Calculate the pH of a saturated solution of Sr(OH)2. The Ksp for Sr(OH)2 is 3.2x10^-4.
...........Sr(OH)2 --> Sr^2+ + 2OH^-
I..........solid........0........0
C..........solid........x........2x
E..........solid........x........2x
Substitute the E line into the Ksp expression and solve for x = (OH^-), then convert that to pOH then to pH.
Thank you!
To calculate the pH of a saturated solution of Sr(OH)2, we need to first determine the concentration of hydroxide ions (OH-) in the solution.
Since Sr(OH)2 is a strong base, it completely dissociates in water, yielding two hydroxide ions for every molecule of Sr(OH)2.
The Ksp for Sr(OH)2 gives us the solubility product constant, which is a measure of the ability of the compound to dissolve in water. In this case, the Ksp = 3.2x10^-4.
The expression for the solubility product constant is Ksp = [Sr^2+][OH-]^2, where [Sr^2+] and [OH-] represent the concentrations of strontium ions and hydroxide ions, respectively.
Since Sr(OH)2 is a strong base, the concentration of hydroxide ions will be twice the concentration of strontium ions.
Let's assume the concentration of strontium ions is x M. Therefore, the concentration of hydroxide ions will be 2x M.
Substituting these values into the expression for Ksp, we get:
Ksp = [x][2x]^2
3.2x10^-4 = 4x^3
Now we can solve for x by taking the cube root of both sides:
x = (3.2x10^-4)^(1/3)
x ≈ 0.065 M
Since the concentration of hydroxide ions is twice the concentration of strontium ions, [OH-] ≈ 2x ≈ 0.13 M.
To calculate the pH, we will use the equation:
pOH = -log[OH-]
pOH = -log(0.13)
pOH ≈ 0.89
Since pH + pOH = 14, we can find the pH by subtracting pOH from 14:
pH = 14 - pOH
pH ≈ 14 - 0.89
pH ≈ 13.11
Therefore, the pH of a saturated solution of Sr(OH)2 is approximately 13.11.
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