Calculate the values of [Cu++] and of [IO3-] in a solution made by saturating pure water with Cu(IO3)2.?

Question

"Calculate the values of [Cu++] and of [IO3-] in a solution made by saturating pure water with Cu(IO3)2. (Ksp = 1.4 x 10^-5). What is the molar solubility of Cu(IO3)2?"

This is a question in my chemistry laboratory notebook, and it has me confused. How can I deduce those concentrations if I am not given a starting concentration? I am not familiar with the expression "saturating pure water with x"... is this telling me the inital concentration of Cu(IO3)2?

Thanks!

Answer 1

Ksp equals the solubility product constant

Ksp = {Cu++][IO3]^2 = 1.4x10^-5

Let X = Moles/L of Cu(IO3)2 that dissolve

[Cu++] = X

[IO3-] = 2X

Ksp = X (2x)^2 = 4x^3 = 1.4x10^-5

X = 1.5x10^-2

Cu++ = 1.5x10^-2 M

IO3- = 3.0x10^-2 M

Answer 2

the h**l if i know