Question

Calculate the ph of a solution that is 0.6 m in sodium acetate and 0.2 m in acetic acid. ka = 1.8 × 10−5 for acetic acid. 1. ph = 4.3 2. ph = 4.7 3. ph = 5.2 4. ph = 2.7 5. ph = 5.6

Answer 1

The pH of the solution is 4.7.

Step-by-step explanation:

The pH of a solution that is 0.6 M in sodium acetate and 0.2 M in acetic acid can be calculated using the Henderson-Hasselbalch equation. The equation is pH = pKa + log([A-]/[HA]), where [A-] is the concentration of the conjugate base (acetate) and [HA] is the concentration of the weak acid (acetic acid).

In this case, the pKa of acetic acid is 1.8 × 10-5. Using the given concentrations, the pH of the solution can be calculated as follows:

pH = -log(1.8 × 10-5) + log(0.6/0.2) = 4.7

Answer 2

0.53 x 200ml = 106 ml of the pH 9.0 buffer + 94 ml of the pH 10 buffer gives the desired solution