Previous Year NEET Question- Ionic Equilibrium
- 2019: What is the pH of a 0.01 M solution of acetic acid? (Given that Ka = 1.8 x 10-5)
The pH of a solution is a measure of the acidity or basicity of that solution. The pH scale ranges from 0 to 14, with 0 being the most acidic and 14 being the most basic. A neutral solution has a pH of 7.
The pH of a solution of acetic acid can be calculated using the following equation:
pH = -log[H+]
where [H+] is the concentration of hydrogen ions in the solution.
In this case, the concentration of acetic acid is 0.01 M, so the concentration of hydrogen ions is approximately 0.001 M.
[H+] = 10^-pH
[H+] = 10^-4 M
Therefore, the pH of the solution is:
pH = -log[H+]
pH = -log(10^-4)
pH = 4
BETA
