxidised.
• What happens to hydrogen ions during the reaction with magnesium?

  Hydrogen ions gain electrons and are reduced.
• What are the half equations for the reaction of zinc with sulfuric acid?

  • Zn(s) → Zn²⁺(aq) + 2e^- (oxidation)
  • 2H⁺(aq) + 2e^- → H₂(g) (reduction)
• Why is the reaction of zinc with sulfuric acid classified as a redox reaction?

  Because zinc loses electrons (oxidation) and hydrogen ions gain electrons (reduction) simultaneously.