Question

Consider the reaction :
$H_{2}S{O}_3(aq)+S{n}^{4+}(aq)+H_{2}O(l)\to S{n}^{2+}(aq)+HS{O}_4^{-}(aq)+3H^{+}(aq)$
Which of the following statements is correct?

• A. $S{n}^{4+}$ is the oxidizing agent because it undergoes oxidation
• B. $S{n}^{4+}$ is the reducing agent because it undergoes oxidation
• C. $H_{2}S{O}_3$ is the reducing agent because it undergoes oxidation
• D. $H_{2}S{O}_3$ is the reducing agent because it undergoes reduction

Answer 1

Answer: (C)

$H_2^{+4}S{O}_3\left(aq\right)+s{n}^{4+}\left(aq\right)+H_{2}O\left(l\right)\to s{n}^{2+}\left(aq\right)+H{S}^{+6}{O}_4^{-}\left(aq\right)+3H^{+}$
Hence $H_{2}S{O}_3$ is the reducing agent because it undergoes oxidation.