Solution of an acid and it's anion (that is, it's conjugate base) or of a base and it's common cation are buffered. When we add a small amount of acid or base to any one of them, the pH of solution changes very little. pH of buffer solution can be computed as
For acidic buffer : pH = pK a + log 
For basic buffer : pOH = pK b + log 
It is generally accepted that a solution has useful buffer capacity (pH change resisting power) provided that the value of [salt or conjugate base] / [acid] for acidic buffer lies within the range of 1 : 10 to 10 : 1. Buffer capacity is maximum when [conjugate base] = [acid]
(i) Select incorrect statement –
Text Solution
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(i) , ,
Sol. when we add small amount of NaOH in acidic
buffer solution, pOH is increased, when we add small
amount of water in acidic buffer solution, pH o
f solution is decreases, when 100 ml of 0.2 M
CH 3 COOH react with 200 ml of 0.1 M NaOH buffer
solution is formed.
(ii) ,
Sol. HCOOH + HCOONa, Na 2 CO 3 + NaHCO 3
(iii) ,
Sol. pH = pK a + log 
∴ 
= 2
Let volume of acid is V ml
= 2 ⇒ V = 200 ml
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