Calculate the number of milliliters of 0.709 M KOH required to precipitate all of the Co2+ ions in 116 mL of 0.502 M Coso, solution as Co(OH)2. The equation for the reaction is:
CosO4(aq) + 2KOH(aq) —Co(OH)2(8) + K2SO4(aq)
mL KOH

Answerthe half-reaction having the greatest tendency to occur at the anode:     i₂(aq) + 2e⁻  ⇄ 2i⁻  ;   e = +0.53 v======oxidation occurs at the anode. we must therefore find the half-reaction with the greatest tendency to oxidize.the given values of e are reduction potentials (the form of the half-reactions are of reduction).the lower the reduction potential, the higher the potential to oxidize. the half-cell with the lowest reduction potential will have the greatest tendency to oxidize at the anode.the half-reaction having the greatest tendency must be    i₂(aq) + 2e⁻  ⇄ 2i⁻    e = +0.53 vbecause its reduction potential is the lowest out of the three.

Ibelieve the answer is balance! hope my answer has you : )

Good job high

Sorry cant answer: c