The pOH of an aqueous solution at 25°C was found to be 2.30. The pH is 11.7.
What is the concentration of the hydronium ion and the hydroxide ion?
To find the concentration of hydronium ion (H3O+) and hydroxide ion (OH-) in an aqueous solution, we can use the equation:
pH + pOH = 14
Given that the pOH is 2.30, we can calculate the pH as follows:
pH = 14 - pOH
pH = 14 - 2.30
pH = 11.7
So we have confirmed that the pH is indeed 11.7.
Now, to find the concentration of H3O+ (hydronium ion) and OH- (hydroxide ion), we need to use the equations:
pH = -log[H3O+]
pOH = -log[OH-]
Rearranging these equations, we get:
[H3O+] = 10^(-pH)
[OH-] = 10^(-pOH)
Substituting the given values, we have:
[H3O+] = 10^(-11.7)
[OH-] = 10^(-2.30)
Using a calculator, we can find the respective concentrations:
[H3O+] ≈ 1.995 x 10^(-12) M
[OH-] ≈ 5.01 x 10^(-3) M
Therefore, the concentration of H3O+ is approximately 1.995 x 10^(-12) M, and the concentration of OH- is approximately 5.01 x 10^(-3) M in the aqueous solution at 25°C.