Question

a. The K_{sp} for Ag_{2}SO_{3} = 1.50 X
10^{-14}. What is the molar solubility of
Ag_{2}SO_{3} in a 5 M solution of lithium
sulfite?

b.The K_{sp} for
Mg_{3}(PO_{4})_{2} = 1.04 X
10^{-24}. What is the molar solubility of
Mg_{3}(PO_{4})_{2} in a 1.40 M solution of
sodium phosphate?

c.If the Ksp for Y(OH)_{3} = 1.00 X 10^{-22},
what is the molar solubility of Y(OH)_{3} in a buffer
solution composed of 1.60M trimethylamine (=
(CH_{3})_{3}N) (K_{b} = 6.5 X
10^{-5}) and 1.40M trimethylaminium hydrochloride (=
(CH_{3})_{3}NH^{+}Cl^{-})?

Answer #1

Q1.

Ksp = [Ag+]^2[SO3-2]

1.5*10^-14 = (2S)^2 * (5)

S = ((1.5*10^-14)/20)^0.5

s = 2.738*10^-8 M;

Q2.

Ksp = [Mg+2]^3 [ PO4-3]^2

let S = moalr solubility of Mg3(PO4)2

[Mg+2] = 3S

[PO4-3] = 2S

substitute in Ksp

(1.04*10^-24) = (3S)^3 * (2S)^2

108*S^5 = (1.04*10^-24)

S = ((1.04*10^-24)/108 )^(1/5)

S = 0.000006262 M for Mg3(PO4)2

Q3

Ksp = [Y+3][OH-]^3

given bufer

pOH = pKb + log(Bh+/B)

pKb = -log(Kb) = -log(6.5*10^-5) = 4.1870

pOH = 4.1870 + log(1.4/1.4)

pOH = 4.1870

[Oh-] = 10^-pOH = 10^-4.1870 = 6.5*10^-5

Ksp = [Y+3][OH-]^3

10^-22 = S*( 6.5*10^-5)^3

S = (10^-22)/(( 6.5*10^-5)^3)

S = 3.6413*10^-10 M

If the Ksp for Co(OH)2 = 5.92 X 10-15, what is the
molar solubility of Co(OH)2 in a buffer solution
composed of 1.80M trimethylamine (= (CH3)3N)
(Kb = 6.5 X 10-5) and 1.00M trimethylaminium hydrochloride (=
(CH3)3NH+Cl-)?

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?

What is the molar solubility of Mg(OH)2,
Ksp is 5.6 x 10-12 for
Mg(OH)2, in the following aqueous solutions?
A. Calculate the molar solubility in 0.24 M NaOH:
B. Calculate the solubility in 0.24 M
MgSO4?

The Ksp for Ag2SO4 = 1.20 X 10-5. What is the molar solubility
of Ag2SO4 in a 2.20M solution of aluminum sulfate?

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

What is the molar solubility (in mol/L) of Pb(OH)2 (Ksp = 5.06 ⋅
10 − 13 ) in a solution buffered at 11.21.

21. (a) Determine the molar solubility of Fe(OH)3 in pure water.
Ksp = 2.79 × 10-39 for Fe(OH)3. (b) Determine the molar
solubility of Fe(OH)3 if the pH of the solution is 8.0. (c)
Determine the molar solubility of Fe(OH)3 if the pH of the solution
is 2.0.
Can someone go over with me the work for this problem? The
answer is given I just dont know how they got those answers.
Answer: (a) S or x = 1.01 × 10-10...

The solubility product constant Ksp of
Mn(OH)2 is 2.1 x 10-13 at 25oC.
The molar mass of Mn(OH)2 is 88.96 g/mol.
a. Calculate its molar solubility
b. Calulate its solubility in g/L

A)Based on the given value of the Ksp , what is the
molar solubility of Mg(OH)2 in pure H2O ?
2.41×10−4 M
B)Based on the given value of the Ksp , what is the
molar solubility of Mg(OH)2 in 0.200 M NaOH ?
Ksp , of 5.61×10−11
D) What is the pH change of a 0.300 M solution of
citric acid (pKa=4.77 ) if citrate is added to a
concentration of 0.140 M with no change in volume?

Question 1 :
The solubility product, Ksp, of
Cd3(PO4)2 is 2.5 x
10-33. What is the solubility (in g/L) of
Cd3(PO4)2 in pure water?
Question 2 :
The solubility product of Cu(OH)2 is 4.8 x
10-20. Calculate the value of pCu2+, or
-log[Cu2+], in an aqueous solution of NaOH which has a
pH of 12.89 and is saturated in Cu(OH)2.
Question 3 :
The equilibrium constant for the formation of
Cu(CN)42- is 2.0 x 1030. Calculate
the value of pCu2+,...

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