MCAT General Chemistry Question 291: Answer and Explanation
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Question: 291
4. In the dissociation of phosphoric acid, the trend Ka1 > Ka2 > Ka3 is predominantly due to:
- A. an equilibrium shift towards the reactants side in Reactions 2 and 3 due to the release of H+ in Reaction 1.
- B. a smaller radius in the H+ liberated in Reaction 1 compared to that in Reactions 2 and 3.
- C. a slower rate of reaction after subsequent ionizations.
- D. an increasing influence of the anion after subsequent ionizations.
Correct Answer: D
Explanation:
D Generation of H+ in Reaction 1 is coupled with a release of H2PO4-. Both the product and reactant sides of Reaction 2 are increased proportionally, causing no shift in equilibrium (eliminate choice A). Atomic radius is a function of an atom's position in the periodic table. Thus, the radius of H+ is the same in all three reactions, eliminating choice B. Equilibrium constants have no relationship to reaction rates, so choice C can be eliminated. The Ka values progressively decrease when removing a proton from a polyprotic acid because it is more difficult to remove a proton from an anion compared to a neutral molecule. In subsequent ionizations, the anion becomes more negative, resulting in greater difficulty liberating a positively charged H+ ion.