Answer:
According to Le-chatelier principle, equilibrium will shift towards left to minimize concentration of [tex]OH^{-}[/tex] and keep same equilibrium constant
Explanation:
In this buffer following equilibrium exists -
[tex]NH_{3}(aq.)+H_{2}O(l)\rightleftharpoons NH_{4}^{+}(aq.)+OH^{-}(aq.)[/tex]
So, [tex]OH^{-}[/tex] is involved in the above equilibrium.
When a strong base is added to this buffer, then concentration of [tex]OH^{-}[/tex] increases. Hence, according to Le-chatelier principle, above equilibrium will shift towards left to minimize concentration of [tex]OH^{-}[/tex] and keep same equilibrium constant.
Therefore excess amount of [tex]OH^{-}[/tex] combines with [tex]NH_{4}^{+}[/tex] to produce ammonia and water. So, effect of addition of strong base on pH of buffer gets minimized.
The buffer solution controls the pH of a solution by shifting the equilibrium towards the left to minimize the concentration.
A buffer solution is made up of the mixing of a weak acid and a weak base.
The equilibrium reaction is
[tex]\rm CH_3(aq) + H_2O = NH_4^+ + OH^_[/tex]
There is OH is present in the equation, which is a weak base.
To reduce concentration and maintain the same equilibrium constant, equilibrium will shift to the left.
So, the addition of an excess amount of buffer will happen to control the buffer of the solution.
Thus, The buffer solution controls the pH of a solution by shifting the equilibrium towards the left to minimize the concentration.
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