if the solubilty of AgC2H3O2 is 5.0 x10^-2mol/L. What is the Ksp?
To find the Ksp (solubility product constant) for AgC2H3O2 based on its solubility, you need to know the balanced chemical equation for its dissolution. Let's assume AgC2H3O2 dissociates into Ag+ and C2H3O2- ions.
The balanced chemical equation for the dissolution of AgC2H3O2 can be written as follows:
AgC2H3O2 (s) ⇌ Ag+ (aq) + C2H3O2- (aq)
From the equation, we can see that one mole of AgC2H3O2 produces one mole of Ag+ and one mole of C2H3O2-. Therefore, Ag+ = C2H3O2- = 5.0 x 10^-2 mol/L.
Now, the solubility product constant (Ksp) expression for AgC2H3O2 can be written as:
Ksp = [Ag+] * [C2H3O2-]
Substituting the molar concentrations of Ag+ and C2H3O2- we obtained from the solubility:
Ksp = (5.0 x 10^-2 mol/L) * (5.0 x 10^-2 mol/L)
Simplifying the expression:
Ksp = 2.5 x 10^-3 mol^2/L^2
Therefore, the Ksp for AgC2H3O2 is 2.5 x 10^-3 mol^2/L^2.
Call AgC2H3O2 as AgAc.
.........AgAc ==> Ag^+ + Ac^-
I.......solid.....0.......0
C.......solid.....x.......x
E.......solid.....x.......x
Ksp = (Ag^+)(Ac^-+
Ksp = (x)(x)
You are given the value of x, substitute that value and solve for Ksp.