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The Ksp of chromium (III) iodate, Cr(IO3)3, is 5.00 × 10-6. Calculate the molar solubility of...

The Ksp of chromium (III) iodate, Cr(IO3)3, is 5.00 × 10-6. Calculate the molar solubility of this compound.

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Answer #1

The equilibrium reaction during dissociation of Cr(IO3)3 can be written as follows :

The expression for solubility product of Cr(IO3)3 can be written as follows:

Let “x” be the amount of Cr(IO3)3 dissociated at equilibrium thus amount of chromium (III) ions is “x” and “3x” is the amount of iodate ions in the equilibrium constant expression:

x represents the moles of solute soluble in one liter of solution. Thus, it is the molar solubility of Cr(IO3)3

Therefore, molar solubility of chromium (III) iodate is 2.07 x 10-2 M

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