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The solubility product of calcium fluoride (CaF2) is 3.45 X 10^-11at 25 degrees C. Will a fluoride concentration of 1.0 mg/L besoluble in a water containing 200mg/L of calcium?

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Deanna Hettinger
Deanna HettingerLv2
28 Sep 2019
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Related questions

Given that the average concentration of calcium ion in natural waters is 3.8 x 10-4 M, and that the solubility product Ksp for CaF2 is 4 x 10-11, calculate the maximum molar concentration of fluoride ion that can be dissolved before precipitation begins. Show that this molarity is equivalent to about 6 ppm. (Hint: Write the solubility product expression for CaF2 and substitute the molar value for [Ca2+] into it.)

1) Pb3(AsO4)2 is slightly soluble in water, if the solubility is 3,0*10^-5 g/L, what is the solubility product constant? Assume that the solubility equilibrium is the only important one.

2) Anhydrite is a calcium sulfate mineral deposited when seawater evaporates. what is the solubility of calcium sulfate in grams per liter? The solubility product constant for calcium sulfate is 2.4*10^-5.

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Nine\

Compound Formula Ksp
Iron(II) sulfide FeS 3.72x10-19
Magnesium hydroxide Mg(OH)2 2.06x10-13
Calcium fluoride CaF2 1.46x10-10

Part A Use the ksp values in the table to calculate the molar solubility of FeS in pure water?

Part B Use the Ksp values in the table to calcualte the molar solubility of Mg(OH)2 in pure water.?

Part C Use the Ksp values in the table to calculate the molar solubilty of CaF2 in pure water.?

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