Question

write balanced net ionic equations for the following electrolysis reactions using platinum electrodes 1)aqueous potassium fluoride 2) aqueous nickle (II) nitrate 3)molten aluminum oxide 4)aqueous cesium bromide 5)aqueous chromium (III) iodide 6)aqueous magnesium sulfide 7)aqueous ammonium chloride 8)molten lithium fluoride 9)aqueous gold (III) acetate 10)aqueous cobalt (II) bromide

Please explain step by step, thanks a lot

I only need question #4-#10

Answer 1

4)aqueous cesium bromide

CsBr (aq)

in aqueous solution of CsBr contains four ions Cs+ , H+ , Br- , OH-

now between cations H+ and Cs+ lowest discharge potentila for H+ than Cs+

so at cathode H2 gas liberated

cathode reaction :

2H+ + 2e- -----------------> H2 (g)

now two anions , OH- and Br - between these two Br- has lowest discharge potential

anode reaction :

2 Br- --------------------> Br2 (g) + 2e-

10)aqueous cobalt (II) bromide

here Co+2 and H+ ions , Br- and OH- are present .

anode reaction : H+ has lower discharge potential

2H+ + 2e- --------------------> H2 (g)

cathode reaction :   Br- has lower discharge potential

2Br- ---------------------> Br2 (g)