Final answer:
The pH of the solution is 2.05.
Step-by-step explanation:
We begin by determining [OH¯]. The concentration of the solute is 0.0044 M, but because Ca(OH)₂ is a strong base, there are two OH ions in solution for every formula unit dissolved, so the actual [OH-] is two times this:
[OH-] = 2 × 0.0044 M = 0.0088 M
Now we can use the Kw expression:
Kw = [H3O+][OH-]
Since water is neutral, the concentration of [H3O+] is equal to the concentration of [OH-]. Therefore, we have:
[OH-] = [H3O+] = 0.0088 M
The pH of a solution is calculated using the equation pH = -log[H3O+]. Plugging in the given concentration:
pH = -log(0.0088) = 2.05