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Oxidation - Reduction Reactions Complete and balance the following half-reactions. In each case indicate oxidation of a reduction. a) Sn²(aq) → Sn(aq) (acidic solution) b) TiO2(s)→ Ti²(aq) (acidic solution) c) H₂SO3(aq) → SO4 (aq) (acidic solution) d) Mn²(aq) → MnO2(s) (basic solution) I

Oxidation - Reduction Reactions Complete and balance the following half-reactions. In each case indicate oxidation of a reduction. a) Sn²(aq) → Sn(aq) (acidic solution) b) TiO2(s)→ Ti²(aq) (acidic solution) c) H₂SO3(aq) → SO4 (aq) (acidic solution) d) Mn²(aq) → MnO2(s) (basic solution) I

Chemistry: Principles and Practice
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter18: Electrochemistry
Section: Chapter Questions
Problem 18.77QE: A solution contains the ions H+, Ag+, Pb2+, and Ba2+, each at a concentration of 1.0 M. (a) Which of...
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Oxidation - Reduction Reactions Complete and balance the following half-reactions. In each case indicate whether the half-reaction is an oxidation of a reduction. a) Sn²(aq) → Sn(aq) (acidic solution) b) TiO₂(s) -> Ti²+ (aq) (acidic solution) c) H₂SO3(aq) ->> SO4 (aq) (acidic solution) d) Mn²+ (aq) ->> MnO₂(s) (basic solution) c) SO² (aq) -> SO4 (aq) (basic solution) f) N₂(g) 1 NH(aq) (acidic solution) H₂O(1) (basic solution) (acidic solution) g) O2(g) → ->> h) ClO3(aq) → Cl(aq) -
Transcribed Image Text:Oxidation - Reduction Reactions Complete and balance the following half-reactions. In each case indicate whether the half-reaction is an oxidation of a reduction. a) Sn²(aq) → Sn(aq) (acidic solution) b) TiO₂(s) -> Ti²+ (aq) (acidic solution) c) H₂SO3(aq) ->> SO4 (aq) (acidic solution) d) Mn²+ (aq) ->> MnO₂(s) (basic solution) c) SO² (aq) -> SO4 (aq) (basic solution) f) N₂(g) 1 NH(aq) (acidic solution) H₂O(1) (basic solution) (acidic solution) g) O2(g) → ->> h) ClO3(aq) → Cl(aq) -
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