aicd and metal

• Practical 2.21: Investigate the reactions between dilute hydrochloric and sulfuric acids and metals (e.g. magnesium, zinc and iron)

  1. Set up apparatus

  2. Place 100 cm3 of hydrochloric acid in conical flask

  3. Record start volume of water in measuring cylinder

  4. Record mass of metal, add to acid, attach bung and start timer

  5. Record new water level after 30 seconds, calculate volume of gas produced and rate of reaction

  6. Repeat with different metals
• Displacement reactions


  • Mg + 2HCl → MgCl2 + H2
  • Zn + 2HCl → ZnCl2 + H2
  • Fe + 2HCl → FeCl2 + H2
• Variables to control


  • Concentration of acid
  • Volume of acid
  • Surface area of metal
  • Mass of metal
  • Temperature of reactants/environment
• Metals below hydrogen in the reactivity series will not react with hydrochloric or sulfuric acid because they are unable to displace hydrogen ions from the acid to form a salt
• Hydrochloric acid is corrosive. Wear safety goggles.
• Make sure the measuring cylinder is large enough to contain the volume gas produced otherwise equipment may get damaged.
• Be careful with the glassware. Clear up any broken glassware immediately.
• Rate of reaction


  Volume of gas produced ÷ time
• Observations and rates for different metals


  • Magnesium: Bubbles of gas, magnesium disappears, colourless solution forms, temperature increases (exothermic), fastest rate
  • Zinc: Bubbles of gas, zinc disappears, colourless solution forms, medium rate
  • Iron: Bubbles of gas, iron disappears, pale green solution forms, slowest rate