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The acid ionization constant for benzoic acid (C6H5COOH) is 6.46 × 10−5 . Compare the percent ionization of 1.00 M benzoic acid in water with its percent ionization in 0.500 M sodium benzoate solution. Support your comparison with calculations similar to those in Model 1.

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Answer:

The percent ionization decreases because the increase in the concentration of C₆H₅COO⁽⁻⁾ causes the equilibrium to shift to the left towards the formation of acid (Le Chatelier's Principle).

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The percent ionization decreases because the increase in the concentration of C₆H₅COO⁽⁻⁾ causes the equilibrium to shift to the left towards the formation of acid (Le Chatelier's Principle).

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