3. Add the equations of the following redox reactions (in electronic and
ionic-electronic forms): (a) Ni(OH)2 Br2 NaOH; (b) Al KNO3 KOH; (c) Na2SnO2 Bi(OH)3;
(d) Mn(NO3)2 KMnO4 H2O; (e) KMnO4 KBr H2SO4. Indicate the oxidizing agent, reducing agent and medium (pH) of the solution. Write down the standard redox potentials of the pairs.

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