Question

Which of the following has the highest molar solubility?

a) AgCl: Ksp = 1.8 x 10^-10

b) CaF2: Ksp = 3.4 x 10^-11

c) Bi2S3: Ksp = 1.1 x 10^-73

Answer #1

What is the molar solubility of AgCl in 0.30 M NH3? Ksp for AgCl
is 1.8 x 10-10 and Kf for Ag(NH3)2 + is 1.7 x 107 .

Which of the following has the greatest molar solubility?
Ca3(PO4)2 Ksp = 1.0 x 10-26
CaF2 Ksp = 3.4 x 10-11
CaCO3 Ksp = 3.9 x 10-9
CaC2O4 Ksp = 2.3 x 10-9
CaSO4 Ksp = 2.4 x 10-5

Which of the following salts has the lowest molar solubility?
Show work.
A.) SrCO3 (Ksp = 9.3 x 10^-10)
B.) MnS (Ksp = 2.5 x 10^-10)
C.) BaF2 (Ksp = 1 x 10^-6)
D.) BaSO4 (Ksp = 1.1 x 10^-10)
E.) AgCl (Ksp = 1.8 x 10^-10)

1. The Ksp for AgCl is 1.6 x 10-10
(a) What is the molar solubility of AgCl?
(b) What is the solubility in g/L solution?
2. The Ksp of Ag2CO3 is 8.1 x 10-12
(a) What is the molar solubility of Ag2CO3
(b) What is the molar solubility of [Ag+]?
(c) what is the solubility of Ag2CO3?

10. Given that the solubility product (Ksp) for AgCl
in water is 1.8 x 10-10, calculate ΔGo at
25oC for: Ag+(aq) + Cl-(aq) ↔ AgCl(s)

Rank the following salts in order of increasing molar
solubility
BaSO4 = 1.1 x 10-10
AgCl = 1.8 x 10-10
BaCO3 = 9.1 x 10-9
CdS = 8 x 10-27
PbSO4 = 1.8 x 10-8
Please explain, thanks!

Which of the following has the greatest solubility in water?
(A) ZnCr2O4 ( Ksp = 2.7 x
10-8)
(B) BaCrO4 ( Ksp = 2.3 x 10-10
)
(C) CaF2 ( Ksp = 3.9 x
10-11)
(D) AgBr ( Ksp = 5.0 x 10-13 )

The Ksp of Fe(OH)2 is 1.8 x 10–15. At what pH will a
0.50 M Fe2+ solution begin to show precipitation of Fe(OH)2?
Rank the molar solubility of the following substances in an
increasing order.
Drag and drop to order
1
A
BaF2 (Ksp=2.4 x 10−5)
2
B
CaF2 (Ksp=4.0 x 10−11)
3
C
PbF2 (Ksp=4 x 10−8)

Which of the following compounds will have the highest molar
solubility in pure water? Which of the following compounds will
have the highest molar solubility in pure water?
PbS, Ksp = 9.04 × 10-29
AgCN, Ksp = 5.97 × 10-17
NiS, Ksp = 3.00 × 10-20
MgCO3, Ksp = 6.82 × 10-6
PbSO4, Ksp = 1.82 × 10-8

The molar solubility of AgCl in 6.5 x10^-3 M AgNO3 is 2.5x10^-8
M. In deriving Ksp from these data, which of the following
assumptions is (are) reasonable
A. Ksp is the same as solubility
B. Ksp of AgCl is the same in 2.5x10^-8 M AgNO3 as in pure
water
C. Solubility of AgCl is independent of the concentration of
AgNO3
D. [Ag+] does not change significantly upon addition of AgCl to
6.5x10^-3 M AgNO3
E. [Ag+] after the addition of...

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