What is the concentration of acetate ions in | vedclass

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(D) Acetic acid $(CH_3COOH)$ is a weak acid that dissociates as: $CH_3COOH \rightleftharpoons CH_3COO^- + H^+$. The dissociation constant is given by

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$2 	imes 10^{-6} \, M$

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(D) Acetic acid $(CH_3COOH)$ is a weak acid that dissociates as: $CH_3COOH ightleftharpoons CH_3COO^- + H^+$. The dissociation constant is given by $K_a = \frac{[CH_3COO^-][H^+]}{[CH_3COOH]}$. Since $HCl$ is a strong acid,it dissociates completely: $HCl ightarrow H^+ + Cl^-$. The concentration of $H^+$ ions from $HCl$ is $1.0 \, M$. Due to the common ion effect,the dissociation of acetic acid is suppressed,so $[CH_3COOH] \approx 0.1 \, M$ and $[H^+] \approx 1.0 \, M$. Substituting these values into the $K_a$ expression: $2 	imes 10^{-5} = \frac{[CH_3COO^-] 	imes 1.0}{0.1}$. Solving for $[CH_3COO^-]$: $[CH_3COO^-] = 2 	imes 10^{-5} 	imes 0.1 = 2 	imes 10^{-6} \, M$.

What is the concentration of acetate ions in a solution containing $0.1 \, M$ acetic acid and $1.0 \, M \, HCl$? $[K_a = 2 \times 10^{-5}]$

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