Final answer:
The pH of a 0.100 M solution of acetic acid is 2.87.
Step-by-step explanation:
The pH of a solution can be calculated using the concentration of the weak acid and the equilibrium constant Ka. In this case, the initial concentration of acetic acid is given as 0.100 M. By setting up an ICE table and solving for the concentration of H+, we can calculate the pH of the solution.
[H+] = Ka × [CH3CO₂H] = sqrt(1.8 × 10^-5 × 0.100) = 1.3 × 10^-3
pH = -log(1.3 × 10^-3) = 2.87