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.

Related questions
See all questions in Molarity
Impact of this question
1826 views around the world
You can reuse this answer
Creative Commons License