(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 6.25e-06 g of Cd3(PO4)2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Cd3(PO4)2.
Ksp =
(c) The Ksp of Sc(OH)3 at 25 oC is 2.22e-31. What is the molar solubility of Sc(OH)3?
solubility = mol/L
a)
At equilibrium:
PbBr2 <----> Pb2+ + 2 Br-
s 2s
Ksp = [Pb2+][Br-]^2
Ksp = (s)*(2s)^2
Ksp = 4(s)^3
Ksp = 4(1.18*10^-2)^3
Ksp = 6.572*10^-6
Answer: 6.57*10^-6
b)
S = 6.52*10^-6 g / 100 mL
S = 6.52*10^-6 g / 0.1 L
S = 6.52*10^-5 g /L
Molar mass of Cd3(PO4)2,
MM = 3*MM(Cd) + 2*MM(P) + 8*MM(O)
= 3*112.4 + 2*30.97 + 8*16.0
= 527.14 g/mol
Molar mass of Cd3(PO4)2= 527.14 g/mol
s = 6.52*10^-5 g/L
To covert it to mol/L, divide it by molar mass
s = 6.52*10^-5 g/L / 527.14 g/mol
s = 1.237*10^-7 mol/L
At equilibrium:
Cd3(PO4)2 <----> Cd2+ + 2 PO43-
s 2s
Ksp = [Cd2+][PO43-]^2
Ksp = (s)*(2s)^2
Ksp = 4(s)^3
Ksp = 4(1.237*10^-7)^3
Ksp = 7.569*10^-21
Answer: 7.57*10^-21
C)
At equilibrium:
Sc(OH)3 <----> Sc3+ + 3 OH-
s 3s
Ksp = [Sc3+][OH-]^3
2.22*10^-31=(s)*(3s)^3
2.22*10^-31= 27(s)^4
s = 9.522*10^-9 M
Answer: 9.52*10^-9 M
(a) If the molar solubility of PbBr2 at 25 oC is 0.0118 mol/L, what is the...
(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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