Oct 27, 2010 . Balance the following oxidation-reduction reactions, which occur in basic solution , using the half-reaction method. (Use the lowest possible . Cr(OH)3(s) + ClO3<sup>-</sup>(aq) --> CrO4<sup>2-</sup>(aq) + Cl<sup>-</sup>(aq) (basic). Solution: Step #1: Cr( OH)3 --> CrO4<sup>2-</sup>. ClO3<sup>-</sup> --> Cl<sup>-</sup>. Step #2: (Not necessary for this example).Answer to Balance each of the following redox reactions occurring in basic solution. Cl2(g) ----> Cl-(aq) +ClO- (aq) Balance each. ClO3¯(aq) + Cl¯(aq) ---> Cl2(g) + ClO2(aq) [acidic sol.] Before balancing. Cl¯ (- 1) Cl2 (0) ClO2 (+4). Solution #1: 1) Half-reactions: Cl¯ ---> Cl2 ClO3¯ ---> ClO2.What are the coefficients in front of. Cr(OH)4- and ClO- in the balanced reaction? Cr(OH)4-(aq) + ClO-(aq) → CrO42-(aq) + Cl-(aq). A) Cr(OH)4- = 2, ClO- = 3.is +2, ON of Cl in ClO- is +1, ON of Pb in. PbO2 is +4 and ON for Cl in Cl- is -1. b) Reduction: ClO-(aq) → Cl-(aq) and oxidation: Pb(OH)2-. 4 (aq) →. PbO2(s).PbO2(s) + SO4<sup>2–</sup>(aq) + 4 H<sup>+</sup>(aq) + 2 e<sup>–</sup> PbSO4(s) + 2 H2O. +1.685. Au<sup>+</sup>(aq) + e <sup>–</sup> Au(s). ClO3<sup>–</sup>(aq) + 6 H<sup>+</sup>(aq) + 5 e<sup>–</sup> 1/2 Cl2(g) + 3 H2O. +1.47. BrO3<sup>–</sup> + 6 . Apr 21, 2006 . Cr(s) + HCl(aq) Cr<sup>3+</sup>(aq) + H2(g) + Cl<sup>–</sup>(aq). Mg(s) + O3(g) Mg(OH)2(s) + O2(g). 1 ). HI(aq) + ClO3<sup>–</sup>(aq) I3<sup>–</sup>(aq) + Cl2(g). Al(s) + ClO<sup>–</sup>(aq) . (b) Zn(s) + O2(g) + H2O(l) --> Zn<sup>2+</sup>(aq) + OH<sup>-</sup>(aq). (c) Fe(NO3)2(aq) + Cr2O7<sup>2-</sup>( aq) --> Fe(NO3)3 + Cr<sup>3+</sup>(aq). (a) Zn(s) + ClO<sup>-</sup>(aq) --> Zn(OH)2(s) + Cl<sup>-</sup>(aq).___ Al(s) + ___ HBr(aq) →. 11.. ___ Ba(C2H3O2)2(aq) + ___ (NH4)2SO4(aq) →. . Cl2 + 4 OH. − → 2 ClO. −. + 2 H2O + 2 e. −. + 4 OH. −. Check: Cl 2 ✓. O 2 ✓.

