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Liono4ka [1.6K]
3 years ago
9

Farmers who raise cotton once used arsenic acid, H₃AsO₄, as a defoliant at harvest time. Arsenic acid is a polyprotic acid with

Ka₁ = 2.5 × 10⁻⁴, Ka₂ = 5.6 × 10⁻⁸, and Ka₃ = 3 × 10⁻¹³. What is the pH of a 0.500 M solution of arsenic acid?
Chemistry
1 answer:
Stels [109]3 years ago
6 0

Explanation:

The reaction equation will be as follows.

      H_{3}AsO_{4} \rightleftharpoons H_{2}AsO^{-}_{4} + H^{+}

Hence, the expression for K_{a} is as follows.

            K_{a} = \frac{[H_{2}SO^{-}_{4}][H^{+}]}{[H_{3}AsO_{4}]}

Let us assume that the concentration of both [H_{2}AsO^{-}_{4}] and [H^{+}] is x.

           2.5 \times 10^{-4} = \frac{x \times x}{0.5}

                          x = 0.01118034

This means that the concentration of [H^{+}] is 0.01118034.

Since, we know that the relation between pH and concentration of hydrogen ions is as follows.

              pH = -log [H^{+}]

                    = -log (0.01118034)

                    = 1.958

Thus, we can conclude that the pH of a 0.500 M solution of arsenic acid is 1.958.

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