How many moles of sodium hypobromite (NaBrO) should be added...

How many moles of sodium hypobromite (NaBrO) should be added to $1.00$ L of $0.050 M$ hypobromous acid (HBrO) to form a buffer solution of $\mathrm{pH}$ 9.15? Assume that no volume change occurs when the $\mathrm{NaBrO}$ is added.

Key Concepts

Buffer Solutions

A buffer solution is a mixture of a weak acid and its conjugate base (or a weak base and its conjugate acid) that resists changes in pH when small amounts of acid or base are added. This property allows buffers to maintain a relatively constant pH under various conditions, which is critical in many chemical and biological systems.

Henderson–Hasselbalch Equation

The Henderson–Hasselbalch equation is used to relate the pH of a buffer solution to the pKa of the weak acid and the ratio of the concentrations of the conjugate base to the acid. It is a convenient tool for designing buffer systems and calculating the amounts of reagents needed to achieve a desired pH.

Molarity and Mole Calculations

Molarity is a measure of the concentration of a substance in a solution, defined as the number of moles of solute per liter of solution. Understanding how to convert between moles and molar concentrations is essential for preparing solutions and calculating the exact amounts of substances required in chemical reactions or buffer preparations.

Acid–Base Equilibrium

Acid–base equilibrium involves the balance between the dissociation of a weak acid into its conjugate base and a proton, governed by the acid’s dissociation constant (Ka) or its pKa. This equilibrium is crucial for understanding the behavior of buffer systems and predicting how they will respond to the addition of acids or bases.

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