pH of a saturated solution of Ca(OH)2Ca(OH)_2Ca(OH)2 is 9. The solubility product (KspK_{sp}Ksp) of Ca(OH)2Ca(OH)_2Ca(OH)2 is:
0.5×10−150.5 \times 10^{-15}0.5×10−15
0.25×10−100.25 \times 10^{-10}0.25×10−10
0.125×10−150.125 \times 10^{-15}0.125×10−15
0.5×10−100.5 \times 10^{-10}0.5×10−10
Ca(OH)2⇌Ca2++2OH−Ca(OH)_2 \rightleftharpoons Ca^{2+} + 2OH^-Ca(OH)2⇌Ca2++2OH−. pH = 9, Hence pOH = 14 - 9 = 5, [OH−]=10−5M[OH^-] = 10^{-5} M[OH−]=10−5M. Hence [Ca2+]=10−52[Ca^{2+}] = \frac{10^{-5}}{2}[Ca2+]=210−5. Thus Ksp=[Ca2+][OH−]2=(10−52)(10−5)2=0.5×10−15K_{sp} = [Ca^{2+}][OH^-]^2 = (\frac{10^{-5}}{2})(10^{-5})^2 = 0.5 \times 10^{-15}Ksp=[Ca2+][OH−]2=(210−5)(10−5)2=0.5×10−15.
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