Suggest a suitable reagent that can carry out each of the following oxidations or reductions. Use the data in Appendix 2  to help you.

a. The reduction of Zn²⁺ ions to Zn.

b. The oxidation of Br^– ions to Br₂.

c. The reduction of acidified SO₄^2– ions to SO₂.

d. The oxidation of Cl^– ions to Cl₂.

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Selected standard electrode potentials Electrode reaction Electrode reactlon Ag* +e- Ag Mn2+ + 2e= Mn +0.80 -1.18 Mno, + 8H* + 5e Mn2+ + 4H,0 Br, + 2e 2Br +1.07 +1.52 Ca2+ + 2e Ca -2.87 Ni24 + 2e NI -0.25 Cl, + 2e 201 NO, + 2H* + e 1 NO, + H,0 +1.36 +0.81 CIO + H,0 + 2e= - Cl+ 20H NO, + 10H* + 8e - NH, +3H,0 +0.89 +0.87 Cr2+ + 2e Cr -0.91 0,+4H* + 4e 2H,0 +1.23 Cr3+ + 3e Cr 0,+ 2H,0 + 4e =40H- -0.74 +0.40 Cr,0,7 +14H* + 6e 2Cr* + 7H,0 Pb2+ + 2e Pb +1.33 -0.13 Cut +e Cu Pbo, + 4H* + 2e - Pb2+ + 2H,0 +1.47 +0.52 Cu2+ + e= Cut +0.15 Snt + 2e Sn -0.14 Cu2+ + 2e Cu +0.34 Sn4+ + 2e Sn2+ +0.15 F,+2e"- 2F- so + 4H* + 2e = so, + 2H,0 +0.17 +2.87 Fe++ 2e - Fe -0.44 s,0,2 +2e- 25o, +2.01 Fe+ +e Fe2+ 5,0,2 + 2e= 25,0, +0.09 +0.77 Fe+ + 3e= Fe -0.04 V2+ + 2e V -1.20 2H* + 2e H, 0.00 V3++e V2+ -0.26 2H,0 + 2e VO2+ + 2H* +e V3+ + H,0 H, + 20H- +0.34 -0.83 H,0, + 2H* + 2e - 2H,0 vo,* + 2H* +e= vo2* + H,0 +1.77 +1.00 I, + 2e 21- Vo,, + 4H* + e= vo2+ + 2H,0 +1.00 +0.54 K*+e=K -2.92 Zn2+ + 2e= Zn -0.76 Mg+ + 2e Mg -2.38