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( a ) If the molar solubility of CaF2 at 35 °C is 1.24 × 10-3 mol/L, what is Ksp at this temperature? (b) It is found that 1.1 × 10-2 g SrF2 dissolves per 100 mL of aqueous solution at 25 °C. Calculate the solubility product for SrF2. (c) The Ksp of Ba(IO3)2 at 25 °C is 6.0 × 10-10. What is the molar solubility of Ba(IO3)2?

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Nestor Rutherford
Nestor RutherfordLv2
20 May 2020

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Related questions

If the Ksp of Ba(IO3)2 at 25°C is 6.0 X 10-10, what is the molar solubility of Ba(IO3)2?

In definition, solubility or molar solubility of a compound is the concentration of the dissolved solids in a saturated solution. Molar solubility can be solved using the given solubility product constant. 

For the compound C2D3, we can express this as the concentration of C and D in the aqueous solution. 

To solve for the molar solubility: 

Let S = molar solubility of C2D3 in mol L-1

[C] = 2S

[D] = 3S

 

Substituting this to the solubility product constant, Ksp formula, we'll have:

  

  

  

  

 

Thus, the molar solubility is 3.958 x 10 -5 M. 

(a) If the molar solubility of Ag2C2O4 at 25 oC is 0.000111 mol/L, what is the Ksp at this temperature?

Ksp =




(b) It is found that 6.25e-06 g of Cd3(PO4)2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Cd3(PO4)2.

Ksp =




(c) The Ksp of Cu3(AsO4)2 at 25 oC is 7.95e-36. What is the molar solubility of Cu3(AsO4)2?

solubility = mol/L



(a) If the molar solubility of Cd3(AsO4)2 at 25 oC is 1.15e-07 mol/L, what is the Ksp at this temperature?

Ksp = ??????




(b) It is found that 1.66e-06 g of Ca3(PO4)2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Ca3(PO4)2.

Ksp = ?????




(c) The Ksp of PbF2 at 25 oC is 3.30e-08. What is the molar solubility of PbF2?

solubility =???????? mol/L

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