Anonymous
Anonymous asked in Science & MathematicsChemistry · 2 months ago

Chemistry - molar solubility?

Here is the question: Calculate and compare the molar solubility of Mg(OH)2 in water and in a solution buffered at a pH of 5.5. Determine the molar solubility of Mg(OH)2 in water and the pH of a saturated Mg(OH)2 solution. 

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  • david
    Lv 7
    2 months ago
    Favorite Answer

    You need Ksp  for Mg(OH)2 ...  wait a sec, while i go to google == If you had looked it up in your book and posted it, then it would not take as long.

       Mg(OH)2  <-->  Mg(2+)  +  2OH(-)

      Ksp  =  1.5x10^-11  =  [Mg(2+)][OH(-)]^2  =  x(2x)^2 = 4x^3

       x = 1.5536x10^-4 M  <<<  solubility of the pure substance

     = = = = = = = == = = = = = = = == = = 

       pH of a sat. solution

       [OH(-)]  =  2x  =  3.1072x10^-4 M

        pOH  =  3.5  ...  pH  =  10.5

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