a)
At equilibrium:
Ag3PO4 <----> 3
Ag+
+
PO43-
3s s
Ksp = [Ag+]^3[PO43-]
Ksp = (3s)^3*(s)
Ksp = 27(s)^4
Ksp = 27(4.26*10^-5)^4
Ksp = 8.892*10^-17
Answer: 8.89*10^-17
b)
S = 0.434 g / 100 mL
S = 0.434 g / 0.1 L
S = 4.34 g /L
Molar mass of PbBr2,
MM = 1*MM(Pb) + 2*MM(Br)
= 1*207.2 + 2*79.9
= 367 g/mol
Molar mass of PbBr2= 367 g/mol
s = 4.34 g/L
To covert it to mol/L, divide it by molar mass
s = 4.34 g/L / 367 g/mol
s = 1.183*10^-2 mol/L
At equilibrium:
PbBr2 <---->
Pb2+
+ 2
Br-
s 2s
Ksp = [Pb2+][Br-]^2
Ksp = (s)*(2s)^2
Ksp = 4(s)^3
Ksp = 4(1.183*10^-2)^3
Ksp = 6.615*10^-6
Answer: 6.62*10^-6
c)
At equilibrium:
Ga(OH)3 <---->
Ga3+
+ 3
OH-
s
3s
Ksp = [Ga3+][OH-]^3
7.28*10^-36=(s)*(3s)^3
7.28*10^-36= 27(s)^4
s = 7.206*10^-10 M
Answer: 7.21*10^-10 M
(a) If the molar solubility of Ag3PO4 at 25 °C is 4.26e-05 mol/L, what is the...
#40. (a) If the molar solubility of Ag3PO4 at 25 oC is 4.26e-05 mol/L, what is the Ksp at this temperature? Ksp = ____ (b) It is found that 6.17e-05 g of YF3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for YF3. Ksp = ___ (c) The Ksp of Cd3(AsO4)2 at 25 oC is 2.20e-33. What is the molar solubility of Cd3(AsO4)2? solubility = ____mol/L
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(a) If the molar solubility of PbBr2 at 25 oC is 0.0118 mol/L, what is the Ksp at this temperature? Ksp = _______ (b) It is found that 9.14e-08 g of Sc(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Sc(OH)3. Ksp = ______ (c) The Ksp of Zn3(AsO4)2 at 25 oC is 2.80e-28. What is the molar solubility of Zn3(AsO4)2? solubility = ________mol/L
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