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NemiM [27]
3 years ago
7

A weak acid. What is the pH of a 0.1 M solution of acetic acid (pKa = 4.75)?

Chemistry
1 answer:
Rashid [163]3 years ago
3 0

Answer:

pH of acetic acid solution is 2.88

Explanation:

pK_{a}=4.75

or, -log(K_{a})=4.75

or, K_{a}=10^{-4.75}=1.78\times 10^{-5}

We have to construct an ICE table to determine concentration of H^{+} and corresponding pH. Initial concentration of acetic acid is 0.1 M.

CH_{3}COOH\rightleftharpoons CH_{3}COO^{-}+H^{+}

I(M):  0.1                            0                    0

C(M): -x                              +x                 +x

E(M): 0.1-x                         x                    x

So, \frac{[CH_{3}COO^{-}][H^{+}]}{[CH_{3}COOH]}=K_{a}

or, \frac{x^{2}}{0.1-x}=1.78\times 10^{-5}

or, x^{2}+(1.78\times 10^{-5}\times x)-(1.78\times 10^{-6})=0

So, x=\frac{-(1.78\times 10^{-5})+\sqrt{(1.78\times 10^{-5})^{2}+(4\times 1\times 1.78\times 10^{-6})}}{2\times 1}(M)

so, x=1.33\times 10^{-3}M

Hence pH=-log[H^{+}]=-log(1.33\times 10^{-3})=2.88

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