Calculate the pH of a 0.1 M sodium acetate s | vedclass

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(A) Sodium acetate $(CH_3COONa)$ is a salt of a weak acid $(CH_3COOH)$ and a strong base $(NaOH)$.It undergoes anionic hydrolysis: $CH_3COO^- + H_2O \

Vedclass · Accepted Answer

$8.87$

Vedclass · Answer

(A) Sodium acetate $(CH_3COONa)$ is a salt of a weak acid $(CH_3COOH)$ and a strong base $(NaOH)$.It undergoes anionic hydrolysis: $CH_3COO^- + H_2O ightleftharpoons CH_3COOH + OH^-$.The $pH$ of a salt of a weak acid and a strong base is given by the formula: $pH = \frac{1}{2} [pK_w + pK_a + \log C]$.Given: $C = 0.1 \ M$,$K_a = 1.8 	imes 10^{-5}$,$K_w = 10^{-14}$.$pK_a = -\log(1.8 	imes 10^{-5}) = 5 - \log(1.8) = 5 - 0.255 = 4.745$.$pK_w = 14$.$pH = \frac{1}{2} [14 + 4.745 + \log(0.1)]$.$pH = \frac{1}{2} [18.745 - 1] = \frac{1}{2} [17.745] = 8.8725 \approx 8.87$.

Calculate the $pH$ of a $0.1 \ M$ sodium acetate solution. Given: $K_a$ for $CH_3COOH = 1.8 \times 10^{-5}$.

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