How much water do I need to dissolve #95.2*g# magnesium hydroxide?

1 Answer
anor277
Sep 10, 2017

Good luck with this endeavour ...... it is chemically UNREASONABLE.

Explanation:

Magnesium hydroxide is fairly insoluble in water, #K_"sp"=5.61xx10^-12#..which corresponds to a solubility of approx. #10*mg*L^-1#.

On the other hand we could make a solution of magnesium chloride with a concentration of #1.25*mol*L^-1#.

And so we take a mass of #1.25*molxx95.2*g# #MgCl_2#..and place this mass in a #1*L# volumetric flask, and make it up to volume....

#"Concentration"xx"Volume"-="Moles"#

And #"mass"="number of moles"xx"molar mass"#

#-=(1.25*molxx95.2*g*mol^-1)/(1.0*L)# #=# #119*g#.....WITH RESPECT to MAGNESIUM CHLORIDE, i.e. I have altered the boundary conditions of your problem.

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