Question

2. Calculate the molar solubility of the following:

a. AgCl added to pure water

b. AgCl added to water that is already 0.25 M Cl-

Answer #1

a

AgCl can dissociate in to

AgCl ------> Ag+ + Cl-

Ksp = [Ag+][Cl-] = 1.8 x 10^{-10} (this value is
standadered value taken from the text book)

Let [Ag+] = s. Then [Cl-] = s, and substituting in the Ksp
expression we have

(s)(s) = 1.8 x 10^{-10}

s^{2} =1.8 x 10^{-10}

s= 1.34 x 10^{-5} mol /L

= molar solubility of AgCl

Part B

Ksp = [Ag+][Cl-] = 1.8 x 10^{-10} (this value is
standadered value taken from the text book)

but here in the solution already 0.25 mol/L Cl^{-} is
there

t [Ag+] = s. Then [Cl-] = s +0.25

(s)(s+0.25) = 1.8 x 10^{-10}

s^{2} + 0.25s - 1.8 x 10^{-10} = 0

solve the quadratic equation

s =7.20 x 10^{-10} mol/L

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...

The molar solubility of AgBr in pure water is 7.3x10^-7 M.
Calculate the Ksp.

Calculate the molar solubility of CuX(Ksp=1.27×10?36)
in each of the following.
Part A
pure water
Express your answer using three significant figures.
Part B
0.25 M CuCl2
Express your answer using two significant figures.
Part C
0.23 M Na2X
Express your answer using two significant figures.

Determine the molar solubility of NiC2O4 in the following
solutions.
a) pure water
b) 150.0 mL of a 0.010 M Ni(NO3)2
c) 150.0 mL of a 0.500 M AlCl3.
d) 150.0mL of a 0.030 M Na2C2O4

What is the molar solubility of plumbous sulfate in a) pure
water; and b) in 0.0500 M plumbous nitrate? Ksp plumbous sulfate =
1.6x10-8

Calculate the solubility of MnCO3
(a) in pure water and (b) in a solution in which
[CO32-] =
0.285 M.
Solubility in pure water = ______M
Solubility in 0.285 M
CO32- = ______M

Calculate the solubility of NiCO3
(a) in pure water and (b) in a solution in which
[CO32-] =
0.283 M.
*Ksp NiCO3 = (6.6 × 10-9)
Solubility in pure water = ______M
Solubility in 0.283 M
CO32- = ______M

A.) Calculate the solubility in g/L of AgBr in pure water.
B.) Calculate the solubility in g/L of AgBr in 0.0018 M NaBr.
(Enter answer in scientific notation.)

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

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)

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