The Ksp of Mg(OH) 2 is 8.9 ×10 -12 at 25 * C. If the pH of solution is adjusted to 9.0 . How much Mg +2 ion will be precipitated as Mg(OH) 2 from a 0.1 M MgCl 2 solution at 25 * C ? Assume that MgCl 2 is completely dissociated. a. 0.011 b. 0.089 c. 0.11 d. 0.89 Please explain in detail.............

Question

The Ksp of Mg(OH) 2 is 8.9 ×10 -12 at 25 * C. If the pH of solution is adjusted to 9.0 . How much Mg +2 ion will be precipitated as Mg(OH) 2 from a 0.1 M MgCl 2 solution at 25 * C ? Assume that MgCl 2 is completely dissociated. ​ a. 0.011 ​b. 0.089 c. 0.11 d. 0.89 Please explain in detail.............

Vikas TU · Answer

Ksp[Mg(OH)2]=8.9×10^−2 pH=9 [H+]=10^−9 [OH−]=10^−5 Ksp=[Mg2+][OH−]^2 8.9×10^−12=[Mg2+][10^−5]^2 [Mg2+]=8.9×10^−2=0.089 Conc. Of Mg2+ precipitated =0.1−0.089 = 0.011mol/L.t

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The Ksp of Mg(OH) 2 is 8.9 ×10 -12 at 25 * C. If the pH of solution is adjusted to 9.0 . How much Mg +2 ion will be precipitated as Mg(OH) 2 from a 0.1 M MgCl 2 solution at 25 * C ? Assume that MgCl 2 is completely dissociated. a. 0.011 b. 0.089 c. 0.11 d. 0.89 Please explain in detail.............

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The Ksp of Mg(OH)2 is 8.9 ×10-12 at 25*C. If the pH of solution is adjusted to 9.0 . How much Mg+2 ion will be precipitated as Mg(OH)2 from a 0.1 M MgCl2 solution at 25*C ? Assume that MgCl2 is completely dissociated.​ a. 0.011​b. 0.089c. 0.11d. 0.89Please explain in detail.............