At 25°C, the solublity product of Mg(OH)2 is 1.0x10-11. At which pH, will Mg2+ ions start precipitating in the form of Mg(OH)2 from a solution of 0.001M Mg2+ ions

Ksp=Mg+2OH−21×10−11=10−3×OH−2OH−2=10−8OH−=10−4pOH=4 [pH+pOH=14]pH=10.

At 25°C, the solublity product of Mg(OH)2 is 1.0x10-11. At which pH, will Mg2+ ions start precipitating in the form of Mg(OH)2 from a solution of 0.001M Mg2+ ions

Ksp=Mg+2OH−21×10−11=10−3×OH−2OH−2=10−8OH−=10−4pOH=4 [pH+pOH=14]pH=10.

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At 25°C, the solublity product of Mg(OH)₂ is 1.0x10^-11. At which pH, will Mg²⁺ ions start precipitating in the form of Mg(OH)₂ from a solution of 0.001M Mg²⁺ ions

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$\begin{array}{l} K_{sp} = [{Mg}^{+ 2}] {[{OH}^{-}]}^{2} \\ 1 \times 10^{- 11} = 10^{- 3} \times {[{OH}^{-}]}^{2} \\ {[{OH}^{-}]}^{2} = 10^{- 8} \\ {OH}^{-} = 10^{- 4} \\ pOH = 4 [pH + pOH = 14] \\ pH = 10 . \end{array}$

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At 25°C, the solublity product of Mg(OH)2 is 1.0x10-11. At which pH, will Mg2+ ions start precipitating in the form of Mg(OH)2 from a solution of 0.001M Mg2+ ions

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At 25°C, the solublity product of Mg(OH)₂ is 1.0x10^-11. At which pH, will Mg²⁺ ions start precipitating in the form of Mg(OH)₂ from a solution of 0.001M Mg²⁺ ions