A buffer is made by dissolving 12.5 g of sodium dihydrogen phosphate, NaH2 PO4, and 15.0 g of

step 1 In order to find the pH of the buffer, we use the Henderson -Hausen -Hauselbach equation. You fi

A buffer is made by dissolving 12.5 g of sodium dihydrogen...

A buffer is made by dissolving $12.5 \mathrm{~g}$ of sodium dihydrogen phosphate, $\mathrm{NaH}_{2} \mathrm{PO}_{4}$, and $15.0 \mathrm{~g}$ of disodium hydrogen phosphate, $\mathrm{Na}_{2} \mathrm{HPO}_{4},$ in a liter of solution. What is the $\mathrm{pH}$ of the buffer?

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Key Concepts

Buffer Solution

A buffer solution is one that resists changes in pH when small amounts of acid or base are added. It typically contains a weak acid and its conjugate base (or a weak base and its conjugate acid), allowing the system to maintain a relatively stable pH by shifting equilibrium according to Le Chatelier’s principle.

Acid–Base Equilibrium

Acid–base equilibrium involves the reversible dissociation of weak acids into hydrogen ions and their conjugate bases. Understanding this equilibrium is essential for predicting how changes in concentrations of the acid or its conjugate base will influence the overall pH of a solution.

Henderson–Hasselbalch Equation

The Henderson–Hasselbalch equation provides a convenient way to calculate the pH of a buffer solution. It relates the pH to the pKa of the weak acid and the ratio of the molar concentrations of the conjugate base and the acid, making it a central tool in buffer calculations.

Molar Conversions

Molar conversions are used to convert the mass of substances to moles using their molar masses. This conversion is fundamental in preparing solutions of known concentration and is critical for determining the precise amounts of acid and conjugate base present in buffer calculations.

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