An unknown diprotic acid requires 28.20 mL of 0.104 M NaOH to completely neutralize a 1.400-g sample. Calculate the approximate molar mass of the acid.
A. 239 g/mol
B. 341 g/mol
C. 682 g/mol
D.955 g/mol
E. 477 g/mol

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.

Ithink the answer is d.

Answerionic bond imfs are stronger than covalent;