What is the pH of a buffer solution containing 0.2 M ammonium hydroxide solution and 0.04 M ammo

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What is the pH of a buffer solution containing 0.2 M...

What is the $\mathrm{pH}$ of a buffer solution containing $0.2 \mathrm{M}$ ammonium hydroxide solution and $0.04 \mathrm{M}$ ammonium chloride solution in one-liter, using the $\mathrm{Ka}$ of ammonia as $5.75 \times 10^{-10}$ at $25^{\circ} \mathrm{C}$ ?

Key Concepts

Acid-Base Equilibrium Constants

Acid-base equilibrium constants, such as Ka for acids and Kb for bases, quantify the degree to which an acid or base dissociates in solution. These constants are fundamental in determining the strength of the acid or base and, when used with the Henderson-Hasselbalch equation, in calculating the pH of buffer systems. Converting between Ka and pKa (and similarly between Kb and pKb) is a common step in such analyses.

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation provides a direct relationship between the pH of a buffer solution and the concentrations of its conjugate acid and base along with the acid dissociation constant (pKa). This equation is invaluable for calculating the pH of both weak acid and weak base buffers under varying concentrations.

Buffer Solutions

A buffer solution is a system that resists changes in pH when small amounts of acid or base are added. It is typically composed of a weak acid and its conjugate base or a weak base and its conjugate acid. The presence of both components allows the buffer to neutralize added acids or bases by shifting the equilibrium between the two species, maintaining a relatively constant pH.

Conjugate Acid-Base Pairs

Conjugate acid-base pairs consist of two species that transform into each other by the gain or loss of a proton. In a buffer, one member of the pair reacts with added acids while the other reacts with added bases. Understanding these pairs is essential for analyzing the behavior of buffer solutions and predicting their pH.

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