Buffer capacity is defined as the number of moles of a...

Buffer capacity is defined as the number of moles of a strong acid or strong base required to change the $\mathrm{pH}$ of $1 \mathrm{~L}$ of the buffer solution by one unit. What is the buffer capacity of a solution that is $0.10 \mathrm{M}$ in acetic acid and $0.10 \mathrm{M}$ in sodium acetate?

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Key Concepts

Buffer Capacity

Buffer capacity refers to the amount of strong acid or base that must be added to one liter of a buffer solution to change its pH by one unit. It quantifies the resistance of the buffer solution against pH changes and depends on the concentrations of the buffer components and their relative proportions.

Buffer Solutions

Buffer solutions are mixtures of a weak acid and its conjugate base, or a weak base and its conjugate acid, that resist changes in pH when small amounts of strong acid or base are added. They work by neutralizing added acids or bases, thereby maintaining a relatively constant pH in the solution.

Acid-Base Equilibrium

Acid-base equilibrium involves the reversible dissociation of a weak acid into its conjugate base and hydrogen ions. In buffer systems, this equilibrium is crucial because it allows the solution to absorb additions of acids or bases by shifting the equilibrium position, thereby minimizing pH changes.

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation is used to relate the pH of a buffer solution to the pKa of the acid and the ratio of the concentrations of the conjugate base to the weak acid. It provides a convenient way to calculate the pH of a buffer solution and to understand how changes in the component concentrations affect the pH.

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