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 $(CH_3COOH)$ is added to test tube $B$. The amount and concentration taken for both the acids are the same. In which test tube will the fizzing occur more vigorously and why?

(A) The fizzing will occur more vigorously in test tube $A$,to which hydrochloric acid $(HCl)$ is added.
This is because $HCl$ is a strong acid,whereas $CH_3COOH$ is a weak acid.
Strong acids dissociate completely in water to produce a higher concentration of hydrogen ions $(H^+)$ compared to weak acids.
Since the reaction between magnesium and acid depends on the concentration of $H^+$ ions,the reaction in test tube $A$ proceeds at a faster rate,resulting in more vigorous evolution of hydrogen gas.