Question

You have a solution that is 0.02M formate (HCOO-) and 0.03M formic acid (HCOOH), which has a Ka of 1.8x10-4. What is the pH of the solution

Answer 1

3.6

Step-by-step explanation:

Step 1: Given data

• Concentration of formic acid: 0.03 M

• Concentration of formate ion: 0.02 M

• Acid dissociation constant (Ka): 1.8 × 10⁻⁴

Step 2: Calculate the pH

We have a buffer system formed by a weak acid (HCOOH) and its conjugate base (HCOO⁻). We can calculate the pH using the Henderson-Hasselbach equation.

`pH = pKa +log([base])/([acid]) = -log 1.8 * 10^(-4) + log (0.02)/(0.03) = 3.6`