The p Ka of certain weak acid is 4.0 . What should be the...

The $\mathrm{p} K_{\mathrm{a}}$ of certain weak acid is $4.0 .$ What should be the salt to acid ratio if we have to prepare a buffer with $\mathrm{pH}=5$ using the acid and of its salts?
(1) $4: 5$
(2) $5: 4$
(3) $10: 1$
(4) $1: 10$

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Key Concepts

Buffer Solutions

Buffer solutions consist of a weak acid and its conjugate base (or a weak base and its conjugate acid) that work together to maintain a relatively constant pH when small amounts of acid or base are added. They are essential in many chemical and biological systems for stabilizing pH levels.

Acid Dissociation Constant (pKa)

The acid dissociation constant, represented as pKa, quantifies the strength of a weak acid by measuring its tendency to donate protons. A lower pKa indicates a stronger acid, and this value is crucial when analyzing buffer solutions and predicting their behavior.

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation is a practical tool in acid-base chemistry that relates the pH of a solution to the pKa of the acid and the ratio of the concentrations of its conjugate base to the acid. It allows for straightforward calculations to determine the requisite proportions to achieve a desired pH.

Conjugate Acid-Base Ratio

The ratio of a conjugate base to its corresponding weak acid in a buffer solution is pivotal in setting the solution's pH, as dictated by the Henderson-Hasselbalch equation. Adjusting this ratio enables the fine-tuning of a buffer's pH for various applications.

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