If a dilute AgNO3 solution is slowly added to the solution, what is the first compound to precipitate: Ag2CrO4 ( Ksp = 1.2×10?12), Ag2CO3 ( Ksp = 8.1×10?12), or AgCl ( Ksp = 1.8×10?10)?
You have to apply the definition of Ksp (constant equilibrium solubility):
for the first one CrO4-2
Ag2CrO4 === 2 Ag+ + CrO4-2
........................2x.....................x
we already know the concentration of [CrO4] = 0.2
ksp = 1.2 x 10-12 = 4x2 * 0.2
4x2 = 1.2 x 10-12 / 0.2
x = 6.12 x 10-7 M
for the second ion
Ag2CO3 ==== 2 Ag + CO3
.........................2x..............x
ksp = 8.1 x 10-12
ksp = (2x)2 * x
concentration of CO3 is 0.1M
8.1 x 10-12 = 4x2 * 0.1
x = 4.5 x 10-6
fo the chloride
AgCl ==== Ag + Cl
...................x.........x
ksp = 1.8 x 10-10 = x (0.01)
the concentration of cl is 0.01
x = 1.8 x 10-8 M
according to the calculations we need a small amount of Cl (compared to the other anions) to produce a precipitate so the first compound to precipitate is AgCl
*hope it helps =)
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