Calculate pH of the following mictures , Given that `K_(a) = 1.8 xx 10^(-5) and K_(b) = 1.8 xx 10^(-5)`
(a) 50 mL of `0.05` NaOH + 50 ml of `0.10 ` M `CH_(3)COOH`
(b) 50 ml of `0.10` NaOH + 50 ml of `0.10` M `CH_(3) COOH`

Explanation

To calculate the pH of the given mixtures, we will use the Henderson-Hasselbalch equation for the first mixture, and for the second mixture, we will use the formula for weak acids and strong bases.

### (a) 50 mL of 0.05 M NaOH + 50 mL of 0.10 M CH₃COOH

1. **Calculate the moles of NaOH and CH₃COOH:**
- Moles of NaOH = Molarity × Volume = 0.05 M × 0.050 L = 0.0025 moles (or 2.5 mmol)
- Moles of CH₃COOH = Molarity × Volume = 0.10 M × 0.050 L = 0.005 moles (or 5 mmol)

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