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 $({CH}_{3} COOH)$ is added to test tube B. In which test tube will the fizzing occur more vigorously and why?

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Solution

The fizzing will occur strongly in test tube A, that contains hydrochloric acid $HCl$ . This is because $HCl$ is a stronger acid than ${CH}_{3} COOH$ , hence the reaction with magnesium would occur vigorously and hydrogen gas would be released at a faster speed (due to which fizzing occurs).

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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?

The fizzing will occur strongly in test tube A, that contains hydrochloric acid HCl. This is because HCl is a stronger acid than CH3COOH, hence the reaction with magnesium would occur vigorously and hydrogen gas would be released at a faster speed (due to which fizzing occurs).

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 $({CH}_{3} COOH)$ is added to test tube B. In which test tube will the fizzing occur more vigorously and why?

The fizzing will occur strongly in test tube A, that contains hydrochloric acid $HCl$ . This is because $HCl$ is a stronger acid than ${CH}_{3} COOH$ , hence the reaction with magnesium would occur vigorously and hydrogen gas would be released at a faster speed (due to which fizzing occurs).