Question

chromate is sparingly soluble in aqueous solutions. The Ksp of Ag2CrO4 is 1.12×10−12 . What is the solubility (in mol/L) of silver chromate in 1.00 M potassium chromate aqueous solution?

Answer 1

`6.5X10^-^5~(mol)/(L)`

Step-by-step explanation:

For this question, we have to start with the ionization equation for
`Ag_2CrO_4_(_s_)`, so:

`Ag_2CrO_4_(_s_)~<->~2Ag^+~_(_a_q_)~+~CrO_4^-^2_(_a_q_)`

With this in mind we can write the Ksp expression:

`Kps~=~[Ag^+]^2[CrO_4^-^2]`

Additionally, for every mole of
`CrO_4^-^2` formed, 2 moles of
`Ag^+` are formed. We can use "X" for the unknown concentration of each ion, so:

`[CrO_4^-^2]~=~X` and
`[Ag^+]~=~2X`

Now, we can plug the values into the Ksp expression:

`1.12x10^-^1^2~=~(2X)^2(X)`

Now we can solve for "X" :

`1.12x10^-^1^2~=~4X^3`

`X^3=(1.12X10^-^1^2~)/(4)`

`X=((1.12X10^-^1^2~)/(4))^(^1^/^3^)`

`X=6.5X10^-^5~(mol)/(L)`

I hope it helps!