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Oct 27, 2010 . Balance the following oxidation-reduction reactions, which occur in basic solution , using the half-reaction method. (Use the lowest possible . Cr(OH)3(s) + ClO3<sup>-</sup>(aq) --> CrO4<sup>2-</sup>(aq) + Cl<sup>-</sup>(aq) (basic). Solution: Step #1: Cr( OH)3 --> CrO4<sup>2-</sup>. ClO3<sup>-</sup> --> Cl<sup>-</sup>. Step #2: (Not necessary for this example).Answer to Balance each of the following redox reactions occurring in basic solution. Cl2(g) ----> Cl-(aq) +ClO- (aq) Balance each. ClO3¯(aq) + Cl¯(aq) ---> Cl2(g) + ClO2(aq) [acidic sol.] Before balancing. Cl¯ (- 1) Cl2 (0) ClO2 (+4). Solution #1: 1) Half-reactions: Cl¯ ---> Cl2 ClO3¯ ---> ClO2.What are the coefficients in front of. Cr(OH)4- and ClO- in the balanced reaction? Cr(OH)4-(aq) + ClO-(aq) → CrO42-(aq) + Cl-(aq). A) Cr(OH)4- = 2, ClO- = 3.is +2, ON of Cl in ClO- is +1, ON of Pb in. PbO2 is +4 and ON for Cl in Cl- is -1. b) Reduction: ClO-(aq) → Cl-(aq) and oxidation: Pb(OH)2-. 4 (aq) →. PbO2(s).PbO2(s) + SO4<sup>2–</sup>(aq) + 4 H<sup>+</sup>(aq) + 2 e<sup>–</sup> PbSO4(s) + 2 H2O. +1.685. Au<sup>+</sup>(aq) + e <sup>–</sup> Au(s). ClO3<sup>–</sup>(aq) + 6 H<sup>+</sup>(aq) + 5 e<sup>–</sup> 1/2 Cl2(g) + 3 H2O. +1.47. BrO3<sup>–</sup> + 6 . Apr 21, 2006 . Cr(s) + HCl(aq) Cr<sup>3+</sup>(aq) + H2(g) + Cl<sup>–</sup>(aq). Mg(s) + O3(g) Mg(OH)2(s) + O2(g). 1 ). HI(aq) + ClO3<sup>–</sup>(aq) I3<sup>–</sup>(aq) + Cl2(g). Al(s) + ClO<sup>–</sup>(aq) . (b) Zn(s) + O2(g) + H2O(l) --> Zn<sup>2+</sup>(aq) + OH<sup>-</sup>(aq). (c) Fe(NO3)2(aq) + Cr2O7<sup>2-</sup>( aq) --> Fe(NO3)3 + Cr<sup>3+</sup>(aq). (a) Zn(s) + ClO<sup>-</sup>(aq) --> Zn(OH)2(s) + Cl<sup>-</sup>(aq).___ Al(s) + ___ HBr(aq) →. 11.. ___ Ba(C2H3O2)2(aq) + ___ (NH4)2SO4(aq) →. . Cl2 + 4 OH. − → 2 ClO. −. + 2 H2O + 2 e. −. + 4 OH. −. Check: Cl 2 ✓. O 2 ✓.

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Oct 27, 2010 . Balance the following oxidation-reduction reactions, which occur in basic solution , using the half-reaction method. (Use the lowest possible . Cr(OH)3(s) + ClO3<sup>-</sup>(aq) --> CrO4<sup>2-</sup>(aq) + Cl<sup>-</sup>(aq) (basic). Solution: Step #1: Cr( OH)3 --> CrO4<sup>2-</sup>. ClO3<sup>-</sup> --> Cl<sup>-</sup>. Step #2: (Not necessary for this example).Answer to Balance each of the following redox reactions occurring in basic solution. Cl2(g) ----> Cl-(aq) +ClO- (aq) Balance each. ClO3¯(aq) + Cl¯(aq) ---> Cl2(g) + ClO2(aq) [acidic sol.] Before balancing. Cl¯ (- 1) Cl2 (0) ClO2 (+4). Solution #1: 1) Half-reactions: Cl¯ ---> Cl2 ClO3¯ ---> ClO2.What are the coefficients in front of. Cr(OH)4- and ClO- in the balanced reaction? Cr(OH)4-(aq) + ClO-(aq) → CrO42-(aq) + Cl-(aq). A) Cr(OH)4- = 2, ClO- = 3.is +2, ON of Cl in ClO- is +1, ON of Pb in. PbO2 is +4 and ON for Cl in Cl- is -1. b) Reduction: ClO-(aq) → Cl-(aq) and oxidation: Pb(OH)2-. 