Consider an aqueous solution that is 0.1 M in HCl and 0.1 M in (). What is the total concentration i — Ionic Equilibrium Chemistry Question
Question
Consider an aqueous solution that is 0.1 M in HCl and 0.1 M in $CH_3COOH$ ($K_a = 1.8 \times 10^{-5}$). What is the total $[H^+]$ concentration in the solution?
Answer: B
💡 Solution & Explanation
The strong acid (HCl) completely dissociates, providing 0.1 M $H^+$. This massive $H^+$ concentration forcefully suppresses the ionization of the weak acid ($CH_3COOH$) via the common ion effect. Total $[H^+] \approx [HCl] = 0.1 \text{ M}$.
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