6. Chemical Quantities & Aqueous Reactions

Balance the redox reaction in basic solution. What is the coefficient on the hydroxide ion, and on which side of the equation does it appear? (a) 2 OH- in reactants (b) 4 OH- in products (c) 4 OH- in reactants (d) 3 OH- in reactants

Complete and balance the following half-reactions. In each case, indicate whether the half-reaction is an oxidation or a reduction. (f) SO32-1aq2 ¡ SO42-1aq2 (basic solution)

Complete and balance the following half-reactions. In each case indicate whether the half-reaction is an oxidation or a reduction. (g) Cr1OH231s2 ¡ CrO42-1aq2 (basic solution)

Complete and balance the following equations, and identify the oxidizing and reducing agents: (e) MnO4-1aq2 + Br -1aq2 ¡ MnO21s2 + BrO3-1aq2 (basic solution)

Complete and balance the following equations, and identify the oxidizing and reducing agents. (Recall that the O atoms in hydrogen peroxide, H2O2, have an atypical oxidation state.) (f) H2O21aq2 + ClO21aq2 ¡ ClO2-1aq2 + O21g2 (basic solution)

Balance each redox reaction occurring in basic aqueous solution. b. Al(s) + MnO4-(aq) ¡ MnO2(s) + Al(OH)4-(aq)

Balance each redox reaction occurring in basic aqueous solution. a. H2O2(aq) + ClO2(aq) ¡ ClO2-(aq) + O2(g)

Balance each redox reaction occurring in basic aqueous solution. c. NO2-(aq) + Al(s) ¡ NH3(g) + AlO2-(aq)

Balance each redox reaction occurring in basic aqueous solution. b. Ag(s) + CN-(aq) + O2(g) ¡ Ag(CN)2-(aq)

Balance each redox reaction occurring in basic aqueous solution. a. MnO4-(aq) + Br-(aq) ¡ MnO2(s) + BrO3-(aq)

Balance the half-reactions in Problem 19.42, assuming that they occur in basic solution.

Balance the following half-reactions. (d) (basic) ClO-(aq) -> Cl-(aq)

Balance the following half-reactions. (c) (basic) Br3+(aq) -> BiO3-(aq)

Balance the following half-reactions. (b) (basic) CrO42-(aq) -> Cr(OH)4-(aq)

Balance the following half-reactions. (a) (acidic) Cr2O22-(aq) -> Cr3+(aq)

Balance the following half-reactions. (d) (basic) Br2(aq) -> BrO3-(aq)

Balance the following half-reactions. (b) (basic) Ni(OH)2(s) -> Ni2O3(s)

Balance the following half-reactions. (c) (acidic) NO3-(aq) -> NO2(aq)

Balance the following half-reactions. (a) (acidic) VO2+(aq) -> V3+(aq)

Write balanced net ionic equations for the following reactions in acidic solution. (c)

Write balanced net ionic equations for the following reactions in acidic solution. (b)

Write balanced net ionic equations for the following reactions in acidic solution. (a)

Write balanced net ionic equations for the following reactions in acidic solution. (c)

Write balanced net ionic equations for the following reactions in acidic solution. (b)

Write balanced net ionic equations for the following reactions in acidic solution. (a)

Consider the unbalanced equation: (a) Balance the equation for this reaction in basic solution.

Gold metal is extracted from its ore by treating the crushed rock with an aerated cyanide solution. The unbalanced equation for the reaction is (a) Balance the equation for this reaction in basic solution.