3. Assume that you prepare a buffer by mixing 42 ml of 0.26 M acetic acid and 56 ml of 0.15 M sodium acetate (the pKa of acetic acid is 4.8). a) What is the pH of the buffer? b) What will be the pH if you add 2 ml of 0.2 M HCI to the buffer?

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**Problem 3: Buffer Preparation and pH Calculation**

**Context:**
Assume that you prepare a buffer by mixing 42 ml of 0.26 M acetic acid and 56 ml of 0.15 M sodium acetate (the pKa of acetic acid is 4.8).

a) What is the pH of the buffer?
b) What will be the pH if you add 2 ml of 0.2 M HCl to the buffer?

**Solution Approach:**

To solve part (a), use the Henderson-Hasselbalch equation:
\[ \text{pH} = \text{pKa} + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \]
where:
- \([\text{A}^-]\) = Concentration of the conjugate base, sodium acetate
- \([\text{HA}]\) = Concentration of the weak acid, acetic acid
- \(\text{pKa}\) = 4.8

To solve part (b), first calculate the change in the concentrations of acetic acid and acetate due to the addition of HCl using stoichiometry. Then, apply the Henderson-Hasselbalch equation again to find the new pH.
Transcribed Image Text:**Problem 3: Buffer Preparation and pH Calculation** **Context:** Assume that you prepare a buffer by mixing 42 ml of 0.26 M acetic acid and 56 ml of 0.15 M sodium acetate (the pKa of acetic acid is 4.8). a) What is the pH of the buffer? b) What will be the pH if you add 2 ml of 0.2 M HCl to the buffer? **Solution Approach:** To solve part (a), use the Henderson-Hasselbalch equation: \[ \text{pH} = \text{pKa} + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right) \] where: - \([\text{A}^-]\) = Concentration of the conjugate base, sodium acetate - \([\text{HA}]\) = Concentration of the weak acid, acetic acid - \(\text{pKa}\) = 4.8 To solve part (b), first calculate the change in the concentrations of acetic acid and acetate due to the addition of HCl using stoichiometry. Then, apply the Henderson-Hasselbalch equation again to find the new pH.
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