Equal lengths of magnesium ribbons are taken in test tubes $A$ and $B$ . Hydrochloric acid $(H C l)$ is added to test tube $A$ , while acetic acid $(C H_{3} C O O H)$ is added to test tube $B$ . Amount and concentration taken for both the acids are same. In which test tube will the fizzing occur more vigorously and why?

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Solution

Magnesium metal when reacts with an acid gives off hydrogen gas in the reaction. In test tube $A$ fizzing occurs more vigorously because $H C l$ is stronger acid than acetic acid. Hence, $H C l$ liberates hydrogen gas more vigorously, which causes fizzing more vigorously.

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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. Amount and concentration taken for both the acids are same. In which test tube will the fizzing occur more vigorously and why?

Magnesium metal when reacts with an acid gives off hydrogen gas in the reaction. In test tube A fizzing occurs more vigorously because HCl is stronger acid than acetic acid. Hence, HCl liberates hydrogen gas more vigorously, which causes fizzing more vigorously.

Magnesium metal when reacts with an acid gives off hydrogen gas in the reaction. In test tube $A$ fizzing occurs more vigorously because $H C l$ is stronger acid than acetic acid. Hence, $H C l$ liberates hydrogen gas more vigorously, which causes fizzing more vigorously.