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 $(C H_{3} C O O H)$ is added to test tube B. In which test tube will the fizzing occur more vigorously and why?

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Solution

When an acid reacts with a metal such as magnesium then it produces hydrogen gas $(H_{2})$ .

Hydrochloric acid (HCl) is a strong acid whereas acetic acid $(C H_{3} C O O H)$ is a weak acid. Thus, the hydrochloric acid solution contains a much greater amount of hydrogen ions.

Therefore, fizzing will occur more vigorously in test tube A (containing HCl acid) because HCl produces hydrogen gas more vigorously (which causes fizzing).

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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. In which test tube will the fizzing occur more vigorously and why?

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 $(C H_{3} C O O H)$ is added to test tube B. In which test tube will the fizzing occur more vigorously and why?