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HC3H5O2(aq)+H2O(l)⇄H3O+(aq)+C3H5O2−(aq)pKa=4.87The acid ionization equilibrium for HC3H5O2 is represented by the equation above. A mixture of 1.00L of 0.100MHC3H5O2 and 0.500L of 0.100MNaOH will produce a buffer solution with a pH=4.87. If the NaOH solution was mislabeled and was 1.00M instead of 0.100M, which of the following would be true?AThe pHpH of the resulting solution would still be 4.87 because buffer solutions regulate changes in pHpH regardless of how much NaOHNaOH is added.BThe pHpH of the resulting solution would be somewhat higher than 4.87 because adding NaOHNaOH that is 10 times more concentrated makes the concentration of the conjugate base 10 times larger.CThe pHpH of the resulting solution would be much higher than 4.87 because the weak acid would be completely neutralized by the larger amount of NaOHNaOH added.DThe pHpH of the resulting solution would still be 4.87 because the solutio

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