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# What will be the solubility of the $Ca{(OH)_2}$solution when $NaOH$ is dissolved in it, compared with that in pure water?A. UnaffectedB. IncreasedC. DecreasedD. None

Last updated date: 04th Aug 2024
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Hint: If you've got a solution and solute in equilibrium, including a common ion (an ion that is common with the dissolving solid) decreases the solubility of the solute. This is due to the fact Le Chatelier's precept states the response will shift closer to the left (in the direction of the reactants) to relieve the pressure of the extra product

Complete Step by step solution:
The solubility of $Ca{(OH)_2}$solution is reduced wherein $NaOH$ is dissolved, as compared with that in pure water due to the common ion effect. The hydroxide ion is a common ion.
The dissolution of $NaOH$ to a solution of $Ca{(OH)_2}$will lower the solubility of $Ca{(OH)_2}$. $Ca{(OH)_2}$ is sparingly soluble salt.
The dissociation of $Ca{(OH)_2}$in solution is represented by following solubility equilibrium.
$Ca{(OH)_2}(s) \to C{a^{ + 2}}(aq) + 2O{H^ - }(aq)$
$NaOH$ is a strong electrolyte and completely dissociates in aqueous solution.
$NaOH(s) \to N{a^ + }(aq) + O{H^ - }(aq)$
The dissociation of hydroxide ions which are common to $Ca{(OH)_2}$ . This suppresses the dissociation of $Ca{(OH)_2}$ .

So the correct answer is C.