One of the main components of hard water is CaCO3. When hard water evaporates, some of the CaCO3 is left behind as a white mineral deposit. If a hard water solution is saturated with CaCO3, what volume of the solution has to evaporate ot deposit 1*10^{2} mg of CaCO3?

Question

04-11-2016
Chemistry

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One of the main components of hard water is CaCO3. When hard water evaporates, some of the CaCO3 is left behind as a white mineral deposit. If a hard water solution is saturated with CaCO3, what volume of the solution has to evaporate ot deposit 1*10^{2} mg of CaCO3?

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Anonymous Anonymous · Answer 1 · 2016-11-07T09:06:53-05:00

My source says the Ksp of CaCO3 at 25 C is 8.7 X 10^-9

Ksp = [Ca++][CO3--] = 8.7 X 10^-9

Let "X" = the solubility; then:

X^2 = 8.7 X 10^-9

X = 9.33 X 10^-5 M

Mol. mass CaCO3 = 40 + 12 + 3(16) = 100 g / mole

Solubility CaCO3 = (100 g / mole)(9.33 X10^-5 mole / liter) = 9.33 X 10^-3 g liter or 9.33 mg / liter

Volume of CaCO3 solution = 1.00 X 10^2 mg / 9.33 mg / liter = 10.7 liters

Answer: 10.7 liters

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