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?

The fizzing, or the production of gas, will occur more vigorously in test tube A (containing hydrochloric acid, HCl) compared to test tube B (containing acetic acid, CH3COOH), and here’s why:

1. Reaction with HCl (Hydrochloric Acid):

Hydrochloric acid (HCl) is a strong acid. When it reacts with magnesium (Mg), it produces magnesium chloride (MgCl2) and hydrogen gas (H2):

2HCl(aq) + Mg(s) → MgCl2(aq) + H2(g)
This reaction occurs rapidly and vigorously because HCl is a strong acid that readily ionizes in water to release a high concentration of hydrogen ions (H+) in the solution. These hydrogen ions can easily react with magnesium to produce hydrogen gas.
2. Reaction with CH3COOH (Acetic Acid):

Acetic acid (CH3COOH) is a weak acid. When it reacts with magnesium, it also produces magnesium acetate (Mg(CH3COO)2) and hydrogen gas (H2):

2CH3COOH(aq) + Mg(s) → Mg(CH3COO)2(aq) + H2(g)
However, this reaction occurs more slowly and less vigorously compared to the reaction with HCl. Weak acids like acetic acid do not readily ionize in water, so they release fewer hydrogen ions for the reaction with magnesium. As a result, the fizzing is less vigorous.
In summary, the fizzing will be more vigorous in test tube A (HCl) because HCl is a strong acid, and the reaction between a strong acid and magnesium is more rapid and efficient in producing hydrogen gas compared to the reaction with the weaker acid acetic acid in test tube B.