if 1.7L of a saturated solution of AgC2H2O2 is found to contain 14.1g of AgC2H3O2. What is the Ksp of AgC2H3O2?

You work this one in reverse from your post on determining the Ksp for AgAc. mols AgC2H3O2 = 14.1 molar mass AgC2H3O2 = approx 0.08

M AgAc = 0.08 AgAc/1.7L = approx 0.05 mols/L.
........AgAc ==> Ag^+ + Ac^-
I.......solid....0.......0
C.......solid....x.......x
E.......solid....x.......x

Ksp = (Ag^+)(Ac^-)
Ksp = (x)(x)
You know the value of x, substitute and solve for Ksp.

To find the Ksp (solubility product constant) of AgC2H3O2, we need to use the given information about the solubility of AgC2H3O2.

First, let's determine the number of moles of AgC2H3O2 present in the solution:
1. Convert the mass of AgC2H3O2 to moles using its molar mass. The molar mass of AgC2H3O2 is calculated as follows:
Molar mass(M) = M(Ag) + 2 * M(C) + 3 * M(H) + 2 * M(O)
= 107.87 + 2 * 12.01 + 3 * 1.008 + 2 * 16.00
= 143.92 g/mol

Mass = 14.1 g
Moles of AgC2H3O2 = Mass / Molar mass
= 14.1 g / 143.92 g/mol

Next, we can use the given volume of the saturated solution to calculate the concentration of AgC2H3O2:
Volume = 1.7 L
Concentration (C) = Moles / Volume

Now, let's use the concentration of AgC2H3O2 to write the expression for Ksp.
AgC2H3O2 (s) ⇌ Ag+ (aq) + C2H3O2− (aq)

The solubility product constant (Ksp) expression is written as:
Ksp = [Ag+] * [C2H3O2−]

Since the solute AgC2H3O2 completely dissociates to form Ag+ and C2H3O2−, the concentrations of Ag+ and C2H3O2− are equal to each other.

Therefore, Ksp = [Ag+]^2

We know that the concentration of Ag+ is equal to the concentration of C2H3O2−, which can be calculated using the molarity formula, M = moles / volume.

Substituting the values into the molarity formula, we get:
[Ag+] = [C2H3O2−] = Moles / Volume

Finally, we can calculate the Ksp by substituting the concentrations into the Ksp expression:
Ksp = ([Ag+] * [C2H3O2−])^2
= ([Moles / Volume] * [Moles / Volume])^2

Now, let's plug in the values and calculate the Ksp.