Calculate the pH of `0.5L` of a`0.2 M NH_(4)Cl-0.2 M NH_(3)` buffer before and after addition of (a)` 0.05` mole of `NaOH` and (b) `0.05` mole of `HCl`. Assume that the volume remains constant.[Given:`pK_(a)`of `NH_(3)=4.74]`

Explanation

To solve the problem, we will use the Henderson-Hasselbalch equation, which is given by:

\[ \text{pH} = \text{pK}_a + \log\left(\frac{[\text{Base}]}{[\text{Acid}]}\right) \]

Where:
- \([\text{Base}]\) is the concentration of the base (NH₃)
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