MX (Ksp = 5.67×10−36)
Use the Ksp values to calculate the molar solubility of each of the following compounds in pure water.
No compounds are given, hence I am using the generic formula of a salt MX where it dissociates to give M+ metal ion and X- halide ion.
The dissociation equilibrium reaction can be written as:
MX(s) M+(aq) + X-(aq)
Ksp = [M+] [X-] / [MX]
As Ksp is very very low we can consider [MX] to be constant.
Ksp = [M+] [X-] = 5.67×10^−36
Let's say [M+] = [X-] = x
then x^2 = 5.67×10^−36
x = (5.67×10^−36)^0.5
x = 2.3812*10^-18 M
Thus the molar solubility of MX is 2.3812*10^-18 M.
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