Consider the reaction between sodium hydroxide and acetic acid: NaOH(aq) HC2H3 02 (9) H2O(0) Nac2 H3 02 (aq)
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A 25,0 mL sample of acetic acid (HC2H302) of unknown molarity is titrated with 12.1ml. of 0.65 M NaOH. What is the molarity of the acetic acid solution?
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c. electrical charges of ionic bonds.

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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.

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