12. What equation or expression would be used to calculate the pH of a 0.12 M solution of formic acid. The Ka of formic acid (CH2O2) is 1.8 × 10-4. A) Ka expression в) кЪ ехpression c) Kw = Ka*Kb D) Henderson Hasselbach Equation Calculate the pH of the solution above.
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![**Question 12: Calculating the pH of Formic Acid Solution**
To determine the appropriate equation or expression for calculating the pH of a 0.12 M solution of formic acid:
**Given:**
- The \( K_a \) of formic acid (\( \text{CH}_2\text{O}_2 \)) is \( 1.8 \times 10^{-4} \).
**Options:**
A) **Ka Expression**
B) **Kb Expression**
C) **Kw = Ka \* Kb**
D) **Henderson Hasselbach Equation**
**Task:** Calculate the pH of the solution above.
**Explanation:**
For a weak acid such as formic acid, the pH can typically be calculated using the **Ka expression**. This involves setting up an equilibrium expression for the dissociation of the acid and solving for the concentration of hydrogen ions. From this, the pH can be determined.
In this context, the correct approach (Choice A) would be to use the \( K_a \) expression:
\[ K_a = \frac{[H^+][A^-]}{[HA]} \]
Given the formic acid concentration and \( K_a \), the equation can be solved to find the pH of the solution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F319348e8-ec3b-434b-beac-e2801422c409%2F763dc404-cff8-42f8-82e2-a27546d4ecd7%2Fmcwo8im_processed.png&w=3840&q=75)
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