Question

Equal lengths of magnesium ribbons are taken in test tubes A and B. Hydrochloric
acid is added to test tube A, while acetic acid is added to test tube B. The amount and
concentration taken for both the acids are same. In which test tube does the reaction
occur more vigourously and why?

Answer 1

In both test tubes there will be formation of hydrogen gas.

Hydrochloric acid is obviously stronger than acetic acid.

HCL is more concentrated than CH3COOH.

As a result of the increased HCL concentration there will be abundance of free H+ ions that will be generated as a result of the reaction.

Reaction will therefore occur more vigorously in Test Tube A.

Magnesium chloride will be formed in Test Tube A together with Hydrogen gas.

Answer 2

|$\large\mathrm\pink{Reason}$|

HCl is a strong acid whereas acetic is a weaker acid. Fizzing occurs because of the production of the hydrogen gas obtained due to reaction of the acid on the magnesium ribbon. Since HCl is a very strong acid there is a lot of liberation of hydrogen gas from test tube A. therefore, more fizzing take place in test tube A.