The addition of sodium acetate to acetic acid solution will...

The addition of sodium acetate to acetic acid solution will cause
(a) increase in its $\mathrm{pH}$ value
(b) decrease in its $\mathrm{pH}$ value
(c) no change in $\mathrm{pH}$ value
(d) change in $\mathrm{pH}$ which cannot be predicted

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Key Concepts

Buffer Solutions

A buffer solution is a system that resists changes in pH when small amounts of acid or base are added. Typically, it consists of a weak acid and its conjugate base (or a weak base and its conjugate acid). In the context of the given problem, acetic acid and sodium acetate form a buffer system that stabilizes the pH of the solution.

Common Ion Effect

The common ion effect describes the shift in equilibrium that occurs when an ion common to the equilibrium is added to the solution. In this case, adding sodium acetate increases the concentration of the acetate ion, which shifts the acetic acid dissociation equilibrium, resulting in an increase in pH.

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation is a formula that relates the pH of a buffer solution to the pKa of the acid and the ratio of the concentrations of its conjugate base and acid. It is useful for quantifying the change in pH upon the addition of a conjugate base like sodium acetate to acetic acid.

Acid-Base Equilibrium

Acid-base equilibrium involves the reversible reaction between an acid and its conjugate base in solution. The addition of a conjugate base, such as the acetate ion from sodium acetate, alters this equilibrium by reducing the concentration of hydrogen ions, which leads to an increase in pH.

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