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.

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

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)

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

What is the molar solubility of silver bromide in each of the
following solutions?
a. pure water
b. 0.0550 M sodium bromide
c. 0.250 M silver nitrate

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 .

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