A buffer consists of 0.22 M KHCO3 and 0.37 M K2 CO3 Carbonic acid is a diprotic acid with Kal=4.

step 1 Polyprotic acids have multiple hydrogen atoms that they can lose, so they can act as buffers in

A buffer consists of 0.22 M KHCO3 and 0.37 M K2 CO3 Carbonic...

$\mathrm{A}$ buffer consists of 0.22 $\mathrm{M} \mathrm{KHCO}_{3}$ and 0.37 $\mathrm{M} \mathrm{K}_{2} \mathrm{CO}_{3}$ Carbonic acid is a diprotic acid with $K_{\mathrm{al}}=4.5 \times 10^{-7}$ and $K_{\mathrm{a} 2}=$ $4.7 \times 10^{-11} .$ (a) Which $K_{\mathrm{a}}$ value is more important to this buffer? (b) What is the buffer pH?

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Key Concepts

Henderson–Hasselbalch Equation

The Henderson–Hasselbalch equation provides a convenient relation between the pH of a buffer solution, the pKa of the acid, and the ratio of the concentrations of the conjugate base to the acid. It is widely used to estimate the pH of buffer solutions where equilibrium between the acid and base forms is established.

Diprotic Acid Chemistry

Diprotic acids are capable of donating two protons, undergoing two distinct dissociation steps, each characterized by its own acid dissociation constant (Ka1 and Ka2). In buffer systems involving diprotic acids, identifying the relevant dissociation step is crucial for accurate pH calculations.

Buffer Solutions

Buffer solutions are mixtures of a weak acid and its conjugate base (or a weak base and its conjugate acid) that resist changes in pH when small amounts of an acid or base are added. They maintain a relatively constant pH due to the equilibrium between the acid and base forms.

Acid Dissociation Constant (Ka)

The acid dissociation constant, Ka, quantifies the strength of an acid by measuring the extent to which it donates protons in solution. It plays a critical role in determining the position of the acid–base equilibrium, which is essential for understanding buffer action.

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