4 (aq) →. PbO2(s).PbO2(s) + SO4<sup>2–</sup>(aq) + 4 H<sup>+</sup>(aq) + 2 e<sup>–</sup> PbSO4(s) + 2 H2O. +1.685. Au<sup>+</sup>(aq) + e <sup>–</sup> Au(s). ClO3<sup>–</sup>(aq) + 6 H<sup>+</sup>(aq) + 5 e<sup>–</sup> 1/2 Cl2(g) + 3 H2O. +1.47. BrO3<sup>–</sup> + 6 . Apr 21, 2006 . Cr(s) + HCl(aq) Cr<sup>3+</sup>(aq) + H2(g) + Cl<sup>–</sup>(aq). Mg(s) + O3(g) Mg(OH)2(s) + O2(g). 1 ). HI(aq) + ClO3<sup>–</sup>(aq) I3<sup>–</sup>(aq) + Cl2(g). Al(s) + ClO<sup>–</sup>(aq) . (b) Zn(s) + O2(g) + H2O(l) --> Zn<sup>2+</sup>(aq) + OH<sup>-</sup>(aq). (c) Fe(NO3)2(aq) + Cr2O7<sup>2-</sup>( aq) --> Fe(NO3)3 + Cr<sup>3+</sup>(aq). (a) Zn(s) + ClO<sup>-</sup>(aq) --> Zn(OH)2(s) + Cl<sup>-</sup>(aq).___ Al(s) + ___ HBr(aq) →. 11.. ___ Ba(C2H3O2)2(aq) + ___ (NH4)2SO4(aq) →. . Cl2 + 4 OH. − → 2 ClO. −. + 2 H2O + 2 e. −. + 4 OH. −. Check: Cl 2 ✓. O 2 ✓.

Oct 27, 2010 . Balance the following oxidation-reduction reactions, which occur in basic solution , using the half-reaction method. (Use the lowest possible . Cr(OH)3(s) + ClO3<sup>-</sup>(aq) --> CrO4<sup>2-</sup>(aq) + Cl<sup>-</sup>(aq) (basic). Solution: Step #1: Cr( OH)3 --> CrO4<sup>2-</sup>. ClO3<sup>-</sup> --> Cl<sup>-</sup>. Step #2: (Not necessary for this example).Answer to Balance each of the following redox reactions occurring in basic solution. Cl2(g) ----> Cl-(aq) +ClO- (aq) Balance each. ClO3¯(aq) + Cl¯(aq) ---> Cl2(g) + ClO2(aq) [acidic sol.] Before balancing. Cl¯ (- 1) Cl2 (0) ClO2 (+4). Solution #1: 1) Half-reactions: Cl¯ ---> Cl2 ClO3¯ ---> ClO2.What are the coefficients in front of. Cr(OH)4- and ClO- in the balanced reaction? Cr(OH)4-(aq) + ClO-(aq) → CrO42-(aq) + Cl-(aq). A) Cr(OH)4- = 2, ClO- = 3.is +2, ON of Cl in ClO- is +1, ON of Pb in. PbO2 is +4 and ON for Cl in Cl- is -1. b) Reduction: ClO-(aq) → Cl-(aq) and oxidation: Pb(OH)2-. 4 (aq) →. PbO2(s).PbO2(s) + SO4<sup>2–</sup>(aq) + 4 H<sup>+</sup>(aq) + 2 e<sup>–</sup> PbSO4(s) + 2 H2O. +1.685. Au<sup>+</sup>(aq) + e <sup>–</sup> Au(s). ClO3<sup>–</sup>(aq) + 6 H<sup>+</sup>(aq) + 5 e<sup>–</sup> 1/2 Cl2(g) + 3 H2O. +1.47. BrO3<sup>–</sup> + 6 . Apr 21, 2006 . Cr(s) + HCl(aq) Cr<sup>3+</sup>(aq) + H2(g) + Cl<sup>–</sup>(aq). Mg(s) + O3(g) Mg(OH)2(s) + O2(g). 1 ). HI(aq) + ClO3<sup>–</sup>(aq) I3<sup>–</sup>(aq) + Cl2(g). Al(s) + ClO<sup>–</sup>(aq) . (b) Zn(s) + O2(g) + H2O(l) --> Zn<sup>2+</sup>(aq) + OH<sup>-</sup>(aq). (c) Fe(NO3)2(aq) + Cr2O7<sup>2-</sup>( aq) --> Fe(NO3)3 + Cr<sup>3+</sup>(aq). (a) Zn(s) + ClO<sup>-</sup>(aq) --> Zn(OH)2(s) + Cl<sup>-</sup>(aq).___ Al(s) + ___ HBr(aq) →. 11.. ___ Ba(C2H3O2)2(aq) + ___ (NH4)2SO4(aq) →. . Cl2 + 4 OH. − → 2 ClO. −. + 2 H2O + 2 e. −. + 4 OH. −. Check: Cl 2 ✓. O 2 ✓.

