QuestionJuly 26, 2025

Complete and balance the following redox reaction in acidic solution . Be sure to include the proper phases for all species within the reaction. As(s)arrow H_(2)AsO_(4)^-(aq)+AsH_(3)(s)

Complete and balance the following redox reaction in acidic solution . Be sure to include the proper phases for all species within the reaction. As(s)arrow H_(2)AsO_(4)^-(aq)+AsH_(3)(s)
Complete and balance the following redox reaction in acidic solution . Be sure to include the proper phases for all species within the reaction. As(s)arrow H_(2)AsO_(4)^-(aq)+AsH_(3)(s)

Solution
4.6(221 votes)

Answer

7As(s) + 12H_2O(l) + 24H^+(aq) \rightarrow 3H_{2}AsO_{4}^{-}(aq) + 4AsH_{3}(s) Explanation 1. Assign Oxidation States As(s) is 0, H_{2}AsO_{4}^{-} has As in +5, and AsH_{3} has As in -3. 2. Write Half-Reactions Oxidation: As(s) \rightarrow H_{2}AsO_{4}^{-}(aq); Reduction: As(s) \rightarrow AsH_{3}(s). 3. Balance Atoms Other Than O and H Oxidation: As(s) \rightarrow H_{2}AsO_{4}^{-}(aq); Reduction: As(s) \rightarrow AsH_{3}(s). 4. Balance Oxygen with Water Oxidation: As(s) + 4H_2O(l) \rightarrow H_{2}AsO_{4}^{-}(aq). 5. Balance Hydrogen with H⁺ Oxidation: As(s) + 4H_2O(l) \rightarrow H_{2}AsO_{4}^{-}(aq) + 8H^+(aq); Reduction: As(s) + 6H^+(aq) \rightarrow AsH_{3}(s). 6. Balance Charges with Electrons Oxidation: As(s) + 4H_2O(l) \rightarrow H_{2}AsO_{4}^{-}(aq) + 8H^+(aq) + 8e^-; Reduction: As(s) + 6H^+(aq) + 6e^- \rightarrow AsH_{3}(s). 7. Equalize Electron Transfer Multiply reduction by 4 and oxidation by 3 to equalize electrons: 3As(s) + 12H_2O(l) \rightarrow 3H_{2}AsO_{4}^{-}(aq) + 24H^+(aq) + 24e^-; 4As(s) + 24H^+(aq) + 24e^- \rightarrow 4AsH_{3}(s). 8. Combine and Simplify 7As(s) + 12H_2O(l) + 24H^+(aq) \rightarrow 3H_{2}AsO_{4}^{-}(aq) + 4AsH_{3}(s).

Explanation

1. Assign Oxidation States<br /> $As(s)$ is 0, $H_{2}AsO_{4}^{-}$ has As in +5, and $AsH_{3}$ has As in -3.<br />2. Write Half-Reactions<br /> Oxidation: $As(s) \rightarrow H_{2}AsO_{4}^{-}(aq)$; Reduction: $As(s) \rightarrow AsH_{3}(s)$.<br />3. Balance Atoms Other Than O and H<br /> Oxidation: $As(s) \rightarrow H_{2}AsO_{4}^{-}(aq)$; Reduction: $As(s) \rightarrow AsH_{3}(s)$.<br />4. Balance Oxygen with Water<br /> Oxidation: $As(s) + 4H_2O(l) \rightarrow H_{2}AsO_{4}^{-}(aq)$.<br />5. Balance Hydrogen with H⁺<br /> Oxidation: $As(s) + 4H_2O(l) \rightarrow H_{2}AsO_{4}^{-}(aq) + 8H^+(aq)$; Reduction: $As(s) + 6H^+(aq) \rightarrow AsH_{3}(s)$.<br />6. Balance Charges with Electrons<br /> Oxidation: $As(s) + 4H_2O(l) \rightarrow H_{2}AsO_{4}^{-}(aq) + 8H^+(aq) + 8e^-$; Reduction: $As(s) + 6H^+(aq) + 6e^- \rightarrow AsH_{3}(s)$.<br />7. Equalize Electron Transfer<br /> Multiply reduction by 4 and oxidation by 3 to equalize electrons: <br /> $3As(s) + 12H_2O(l) \rightarrow 3H_{2}AsO_{4}^{-}(aq) + 24H^+(aq) + 24e^-$; $4As(s) + 24H^+(aq) + 24e^- \rightarrow 4AsH_{3}(s)$.<br />8. Combine and Simplify<br /> $7As(s) + 12H_2O(l) + 24H^+(aq) \rightarrow 3H_{2}AsO_{4}^{-}(aq) + 4AsH_{3}(s)$.
Click to rate:

Similar Questions