Ksp = (Ag^+)(Cl^-) = 1.8E-10
Ksp = (x)(x) = x^2
1.8E-10 = x^2
Now, we need to solve for x:
x^2 = 1.8E-10
x = sqrt(1.8E-10)
x ≈ 1.34E-5
So, the concentration of silver ions (Ag^+) in the saturated solution is approximately 1.34 * 10^-5 M.
To find the total ion concentration, you need to add the concentrations of both ions (Ag^+ and Cl^-), which are equal, x and x.
Total ion concentration = (Ag^+) + (Cl^-)
Total ion concentration = x + x
Total ion concentration = 2 * 1.34E-5
Total ion concentration ≈ 2.68 * 10^-5 M
So the Ksp for silver chloride is 1.8*10^-10, how could I find the concentration of silver ions in this saturated solution. Then how I find the total ion concentration?
AgCl ==> Ag^+ + Cl^-
Let AgCl solubility is x.
Then (Ag^+) is x and (Cl^-) is x
Ksp = (Ag^+)(Cl^-) = 1.8E-10
Substitute x into the Ksp expression and solve for x. Twice that will be the total ion concentration (neglecting the ionization of water).
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