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Determine the pH of an acidic buffer sol...

Determine the `pH` of an acidic buffer solution `(HA+NaA)` having acid and salt concentration respectively `0.1M` and `0.2M`. (Given `pK_(a) = 4.7, log 2= 0.30, log 5=0.70)`

A

`4`

B

`5`

C

`3`

D

None of these

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The correct Answer is:
To determine the pH of the acidic buffer solution (HA + NaA) with given concentrations of acid and salt, we can use the Henderson-Hasselbalch equation: ### Step-by-Step Solution: 1. **Identify the concentrations**: - Concentration of the acid (HA) = 0.1 M - Concentration of the salt (NaA) = 0.2 M 2. **Use the Henderson-Hasselbalch equation**: The equation is given by: \[ \text{pH} = \text{pK}_a + \log\left(\frac{[\text{Salt}]}{[\text{Acid}]}\right) \] 3. **Substitute the known values**: - Given \( \text{pK}_a = 4.7 \) - Substitute the concentrations into the equation: \[ \text{pH} = 4.7 + \log\left(\frac{0.2}{0.1}\right) \] 4. **Calculate the ratio**: - The ratio \( \frac{0.2}{0.1} = 2 \) 5. **Calculate the logarithm**: - Using the given value \( \log 2 = 0.30 \): \[ \log(2) = 0.30 \] 6. **Substitute back into the equation**: \[ \text{pH} = 4.7 + 0.30 \] 7. **Final calculation**: \[ \text{pH} = 5.0 \] ### Conclusion: The pH of the acidic buffer solution is **5.0**.
To determine the pH of the acidic buffer solution (HA + NaA) with given concentrations of acid and salt, we can use the Henderson-Hasselbalch equation: ### Step-by-Step Solution: 1. **Identify the concentrations**: - Concentration of the acid (HA) = 0.1 M - Concentration of the salt (NaA) = 0.2 M ...
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