For calcium sulfate, the K SP value has to be calculated. Concept Introduction: Solubility product constant: The equilibrium constant of a more soluble ionic compound in water at the higher solubility is known as solubility product constant. The equilibrium constant of more soluble ionic compound is given by K SP and it is expressed by product of each ion present in the compound which are raised to the power of number respective ion present in the compound to give a maximum solubility of the compound. M m X x (s) ⇌ mM n+ (aq) + xX y- (aq) K sp = [M n+ ] m [X y- ] x Ion product: The multiplication of concentrations of ions which are raised to the power of number of respective ions present in the molecular formula. This gives the ion product. M m X x (s) ⇌ mM n+ (aq) + xX y- (aq) IP = [M n+ ] t m ×[X y- ] x Precipitation occurs when solution is supersaturated, IP > K sp . Precipitation will not occurs when solution is saturated and in equilibrium, IP > K sp . Precipitation will not occurs when solution is unsaturated, IP < K sp .

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Chapter 19, Problem 19.74P

Interpretation Introduction

Interpretation:

For calcium sulfate, the $KSP$ value has to be calculated.

Concept Introduction:

Solubility product constant:

The equilibrium constant of a more soluble ionic compound in water at the higher solubility is known as solubility product constant.

The equilibrium constant of more soluble ionic compound is given by $KSP$ and it is expressed by product of each ion present in the compound which are raised to the power of number respective ion present in the compound to give a maximum solubility of the compound.

$MmXx(s)⇌ mMn+(aq) + xXy-(aq)Ksp = [Mn+]m[Xy-]x$

Ion product:

The multiplication of concentrations of ions which are raised to the power of number of respective ions present in the molecular formula. This gives the ion product.

$MmXx(s)⇌ mMn+(aq) + xXy-(aq)IP = [Mn+]tm×[Xy-]x$

Precipitation occurs when solution is supersaturated, $IP > Ksp$ .

Precipitation will not occurs when solution is saturated and in equilibrium, $IP > Ksp$ .

Precipitation will not occurs when solution is unsaturated, $IP <Ksp$ .

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