The scenes below depict the relative concentrations of h3po4, h2po4− , and hpo42− during a titration with aqueous naoh, but they are out of order. (phosphate groups are purple, hydrogens are blue, and na+ ions and water molecules are not shown.) (a) list the scenes in the correct order. first last (b) what is the ph in the correctly ordered second scene (ka1 = 7.2 × 10−3, ka2 = 6.3 × 10−8)? ph = (c) if it requires 28.00 ml of the naoh solution to reach this scene, how much more is needed to reach the last scene? ml naoh

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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.

Answersublimation;