The ionization constant of benzoic acid is 6.46 × 10^–5 and K_sp for silver benzoate is 2.5 × 10^–13. How many times is silver benzoate more soluble in a buffer of pH 3.19 compared to its solubility in pure water?

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Solution

Since pH = 3.19,

Let the solubility of C₆H₅COOAg be x mol/L.

Then,

Thus, the solubility of silver benzoate in a pH 3.19 solution is 1.66 × 10^–6 mol/L.

Now, let the solubility of C₆H₅COOAg be x’ mol/L.

Hence, C₆H₅COOAg is approximately 3.317 times more soluble in a low pH solution.

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The ionization constant of benzoic acid is $6.46 \times 10^{- 5}$ and Ksp for silver benzoate is $2.5 \times 10^{- 13}$ . How many times is silver benzoate more soluble in a buffer of pH 3.19 compared to its solubility in pure water?

The ionization constant of benzoic acid is 6.46 x 10^-5 and K_sp for silver benzoate is 2.5 x 10^-13. How many times is silver benzoate more soluble in a buffer of pH 3.19 as compared to its solubility in pure water?

Q. The ionization constant of benzoic acid is