What is the pH of a liter buffer solution containing 0.5 M boric acid and 0.25 sodium borate per

step 1 Anytime you're asked to determine the pH of a buffer solution, as in problem 811, you'll be usin

What is the pH of a liter buffer solution containing 0.5 M...

What is the $\mathrm{pH}$ of a liter buffer solution containing $0.5 \mathrm{M}$ boric acid and 0.25 sodium borate per liter? The $\mathrm{pK}_{\mathrm{a}}$ of boric acid is 9.24 at $25^{\circ} \mathrm{C}$.

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Key Concepts

Acid Dissociation Constant (pKa)

The pKa is a numerical value that represents the strength of a weak acid, indicating its tendency to donate protons. In the context of buffer solutions, the pKa is crucial because it determines the optimal pH range in which the buffer can effectively neutralize added acids or bases. A buffer works best when the pH is close to the pKa value of the weak acid present.

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation is a mathematical relationship used to estimate the pH of a buffer solution. It relates the pH to the pKa (acid dissociation constant) of the weak acid and the ratio of the concentrations of the conjugate base to the weak acid. This equation simplifies the understanding of how the buffer components interact to maintain pH balance.

Buffer Solution

A buffer solution is a system that resists pH changes upon the addition of small amounts of acids or bases. It typically consists of a weak acid and its conjugate base, or a weak base and its conjugate acid. Buffers work by neutralizing added acids and bases through equilibrium reactions, maintaining a relatively stable pH in the solution.

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