Question

If a buffer solution is 0.570m in a weak acid (kt = 3.4 x 10⁻⁶) and 0.120 m in its conjugate base, what is the ph?

Answer 1

To find the pH of a buffer solution, use the Henderson-Hasselbalch equation with the provided concentrations of the weak acid and its conjugate base, and the acid dissociation constant.

Step-by-step explanation:

To calculate the pH of a buffer solution that is 0.570 M in a weak acid with a dissociation constant (Ka = 3.4 × 10⁻⁶) and 0.120 M in its conjugate base, we can use the Henderson-Hasselbalch equation:

pH = pKa + log([A⁻]/[HA])

First, we need to calculate the pKa from the given Ka:

pKa = -log(Ka) = -log(3.4 × 10⁻⁶)

Then, we use the Henderson-Hasselbalch equation by plugging in the values for the concentrations of the conjugate base ([A⁻]) and the weak acid ([HA]):

pH = pKa + log(0.120/0.570)

After performing the calculations, we find the pH of the buffer solution.