When solid silver chloride (MM=143.4) is added to 100ml of H2O, 1.9x10^-4 grams dissolves. What is the Ksp for

Question

.....for silver chloride?

Answer 1

Convert the mass that dissolved into moles by dividing by the molar mass of AgCl. Since you dissolved that many moles in 100 mL (0.100L), multiply that number of moles by 10 to get moles AgCl/L. Now to calculate Ksp, you recognize that the concentration of Ag+ ions is equal to Cl- ions, and that they are both equal to the concentration of AgCl dissolved.

So, multiply the [Ag+] time [Cl-], and you have Ksp.

Answer 2

The equilibrium for the satured solution is

AgCl <> Ag+ + Cl-

and the equilibrium condition is given by

Ksp = (Ag+)(Cl-)

1.9 10^-4 g AgCl is 1.9 10^-4 / 143.3= 1.33 10^-6 mole

the volume is 0.100 L

Concentration of dissolved AgCl is 1.33 10^-6 / 0.100=1.33 10^-5 M

Ksp= (1.33 10^-5)^2 = 1.76 10 ^-10

Answer 3

ksp= 1.32*10^-5 =x


x^2=1.74*10^-10