A sample of groundwater that has percolated through a layer of gypsum CaSO4 with Ksp-4-9- 10-5 is found to have 8-4- 10-5 M in Ca2- and 7-2- 10-5 M in SO42- The equilibrium state of this solution with respect to gypsumCaSO4 is -

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Reaction Quotient

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Question

A sample of groundwater that has percolated through a layer of gypsum $(C a S O_{4})$ with $K_{s p} = 4.9 \times 10^{- 5}$ is found to have $8.4 \times 10^{- 5} M$ in $C a^{2 +}$ and $7.2 \times 10^{- 5} M$ in $S O_{4}^{2 -}$ .
The equilibrium state of this solution with respect to gypsum $(C a S O_{4})$ is :

Unsaturated solution

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Saturated solution

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Supersaturated solution

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Cannot be determined

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Solution

The correct option is A Unsaturated solution
The equilibrium established will be:
$C a S O_{4} (s) ⇌ C a^{2 +} (a q .) + S O_{4}^{2 -} (a q .)$

Finding the ion product $Q_{s p}$
$Q_{s p} = (8.4 \times 10^{- 5}) \times (7.2 \times 10^{- 5}) Q_{s p} = 6.04 \times 10^{- 9} < K_{s p} = 4.9 \times 10^{- 5}$

Since, $\frac{Q s p}{K_{s p}} < 1$
$\Rightarrow$ The solution is unsaturated in $C a S O_{4} .$

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Reaction Quotient

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A sample of groundwater that has percolated through a layer of gypsum (CaSO4) with Ksp=4.9×10−5 is found to have 8.4×10−5 M in Ca2+ and 7.2×10−5 M in SO2−4. The equilibrium state of this solution with respect to gypsum(CaSO4) is :

The correct option is A Unsaturated solutionThe equilibrium established will be: CaSO4 (s)⇌Ca2+ (aq.)+SO2−4 (aq.) Finding the ion product Qsp Qsp=(8.4×10−5)×(7.2×10−5)Qsp=6.04×10−9<Ksp=4.9×10−5 Since, QspKsp<1 ⇒The solution is unsaturated in CaSO4.