1. What is the pH of a 0.01M solution of phthalic acid(H2P)
2. What is the pH of a 0.01M solution of potassium acid phthalate(KHP)?
3. What is the pH of a solution that is 0.20M in H2P and 0.1M inKHP?

H2P Ka1 = 1.2x10^-3
Ka2 = 3.9x10^-6

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Calculate the pH of the following solutions.

a) A solution containing 0.0218 M maleic acid and 0.0299 M disodium maleate. The Ka values for maleic acid are 1.20 ï¿½ 10-2 (Ka1) and 5.37 ï¿½ 10-7 (Ka2).

b) A solution containing 0.0412 M phthalic acid and 0.023 M potassium hydrogen phthalate. The Ka values for phthalic acid are 1.12 ï¿½ 10-3 (Ka1) and 3.90 ï¿½ 10-6 (Ka2).

The hydrogen phthalate ion, C₈H₅O₄-, is a weak acid with K_a = 3.91×10^-6.

What is the pH of a 0.050 M solution of potassium hydrogen phthalate, KC₈H₅O₄? Note: To find the pH for a solution of the anion, we must take into account that the ion is amphiprotic. It can be shown that, for most cases of amphiprotic ions, the H₃O⁺ concentration is