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.

Question

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.

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