Chemistry > Ionic Equilibrium > 7.0 Buffer Solution
Ionic Equilibrium
1.0 Reversible Reaction
2.0 $pH$ Scale
3.0 Arrehenius Theory of Electrolyte Ionization (Dissociation)
4.0 Ionization of Water
5.0 Determination of $pH$ of acids and bases
5.1 Strong acid
5.2 Weak acid
5.3 Strong Acid + Weak Acid
5.4 Two weak acids
5.5 Dibasic and polyprotic weak acids
6.0 Salt Hydrolysis
6.1 Salts of weak acid + strong base
6.2 Salt of weak base + strong acid
6.3 Salt of weak acid and weak base
7.0 Buffer Solution
8.0 Solubility and Solubility Product
7.2 Basic buffer
5.2 Weak acid
5.3 Strong Acid + Weak Acid
5.4 Two weak acids
5.5 Dibasic and polyprotic weak acids
6.2 Salt of weak base + strong acid
6.3 Salt of weak acid and weak base
Aqueous solution of mixture of weak base and salt of the same weak base with any type of strong acid is called basic buffer. For example,
$$N{H_4}OH + N{H_4}Cl$$
$$N{H_4}OH \rightleftharpoons N{H_4}^ + + O{H^ - }$$$$N{H_4}Cl \rightleftharpoons N{H_4}^ + + C{l^ - }$$
Case 1. When mixing of acid ${H^ + }$
$$N{H_4}OH + {H^ + } \rightleftharpoons N{H_4}^ + + {H_2}O$$
Case 2. When mixing of base $O{H^ - }$
$$N{H_4}^ + + O{H^ - } \rightleftharpoons N{H_4}OH$$
For a basic buffer, $$pOH = p{K_b} + \log \frac{{\left[ {Salt} \right]}}{{\left[ {Base} \right]}}$$