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Oct 27, 2010 . Balance the following oxidation-reduction reactions, which occur in basic solution , using the half-reaction method. (Use the lowest possible . Cr(OH)3(s) + ClO3<sup>-</sup>(aq) --> CrO4<sup>2-</sup>(aq) + Cl<sup>-</sup>(aq) (basic). Solution: Step #1: Cr( OH)3 --> CrO4<sup>2-</sup>. ClO3<sup>-</sup> --> Cl<sup>-</sup>. Step #2: (Not necessary for this example).Answer to Balance each of the following redox reactions occurring in basic solution. Cl2(g) ----> Cl-(aq) +ClO- (aq) Balance each. ClO3¯(aq) + Cl¯(aq) ---> Cl2(g) + ClO2(aq) [acidic sol.] Before balancing. Cl¯ (- 1) Cl2 (0) ClO2 (+4). Solution #1: 1) Half-reactions: Cl¯ ---> Cl2 ClO3¯ ---> ClO2.What are the coefficients in front of. Cr(OH)4- and ClO- in the balanced reaction? Cr(OH)4-(aq) + ClO-(aq) → CrO42-(aq) + Cl-(aq). A) Cr(OH)4- = 2, ClO- = 3.is +2, ON of Cl in ClO- is +1, ON of Pb in. PbO2 is +4 and ON for Cl in Cl- is -1. b) Reduction: ClO-(aq) → Cl-(aq) and oxidation: Pb(OH)2-. 4 (aq) →. PbO2(s).PbO2(s) + SO4<sup>2–</sup>(aq) + 4 H<sup>+</sup>(aq) + 2 e<sup>–</sup> PbSO4(s) + 2 H2O. +1.685. Au<sup>+</sup>(aq) + e <sup>–</sup> Au(s). ClO3<sup>–</sup>(aq) + 6 H<sup>+</sup>(aq) + 5 e<sup>–</sup> 1/2 Cl2(g) + 3 H2O. +1.47. BrO3<sup>–</sup> + 6 . Apr 21, 2006 . Cr(s) + HCl(aq) Cr<sup>3+</sup>(aq) + H2(g) + Cl<sup>–</sup>(aq). Mg(s) + O3(g) Mg(OH)2(s) + O2(g). 1 ). HI(aq) + ClO3<sup>–</sup>(aq) I3<sup>–</sup>(aq) + Cl2(g). Al(s) + ClO<sup>–</sup>(aq) . (b) Zn(s) + O2(g) + H2O(l) --> Zn<sup>2+</sup>(aq) + OH<sup>-</sup>(aq). (c) Fe(NO3)2(aq) + Cr2O7<sup>2-</sup>( aq) --> Fe(NO3)3 + Cr<sup>3+</sup>(aq). (a) Zn(s) + ClO<sup>-</sup>(aq) --> Zn(OH)2(s) + Cl<sup>-</sup>(aq).___ Al(s) + ___ HBr(aq) →. 11.. ___ Ba(C2H3O2)2(aq) + ___ (NH4)2SO4(aq) →. . Cl2 + 4 OH. − → 2 ClO. −. + 2 H2O + 2 e. −. + 4 OH. −. Check: Cl 2 ✓. O 2 ✓.

