The solubility of Ca(OH)_2 in water is ...... | vedclass

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(C) The dissociation of $Ca(OH)_2$ is represented as:$Ca(OH)_2(s) \rightleftharpoons Ca^{2+}(aq) + 2OH^-(aq)$If $s$ is the solubility,then $[Ca^{2+}]

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$1.11 	imes 10^{-2}$

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(C) The dissociation of $Ca(OH)_2$ is represented as:$Ca(OH)_2(s) ightleftharpoons Ca^{2+}(aq) + 2OH^-(aq)$If $s$ is the solubility,then $[Ca^{2+}] = s$ and $[OH^-] = 2s$.The solubility product expression is:$K_{sp} = [Ca^{2+}][OH^-]^2 = (s)(2s)^2 = 4s^3$Given $K_{sp} = 5.5 	imes 10^{-6}$,we have:$4s^3 = 5.5 	imes 10^{-6}$$s^3 = \frac{5.5}{4} 	imes 10^{-6} = 1.375 	imes 10^{-6}$$s = (1.375 	imes 10^{-6})^{1/3} \approx 1.11 	imes 10^{-2} 	ext{ M}$

The solubility of $Ca(OH)_2$ in water is ....... .
[Given : The solubility product of $Ca(OH)_2$ in water $= 5.5 \times 10^{-6}$]

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The solubility of $Ca(OH)_2$ in water is ....... .[Given : The solubility product of $Ca(OH)_2$ in water $= 5.5 \times 10^{-6}$]