The concentration of acetate ions in 1 M acetic acid (Ka=2 ×10^-5) solution containing 0.1 M-HCl

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The concentration of acetate ions in 1 M acetic acid (Ka=2...

The concentration of acetate ions in $1 \mathrm{M}$ acetic acid $\left(K_{\mathrm{a}}=2 \times 10^{-5}\right)$ solution containing $0.1 \mathrm{M}-\mathrm{HCl}$ is (a) $2 \times 10^{-1} \mathrm{M}$ (b) $2 \times 10^{-3} \mathrm{M}$ (c) $2 \times 10^{-4} \mathrm{M}$ (d) $4.4 \times 10^{-3} \mathrm{M}$c

The concentration of acetate ions in $1 \mathrm{M}$ acetic acid $\left(K_{\mathrm{a}}=2 \times 10^{-5}\right)$ solution containing $0.1 \mathrm{M}-\mathrm{HCl}$ is
(a) $2 \times 10^{-1} \mathrm{M}$
(b) $2 \times 10^{-3} \mathrm{M}$
(c) $2 \times 10^{-4} \mathrm{M}$
(d) $4.4 \times 10^{-3} \mathrm{M}$c

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Key Concepts

Acid Dissociation Equilibrium

This concept explains how weak acids only partially ionize in solution to produce their conjugate base and hydrogen ions. The degree of ionization is described by the acid dissociation constant (Ka), which quantifies the equilibrium between the undissociated acid and its dissociated ions. The equilibrium expression allows chemists to predict the concentrations of species in the solution under various conditions.

Common Ion Effect

The common ion effect is the phenomenon where the addition of an ion that is common to the equilibrium system causes the equilibrium to shift, thereby decreasing the ionization of a weak acid or base. In the context of weak acid solutions, the presence of an added strong acid or a salt containing the conjugate base can significantly suppress the formation of additional ions, altering the concentrations predicted by the initial equilibrium.

Equilibrium Constant (Ka) Understanding

Understanding the equilibrium constant is crucial as it reflects the relative strengths of acids by indicating the extent to which the acid dissociates in solution. A small Ka value implies that the acid is weak and only a small fraction ionizes, which becomes especially significant when external sources of hydrogen ions are introduced, shifting the equilibrium further towards the undissociated acid.

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