can you do the same calculation with a buffer that contains 10 ml of 0.05M formic acid and 10 ml of 0.05M sodium formate?

To calculate the pH of a buffer solution containing 10 mL of 0.05 M formic acid (HCOOH) and 10 mL of 0.05 M sodium formate (HCOONa), we can use the Henderson-Hasselbalch equation:

\[
\text{pH} = \text{pK}_a + \log \left( \frac{[\text{A}^-]}{[\text{HA}]} \right)
\]

### Step 1: Calculate the concentrations of the components in the mixed solution.

Since both solutions are mixed in equal volumes (10 mL), the total volume becomes 20 mL. The concentrations of the components after mixing can be calculated as follows:

- For formic acid (HA):
\[
[\text{HA}] = \frac{(0.05 \, \text{M}) \times (10 \, \text{mL})}{20 \, \text{mL}} = 0.025 \, \text{M}
\]

- For sodium formate (A^-):
\[
[\text{A}^-] = \frac{(0.05 \, \text{M}) \times (10 \, \text{mL})}{20 \, \text{mL}} = 0.025 \, \text{M}
\]

### Step 2: Determine the \( \text{pK}_a \) of formic acid.

The dissociation constant \( K_a \) for formic acid is approximately \( 1.8 \times 10^{-4} \). The \( \text{pK}_a \) is calculated as follows:

\[
\text{pK}_a = -\log(1.8 \times 10^{-4}) \approx 3.74
\]

### Step 3: Apply the Henderson-Hasselbalch equation.

Now substituting the values into the equation:

\[
\text{pH} = 3.74 + \log \left( \frac{0.025}{0.025} \right) = 3.74 + \log(1) = 3.74
\]

### Conclusion

The pH of the buffer solution containing 10 mL of 0.05 M formic acid and 10 mL of 0.05 M sodium formate is **3.74**.

Would you like any further details or have any questions? Here are some related questions you might find interesting:

1. How does the pH change if the concentration of formic acid is increased?
2. What would happen to the pH if more sodium formate is added?
3. Can you explain how buffers resist changes in pH?
4. How does temperature affect the pH of buffer solutions?
5. What are some practical applications of formic acid buffers in laboratories? 

**Tip:** Always ensure that the concentrations and volumes are carefully measured for accurate buffer preparation.

Can you do the same calculation with a buffer that contains 10 ml of 0.05M formic acid and 10 ml of 0.05M sodium formate?

Explore how to calculate the pH of a buffer solution containing 10 mL of 0.05 M formic acid and 10 mL of 0.05 M sodium formate. Learn about the Henderson-Hasselbalch equation and the properties of buffer solutions. Ideal for high school students studying chemistry.

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