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Strong and Weak Acids and Bases

Calculate the...

Question

Calculate the concentration of H3O+ ions in a mixture of 0.02M acetic acid and 0.2M sodium acetate. Given that ionization constant (Ka) for acetic acid is 1.8 * 10^-5.

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Solution

$A c c o r d i n g t o H e n d e r s o n e q u a t i o n p H = p K_{a} + \log \frac{[s a l t]}{[a c i d]} p K_{a} = - \log K_{a} = - \log [1.8 \times 10^{- 5}] = 5 \log 10 - \log 1.8 = 5 - 0.2553 = 4.7447 p H = 4.7447 + \log \frac{0.2}{0.02} = 5.7447 - \log [H^{+}] = 5.7447 M [H^{+}] = a . \log (- 5.7447) = a . \log (- 6 + 0.2553) = 1.8 \times 10^{- 6} M$

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