Question

Calculate the molar solubility of Ag2CrO4 (Ksp = 1.1 × 10-12) at 25 °C in various aqueous solutions.

Calculate the solubility in 0.249 *M*
AgNO_{3}

Calculate the solubility in 0.134 *M*
Na_{2}CrO_{4}

Answer #1

Ag2CrO4 (s) <------------> 2Ag+ + CrO4^{-2}

x 0 0 initial moles

- 2x x at equilibrium

Thus Ksp = [Ag+]^{2}[CrO4-2] = 1.1x10^{-12}

Now

1) in 0.249M AgNO3

Ag2CrO4 (s) <------------> 2Ag+ + CrO4^{-2}

s 0.249 0 initial moles

- 0.249+x s at equilibrium

= 0.249 s as s is very very small compared to 0.249 due to common ion

Thus Ksp = [Ag+]^{2}[CrO4-2] =
1.1x10^{-12}

= (0.249)^{2} [s] = 1.1x10^{-12}

Thus s = 1.774 x10^{-11} M

Thus the solubility is very much decreased due to common ion effect.

2) in 0.134 M Na2CRO4

Ag2CrO4 (s) <------------> 2Ag+ + CrO4^{-2}

s 0 0.134 initial moles

- s 0.134 +s =0.134 at equilibrium

Thus Ksp = [Ag+]^{2}[CrO4-2] =
1.1x10^{-12}

= s^{2} (0.134) = 1.1x10^{-12}

Hence s = 2.86x 10^{-6} M

Thus the solubility is decreased than in pure water , but not as much with silver nitrate, due to common ion effect.

Calculate the molar solubility of Ag2CrO4
(Ksp = 1.1 × 10-12) at 25 °C in
various aqueous solutions.
A)Calculate the solubility in 0.200 M
AgNO3
B)Calculate the solubility in 0.200 M
Na2CrO4

Ksp for Ag2CrO4=5.4x10^-12. Calc molar solubility of Ag2CrO4 in
0.0050M K2CrO4

Gold(III) chloride, AuCl3, has Ksp = 3.2 x 10-25. Calculate the
molar solubility of gold(III) chloride in pure water and in various
aqueous solutions.
A) Calculate the molar solubility of gold(III) chloride in pure
water.
B) Calculate the molar solubility of gold(III) chloride in 0.010
M HCl solution.

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?

Gold(III) chloride, AuCl3, has
Ksp= 3.2 x 10-25. Calculate the
molar solubility of gold(III) chloride in pure water and in various
aqueous solutions.
Put your answers with 2 significant figures.
Calculate the molar solubility of gold(III) chloride in 0.010
M Au(NO3)3 solution.
Enter your response in scientific notation, e.g. enter 2E3 for
2000

Rank the following salts in order of increasing molar
solubility. Salt Ksp AgSCN 1.0 × 10–12 Ag2CrO4 1.1 × 10–12 Ag3PO4
1.0 × 10–16

Use the Ksp values to calculate the molar solubility of each of
the following compounds in pure water.
MX (Ksp = 1.47×10−38)
Ag2CrO4 (Ksp = 1.12×10−12)

3a. Write the balanced reaction and solubility product
expression (KSP) for dissolving
silver chromate:
Ag2CrO4(s).
Include all charges, stoichiometric coefficients, and phase
subscripts. (4 pts)
c. Determine [Ag+1]
and [CrO4−2] fo
a saturated solution of
Ag2CrO4
if KSP = 1.1 ×
10−12. Also, determine the molar
solubility. (8 pts)
d. Use the KSP above
to determine
[CrO4−2] for a
solution that is saturated with
Ag2CrO4,
and also has a common ion effect where
[Ag+1] = 0.495 M. (4
pts)

Use the Ksp values to calculate the molar solubility of each of
the following compounds in pure water.
Part A MX (Ksp = 9.20×10−11) Express your answer in moles per
liter.
Part B Ag2CrO4 (Ksp = 1.12×10−12)
Part C Ca(OH)2 (Ksp = 4.68×10−6) Express your answer in moles
per liter.

The solubility-product constant (Ksp) for
MnCO3 at 25°C is 2.2 ✕ 10−11. What is the
molar solubility of this substance in 0.22 M
MnCl2 at 25°C?
AND
Calculate the Qsp or
Ksp, as indicated, and determine whether a
precipitate will form when each of the following mixtures is
prepared. (You may assume temperature is held constant, volumes are
additive, and that the initial solutions, prior to mixing, are
unsaturated.)
(a) 25.12 mL 1.30 ✕ 10−4M CaCl2
is mixed with 25.19...

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