21) A buffer solution with a pH of 4.78 is prepared with M formic acid and 0.90 M sodium formate. The Ka of formic acid is 1.8 x 10-4.

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**Buffer Solution Preparation**

**Problem Statement:**

A buffer solution with a pH of 4.78 is prepared with ______ M formic acid and 0.90 M sodium formate. The \( K_a \) of formic acid is \( 1.8 \times 10^{-4} \).

**Task:**

Determine the concentration (Molarity) of formic acid required to achieve the desired pH when mixed with 0.90 M sodium formate. 

**Notes:**

- Buffer solutions consist of a weak acid and its conjugate base.
- The \( K_a \) value is essential for calculating the necessary concentrations for buffer solutions.
  
**Equation:**

- Use the Henderson-Hasselbalch equation:
  \[
  \text{pH} = \text{pKa} + \log{\left(\frac{\text{[A}^-]}{\text{[HA]}}\right)}
  \]
   where:
   - [A\(^-\)] is the concentration of the conjugate base (sodium formate).
   - [HA] is the concentration of the weak acid (formic acid).
Transcribed Image Text:**Buffer Solution Preparation** **Problem Statement:** A buffer solution with a pH of 4.78 is prepared with ______ M formic acid and 0.90 M sodium formate. The \( K_a \) of formic acid is \( 1.8 \times 10^{-4} \). **Task:** Determine the concentration (Molarity) of formic acid required to achieve the desired pH when mixed with 0.90 M sodium formate. **Notes:** - Buffer solutions consist of a weak acid and its conjugate base. - The \( K_a \) value is essential for calculating the necessary concentrations for buffer solutions. **Equation:** - Use the Henderson-Hasselbalch equation: \[ \text{pH} = \text{pKa} + \log{\left(\frac{\text{[A}^-]}{\text{[HA]}}\right)} \] where: - [A\(^-\)] is the concentration of the conjugate base (sodium formate). - [HA] is the concentration of the weak acid (formic acid).
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