Question

Henderson-Hasselbalch equation among the following is :

• A. $pH=\frac{1}{2}p{K}_a-logC$
• B. $pOH=\frac{1}{2}p{K}_b-logC$
• C. $pH=p{K}_a+\frac{\left[salt\right]}{\left[acid\right]}$
• D. $K_h=\frac{K_w}{K_a\times K_b}$

Answer 1

The correct option is C $pH=p{K}_a+\frac{\left[salt\right]}{\left[acid\right]}$

The Henderson–Hasselbalch equation describes the derivation of $pH$ as a measure of acidity (using $p{K}_a$, the negative log of the acid dissociation constant) in biological and chemical systems. The equation is also useful for estimating the pH of a buffer solution and finding the equilibrium pH in acid-base reactions.

Henderson's Equations is :

$pH=p{K}_a+\frac{\left[salt\right]}{\left[acid\right]}$