Chapter 17.2, Problem 2PE

Interpretation Introduction

Interpretation:

The pH has to be calculated for $0.30MN{H}_3/0.36MN{H}_{4}Cl$ buffer system, The pH has to be calculated after adding $\text{20}\text{.0 ml of 0}\text{.050 M NaOH to 80}\text{.0 mL}$ of buffer solution.

Concept introduction:

Buffer Solutions:

Buffers are solutions that resist change in pH on dilution or on the addition of small amounts of acids or alkali.

Buffer solution must have weak acid and its salt (weak conjugate base) or weak base and it salt (weak conjugate acid)

$\text{pH}$ can be calculete by using following formula,

  $\text{pH}\text{=}p{K}_b+\log \frac{(base)}{(salt)}$

  ${\text{pK}}_{\text{b}}\text{ = -log}\left[{\text{K}}_{\text{b}}\right]$

The acid dissociation constant $\left(K_b\right)$ is the equilibrium constant of the dissociation reaction of an acid.