Part A Calculate the solubility (n grams per 1.00 -12. 10P mL of solution) of ma

Question

Part A Calculate the solubility (n grams per 1.00 -12. 10P mL of solution) of magnesium hydraxide in a solution buffered at pH x Express your answer using two signifioant figures g/(1.00 x 10P mL Part B Calculate the solubility (in grams per 1.00 × 10, mL of solution) of magnesium hydro de n pure water Express your answer using two significant figures. g/1.00 x 10mL Part C How does the solubility of Mg(OH) in a buffered solution compare to the solubilty of Mg(OH)2 in pure water? Express your answer using two significant figures Si

Explanation / Answer

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

pH=12. so, pOH =14-12=2

sp, [OH-]= 10-pOH

=0.01

so, Mg+2 is half of OH-. so, [Mg+2]= 0.01/2=0.005

Ksp =[Mg+2]*[OH-]

=0.005*0.01

S1= 5* 10-5 is the solubility of magnesium hydroxide in given solution

pH of pure water is 6.14

so, pOH- 14-6.14=7.86

[OH-]= -antilog 7.86= 1.38 *10-8

[Mg+2]=6.9*10-9

Ksp= [Mg+2]*[OH-]

S = 9.52*10-16 solubility in pure water

your compound is less soluble in pure water

S1/S= 5*10-5/9.52*10-16= 5.25*1010

note: higher the Ksp more the solubility and vice-versa!

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