What is the pH of a buffer solution containing 0.005 M oxalic acid and 0.05 M potassium oxalate

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What is the pH of a buffer solution containing 0.005 M...

What is the $\mathrm{pH}$ of a buffer solution containing $0.005 \mathrm{M}$ oxalic acid and $0.05 \mathrm{M}$ potassium oxalate solution in one-liter? The dissociation constant of oxalic acid is $6.5 \times 10^{-2}$ at $25^{\circ} \mathrm{C}$.

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Key Concepts

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 acid or base are added. They are critical in maintaining a stable pH in many chemical and biological systems.

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation provides a convenient way to estimate the pH of a buffer solution using the pKa of the weak acid and the ratio of the concentrations of the conjugate base to the acid. This equation highlights how the balance between these two components determines the overall pH of the buffer.

Acid Dissociation Constant (Ka) and pKa

The acid dissociation constant (Ka) quantifies the extent to which a weak acid dissociates in water, and the pKa, which is the negative base-10 logarithm of Ka, offers a more manageable numerical value for acid strength. These concepts are essential for calculating the pH of a buffer since they reveal the acid’s propensity to donate protons.

pH is a measure of the acidity or basicity of a solution, defined as the negative logarithm of the hydrogen ion concentration. It indicates how acidic or basic a buffer or any solution is, and is a fundamental property in chemistry and biology used to describe the environment of a reaction or biological system.

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