At 25°C, the solubility product of Mg(OH)₂ is 1.0 × 10^–11. At which pH, will Mg²⁺ ions start precipitating in the form of Mg(OH)₂ from a solution of 0.001 M Mg²⁺ ions?

9

10

11

8

Solution

straight K subscript sp space equals space left square bracket Mg to the power of 2 plus end exponent right square bracket left square bracket OH to the power of negative 1 end exponent right square bracket squared left square bracket OH to the power of minus right square bracket squared space equals space straight K subscript sp left square bracket Mg to the power of 2 plus end exponent right square bracket space equals space 10 to the power of negative 11 end exponent over blank left square bracket OH to the power of minus right square bracket space equals space 10 to the power of negative 4 end exponent left square bracket straight H to the power of plus right square bracket space equals space 10 to the power of negative 14 end exponent over 10 to the power of negative 4 end exponent space equals space 10 to the power of negative 10 end exponent pH space equals space 10 space

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