Oct 27, 2010 . Balance the following oxidation-reduction reactions, which occur in basic solution , using the half-reaction method. (Use the lowest possible . Cr(OH)3(s) + ClO3<sup>-</sup>(aq) --> CrO4<sup>2-</sup>(aq) + Cl<sup>-</sup>(aq) (basic). Solution: Step #1: Cr( OH)3 --> CrO4<sup>2-</sup>. ClO3<sup>-</sup> --> Cl<sup>-</sup>. Step #2: (Not necessary for this example).Answer to Balance each of the following redox reactions occurring in basic solution. Cl2(g) ----> Cl-(aq) +ClO- (aq) Balance each. ClO3¯(aq) + Cl¯(aq) ---> Cl2(g) + ClO2(aq) [acidic sol.] Before balancing. Cl¯ (- 1) Cl2 (0) ClO2 (+4). Solution #1: 1) Half-reactions: Cl¯ ---> Cl2 ClO3¯ ---> ClO2.What are the coefficients in front of. Cr(OH)4- and ClO- in the balanced reaction? Cr(OH)4-(aq) + ClO-(aq) → CrO42-(aq) + Cl-(aq). A) Cr(OH)4- = 2, ClO- = 3.is +2, ON of Cl in ClO- is +1, ON of Pb in. PbO2 is +4 and ON for Cl in Cl- is -1. b) Reduction: ClO-(aq) → Cl-(aq) and oxidation: Pb(OH)2-. 4 (aq) →. PbO2(s).PbO2(s) + SO4<sup>2–</sup>(aq) + 4 H<sup>+</sup>(aq) + 2 e<sup>–</sup> PbSO4(s) + 2 H2O. +1.685. Au<sup>+</sup>(aq) + e <sup>–</sup> Au(s). ClO3<sup>–</sup>(aq) + 6 H<sup>+</sup>(aq) + 5 e<sup>–</sup> 1/2 Cl2(g) + 3 H2O. +1.47. BrO3<sup>–</sup> + 6 . Apr 21, 2006 . Cr(s) + HCl(aq) Cr<sup>3+</sup>(aq) + H2(g) + Cl<sup>–</sup>(aq). Mg(s) + O3(g) Mg(OH)2(s) + O2(g). 1 ). HI(aq) + ClO3<sup>–</sup>(aq) I3<sup>–</sup>(aq) + Cl2(g). Al(s) + ClO<sup>–</sup>(aq) . (b) Zn(s) + O2(g) + H2O(l) --> Zn<sup>2+</sup>(aq) + OH<sup>-</sup>(aq). (c) Fe(NO3)2(aq) + Cr2O7<sup>2-</sup>( aq) --> Fe(NO3)3 + Cr<sup>3+</sup>(aq). (a) Zn(s) + ClO<sup>-</sup>(aq) --> Zn(OH)2(s) + Cl<sup>-</sup>(aq).___ Al(s) + ___ HBr(aq) →. 11.. ___ Ba(C2H3O2)2(aq) + ___ (NH4)2SO4(aq) →. . Cl2 + 4 OH. − → 2 ClO. −. + 2 H2O + 2 e. −. + 4 OH. −. Check: Cl 2 ✓. O 2 ✓.

Oct 27, 2010 . Balance the following oxidation-reduction reactions, which occur in basic solution , using the half-reaction method. (Use the lowest possible . Cr(OH)3(s) + ClO3<sup>-</sup>(aq) --> CrO4<sup>2-</sup>(aq) + Cl<sup>-</sup>(aq) (basic). Solution: Step #1: Cr( OH)3 --> CrO4<sup>2-</sup>. ClO3<sup>-</sup> --> Cl<sup>-</sup>. Step #2: (Not necessary for this example).Answer to Balance each of the following redox reactions occurring in basic solution. Cl2(g) ----> Cl-(aq) +ClO- (aq) Balance each. ClO3¯(aq) + Cl¯(aq) ---> Cl2(g) + ClO2(aq) [acidic sol.] Before balancing. Cl¯ (- 1) Cl2 (0) ClO2 (+4). Solution #1: 1) Half-reactions: Cl¯ ---> Cl2 ClO3¯ ---> ClO2.What are the coefficients in front of. Cr(OH)4- and ClO- in the balanced reaction? Cr(OH)4-(aq) + ClO-(aq) → CrO42-(aq) + Cl-(aq). A) Cr(OH)4- = 2, ClO- = 3.is +2, ON of Cl in ClO- is +1, ON of Pb in. PbO2 is +4 and ON for Cl in Cl- is -1. b) Reduction: ClO-(aq) → Cl-(aq) and oxidation: Pb(OH)2-. 