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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 have fizzing occur more vigorously?
A. A
B. B
C. Both
D. None

Answer
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Hint: As we know that fizzing occurs in a chemical reaction due to the presence of a gas. Here, to identify the test tube in which fizzing occurs more vigorously, then we need to compare the acidity of both CH3COOH and HCl.

Complete step by step answer:
According to question when equal lengths of magnesium ribbons are taken in test tubes A and B. Then, hydrochloric acid (HCl) is added to test-tube A, while acetic acid (CH3COOH) is added to test tube B.
Thus, the reaction in test tube A is:
Mg(s)+2HCl(aq)MgCl2(aq)+H2(g)
And the reaction in test tube B is:
Mg(s)+CH3COOH(aq)Mg(CH3COO)2(aq)+H2(g)
It is evident that hydrogen gas is released in both the reactions. Though concentration of both the acids is same but we also know that hydrochloric acid is a stronger and reactive acid than acetic acid and therefore, the hydrogen gas produced in the reaction is at a faster rate due to which frizzing occurs in test tube A. ​
As HCl is a stronger acid as compared toCH3COOH, magnesium metal is added to the chemical reaction. Thus, HCl produces hydrogen gas due to which fizzing will be more vigorous in test-tube A.

So, the correct answer is Option A .

Note:
From the above question, we get to know that fizzing will occur more in test tube A because:
HCl is a stronger acid whereas CH3COOH is a weaker acid.
Hydrochloric acid completely dissociates into H+ and Clions while CH3COOHdoesn’t ionize completely.