1000 mL x 1.02 g/mL x 0.0013 = approx 1.4 grams Ca(OH)2 but that's just a close estimate.
Then mols = grams/molar mass Ca(OH)2 and since that is mols/L that is the M and = approx 0.02. Again, that's an estimate.
.......Ca(OH)2 ==> Ca^2+ + 2OH^-
I......0.02.........0.......0
C.....=0.02........0.02...0.04
E........0.........0.01...0.04
So pOH = -log(OH^-) and convert to pH with
pH + pOH = pKw = 14.
You know pKw and pOH, solve for pH.
A saturated aqueous solution of calcium hydroxide, Ca(OH)2, is approximately 0.13% calcium hydroxide, by mass, and has a density of 1.02 g/mL. What is the pH of such a solution?
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1 answer