Which of the following compounds can form a buffer solution? a. Na2 HPO4 and NaH2 PO4 b. HCl and

step 1 Dear students, in problem 14 of chapter 5, we have asked that which of the following compound ca

Which of the following compounds can form a buffer solution?...

Which of the following compounds can form a buffer solution? a. $\mathrm{Na}_{2} \mathrm{HPO}_{4}$ and $\mathrm{NaH}_{2} \mathrm{PO}_{4}$ b. $\mathrm{HCl}$ and $\mathrm{NH}_{4} \mathrm{Cl}$ c. $\mathrm{CH}_{3} \mathrm{COOH}$ and $\mathrm{HCOOH}$ d. $\mathrm{Na}_{3} \mathrm{PO}_{4}$ and $\mathrm{NaOH}$

Which of the following compounds can form a buffer solution?
a. $\mathrm{Na}_{2} \mathrm{HPO}_{4}$ and $\mathrm{NaH}_{2} \mathrm{PO}_{4}$
b. $\mathrm{HCl}$ and $\mathrm{NH}_{4} \mathrm{Cl}$
c. $\mathrm{CH}_{3} \mathrm{COOH}$ and $\mathrm{HCOOH}$
d. $\mathrm{Na}_{3} \mathrm{PO}_{4}$ and $\mathrm{NaOH}$

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Key Concepts

Buffer Solution

A buffer solution is one that resists large changes in pH when small amounts of an acid or base are added. This resistance is achieved by having a mixture of a weak acid and its conjugate base, or a weak base and its conjugate acid, which together neutralize added acids or bases.

Conjugate Acid-Base Pair

A conjugate acid-base pair consists of two chemical species that differ by one proton; the weak acid donates a proton to become its conjugate base, and the weak base accepts a proton to become its conjugate acid. This pairing is fundamental to buffer systems since it allows the solution to counteract changes in pH.

Henderson-Hasselbalch Equation

The Henderson-Hasselbalch equation relates the pH of a buffer solution to the acid dissociation constant (pKa) and the ratio of the concentrations of the conjugate base to the weak acid. It provides a useful means for calculating the expected pH of a buffer, illustrating how the balance between the acid and the base components determines pH stability.

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