4 (aq) →. PbO2(s).PbO2(s) + SO4<sup>2–</sup>(aq) + 4 H<sup>+</sup>(aq) + 2 e<sup>–</sup> PbSO4(s) + 2 H2O. +1.685. Au<sup>+</sup>(aq) + e <sup>–</sup> Au(s). ClO3<sup>–</sup>(aq) + 6 H<sup>+</sup>(aq) + 5 e<sup>–</sup> 1/2 Cl2(g) + 3 H2O. +1.47. BrO3<sup>–</sup> + 6 . Apr 21, 2006 . Cr(s) + HCl(aq) Cr<sup>3+</sup>(aq) + H2(g) + Cl<sup>–</sup>(aq). Mg(s) + O3(g) Mg(OH)2(s) + O2(g). 1 ). HI(aq) + ClO3<sup>–</sup>(aq) I3<sup>–</sup>(aq) + Cl2(g). Al(s) + ClO<sup>–</sup>(aq) . (b) Zn(s) + O2(g) + H2O(l) --> Zn<sup>2+</sup>(aq) + OH<sup>-</sup>(aq). (c) Fe(NO3)2(aq) + Cr2O7<sup>2-</sup>( aq) --> Fe(NO3)3 + Cr<sup>3+</sup>(aq). (a) Zn(s) + ClO<sup>-</sup>(aq) --> Zn(OH)2(s) + Cl<sup>-</sup>(aq).___ Al(s) + ___ HBr(aq) →. 11.. ___ Ba(C2H3O2)2(aq) + ___ (NH4)2SO4(aq) →. . Cl2 + 4 OH. − → 2 ClO. −. + 2 H2O + 2 e. −. + 4 OH. −. Check: Cl 2 ✓. O 2 ✓.

Oct 27, 2010 . Balance the following oxidation-reduction reactions, which occur in basic solution , using the half-reaction method. (Use the lowest possible . Cr(OH)3(s) + ClO3<sup>-</sup>(aq) --> CrO4<sup>2-</sup>(aq) + Cl<sup>-</sup>(aq) (basic). Solution: Step #1: Cr( OH)3 --> CrO4<sup>2-</sup>. ClO3<sup>-</sup> --> Cl<sup>-</sup>. Step #2: (Not necessary for this example).Answer to Balance each of the following redox reactions occurring in basic solution. Cl2(g) ----> Cl-(aq) +ClO- (aq) Balance each. ClO3¯(aq) + Cl¯(aq) ---> Cl2(g) + ClO2(aq) [acidic sol.] Before balancing. Cl¯ (- 1) Cl2 (0) ClO2 (+4). Solution #1: 1) Half-reactions: Cl¯ ---> Cl2 ClO3¯ ---> ClO2.What are the coefficients in front of. Cr(OH)4- and ClO- in the balanced reaction? Cr(OH)4-(aq) + ClO-(aq) → CrO42-(aq) + Cl-(aq). A) Cr(OH)4- = 2, ClO- = 3.is +2, ON of Cl in ClO- is +1, ON of Pb in. PbO2 is +4 and ON for Cl in Cl- is -1. b) Reduction: ClO-(aq) → Cl-(aq) and oxidation: Pb(OH)2-. 4 (aq) →. PbO2(s).PbO2(s) + SO4<sup>2–</sup>(aq) + 4 H<sup>+</sup>(aq) + 2 e<sup>–</sup> PbSO4(s) + 2 H2O. +1.685. Au<sup>+</sup>(aq) + e <sup>–</sup> Au(s). ClO3<sup>–</sup>(aq) + 6 H<sup>+</sup>(aq) + 5 e<sup>–</sup> 1/2 Cl2(g) + 3 H2O. +1.47. BrO3<sup>–</sup> + 6 . Apr 21, 2006 . Cr(s) + HCl(aq) Cr<sup>3+</sup>(aq) + H2(g) + Cl<sup>–</sup>(aq). Mg(s) + O3(g) Mg(OH)2(s) + O2(g). 1 ). HI(aq) + ClO3<sup>–</sup>(aq) I3<sup>–</sup>(aq) + Cl2(g). Al(s) + ClO<sup>–</sup>(aq) . (b) Zn(s) + O2(g) + H2O(l) --> Zn<sup>2+</sup>(aq) + OH<sup>-</sup>(aq). (c) Fe(NO3)2(aq) + Cr2O7<sup>2-</sup>( aq) --> Fe(NO3)3 + Cr<sup>3+</sup>(aq). (a) Zn(s) + ClO<sup>-</sup>(aq) --> Zn(OH)2(s) + Cl<sup>-</sup>(aq).___ Al(s) + ___ HBr(aq) →. 11.. ___ Ba(C2H3O2)2(aq) + ___ (NH4)2SO4(aq) →. . Cl2 + 4 OH. − → 2 ClO. −. + 2 H2O + 2 e. −. + 4 OH. −. Check: Cl 2 ✓. O 2 ✓.

