Which of these equations relates the pOH of a buffer to the p𝐾𝑏 of its weak base, analogous to the Henderson–Hasselbalch equation for weak acids?
a. p𝐾𝑏=pOH+p𝐾𝑏=pOH+log[acid]/[base]
b. p𝐾𝑏=pOH−log[acid]/[base]
c. p𝐾𝑏=pOH−log[base]/[acid]
d. p𝐾𝑏=pOH+log[base]/[[acid]

검증된 단계별 안내

Identify the Henderson-Hasselbalch equation for weak acids: \( \text{pH} = \text{pK}_a + \log \left( \frac{[\text{base}]}{[\text{acid}]} \right) \).

Recognize that the analogous equation for bases involves pOH and pK_b.

The equation should relate pOH to pK_b and the ratio of concentrations of the base and its conjugate acid.

The correct form should be \( \text{pOH} = \text{pK}_b + \log \left( \frac{[\text{acid}]}{[\text{base}]} \right) \).

Match this form to the given options to find the correct answer.

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주요 개념

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Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation is a formula used to calculate the pH of a buffer solution. It relates the pH to the pKa of the weak acid and the ratio of the concentrations of the conjugate base and the weak acid. This equation can be adapted for bases, allowing for the calculation of pOH in relation to pKb and the concentrations of the acid and base components.

pOH and pKb Relationship

pOH is a measure of the hydroxide ion concentration in a solution, while pKb is the base dissociation constant that indicates the strength of a weak base. The relationship between pOH and pKb is crucial for understanding buffer systems involving weak bases. By manipulating these values, one can derive equations that express the pOH in terms of pKb and the concentrations of the acid and base.

Buffer Solutions

Buffer solutions are mixtures that resist changes in pH when small amounts of acid or base are added. They typically consist of a weak acid and its conjugate base or a weak base and its conjugate acid. Understanding how buffers work is essential for applying the Henderson-Hasselbalch equation and its variations, as they help maintain pH stability in biological and chemical systems.