Final answer:
To find the pH of a 0.100 M solution of a weak acid with Ka = 1.2x10^-3, an ICE table can be used to calculate the concentration of the conjugate base and the hydrogen ion. Solving for x gives x = 3.27x10^-3 M. The negative logarithm of the hydrogen ion concentration gives a pH of 2.49.
Step-by-step explanation:
The pH of a 0.100 M solution of a weak monoprotic acid can be determined using the dissociation constant, Ka. In this case, the Ka is given as 1.2x10^-3. To calculate the pH, we can set up an ICE table. Let's call the initial concentration of the acid x. Then, the table would look like this:
Acid Conjugate Base0.100 M - xx
After applying the dissociation constant and solving for x, we obtain x = 3.27x10^-3 M. The pH can be calculated as -log[H+], which gives a pH of 2.49.