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Oct 27, 2010 . Balance the following oxidation-reduction reactions, which occur in basic solution , using the half-reaction method. (Use the lowest possible . Cr(OH)3(s) + ClO3<sup>-</sup>(aq) --> CrO4<sup>2-</sup>(aq) + Cl<sup>-</sup>(aq) (basic). Solution: Step #1: Cr( OH)3 --> CrO4<sup>2-</sup>. ClO3<sup>-</sup> --> Cl<sup>-</sup>. Step #2: (Not necessary for this example).Answer to Balance each of the following redox reactions occurring in basic solution. Cl2(g) ----> Cl-(aq) +ClO- (aq) Balance each. ClO3¯(aq) + Cl¯(aq) ---> Cl2(g) + ClO2(aq) [acidic sol.] Before balancing. Cl¯ (- 1) Cl2 (0) ClO2 (+4). Solution #1: 1) Half-reactions: Cl¯ ---> Cl2 ClO3¯ ---> ClO2.What are the coefficients in front of. Cr(OH)4- and ClO- in the balanced reaction? Cr(OH)4-(aq) + ClO-(aq) → CrO42-(aq) + Cl-(aq). A) Cr(OH)4- = 2, ClO- = 3.is +2, ON of Cl in ClO- is +1, ON of Pb in. PbO2 is +4 and ON for Cl in Cl- is -1. b) Reduction: ClO-(aq) → Cl-(aq) and oxidation: Pb(OH)2-. 4 (aq) →. PbO2(s).PbO2(s) + SO4<sup>2–</sup>(aq) + 4 H<sup>+</sup>(aq) + 2 e<sup>–</sup> PbSO4(s) + 2 H2O. +1.685. Au<sup>+</sup>(aq) + e <sup>–</sup> Au(s). ClO3<sup>–</sup>(aq) + 6 H<sup>+</sup>(aq) + 5 e<sup>–</sup> 1/2 Cl2(g) + 3 H2O. +1.47. BrO3<sup>–</sup> + 6 . Apr 21, 2006 . Cr(s) + HCl(aq) Cr<sup>3+</sup>(aq) + H2(g) + Cl<sup>–</sup>(aq). Mg(s) + O3(g) Mg(OH)2(s) + O2(g). 1 ). HI(aq) + ClO3<sup>–</sup>(aq) I3<sup>–</sup>(aq) + Cl2(g). Al(s) + ClO<sup>–</sup>(aq) . (b) Zn(s) + O2(g) + H2O(l) --> Zn<sup>2+</sup>(aq) + OH<sup>-</sup>(aq). (c) Fe(NO3)2(aq) + Cr2O7<sup>2-</sup>( aq) --> Fe(NO3)3 + Cr<sup>3+</sup>(aq). (a) Zn(s) + ClO<sup>-</sup>(aq) --> Zn(OH)2(s) + Cl<sup>-</sup>(aq).___ Al(s) + ___ HBr(aq) →. 11.. ___ Ba(C2H3O2)2(aq) + ___ (NH4)2SO4(aq) →. . Cl2 + 4 OH. − → 2 ClO. −. + 2 H2O + 2 e. −. + 4 OH. −. Check: Cl 2 ✓. O 2 ✓.

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