The cell potential for the unbalanced chemical reaction
$Sn^{2 +} + ClO_{3}^{-} + H^{+} \to Sn^{4 +} + Cl^{-} + H_{2} O$ ; $E_{ce ll}^{\circ} = 0.12$ V
is measured under standard state conditions in an electrochemical cell. ( $\frac{2.303 RT}{F} = 0.06$ ). Then which is the correct statement?

Question

The cell potential for the unbalanced chemical reaction

$Sn^{2 +} + ClO_{3}^{-} + H^{+} \to Sn^{4 +} + Cl^{-} + H_{2} O$ ; $E_{ce ll}^{\circ} = 0.12$ V

is measured under standard state conditions in an electrochemical cell. ( $\frac{2.303 RT}{F} = 0.06$ ). Then which is the correct statement?

TestHub · Accepted Answer

Balanced: 3 Sn 2 + + ClO 3 − ​ + 6 H + → 3 Sn 4 + + Cl − + 3 H 2 ​ O , n = 6 . H + is used at the cathode ( ClO 3 − ​ reduction), so the cathodic solution is acidic: (A) true, (B) false. E = 0.12 − 6 0.06 ​ lo g [ H + ] 6 1 ​ = 0.12 − 0.06 pH . E = 0 at pH = 2: (C) true. Each Sn 2 + → Sn 4 + takes 2 electrons, so 0.3 mole of Sn 4 + needs 0.6 mole of electrons: (D) false. Answer: (A), (C).

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