mols Mn(OH)2 = grams/molar mass =?
Then M Mn(OH)2 = mols/0.1L = ? . Let's call this y because I don't have a calculator with me.
........Mn(OH)2 ==> Mn^2+ + 2OH^-
I.......solid.......0........0
C......solid........y........2y
E.......solid.......y........2y
Ksp = (Mn^2+)(OH^-)^2
You know y from above. Substitute into the Ksp expression the y value found above and solve for Ksp.
The solubility of Mn(OH)2 is 3.04 x 10^-4 gram per 100 ml of solution .
A) write the balanced chem equation for Mn(OH)2 in aqueous solution
B) calculate the molar solubility of Mn(OH)2 at 25 degrees celcius
C) calculate the value of the solubility product constant, Ksp, for Mn(OH)2 at 25 degrees celcius
1 answer
2 answers