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Question

Equal lengths of magnesium ribbons are taken in test tubes A and B. Hydrochloric acid (HCl) is added to test tube A, while acetic acid (CH3COOH) is added to test tube B. Amount and concentration taken for both the acids are the same. In which test tube will the fizzing occur more vigorously and why?


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Solution

Part 1: Reaction of metal with an acid

  • When an acid reacts with metal, it will lead to the formation of salt and hydrogen gas.
  • Metal+AcidSalt+H2
  • The production of hydrogen gas is responsible for fizzing.

Part 2: Identifying the test tube which is fizzing more vigorously

Test Tube A: Magnesium Ribbon + Hydrochloric acid

  • Hydrochloric acid is a strong acid that reacts with magnesium leading to the formation of magnesium chloride and hydrogen gas.
  • The balanced chemical reaction can be represented as:

MgMagnesium+2HClHydrochloricacidMgCl2Magnesiumchloride+H2Hydrogengas

Test Tube B: Magnesium Ribbon + Acetic acid

  • Acetic acid is a weak acid that reacts with magnesium leading to the formation of magnesium acetate and hydrogen gas.
  • The balanced chemical reaction can be represented as:

MgMagnesium+2CH3COOHAceticacidMg(CH3COO)2Magnesiumacetate+H2Hydrogengas

Hence, Hydrochloric acid is a strong acid, a lot of hydrogen gas is liberated from test tube A. As a result, more fizzing occurs in test tube A.


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