Question

In: Chemistry

9. Calculate the solubility product of each of the following ions from the solubility given: (a)...

9. Calculate the solubility product of each of the following ions from the solubility given:

(a) AgBr, 5.7 x 10 - 7 mole/L

(b) PbF2 , 2.1 x 10 - 3 mole/L

(d) Ag 2CrO 4 , 4.3 x 10 - 2 g//L

Solutions

Expert Solution

Determine the Ksp of silver bromide, given that its molar solubility is 5.71 x 10¯7 moles per liter.

When AgBr dissolves, it dissociates like this:

AgBr (s) ⇌ Ag+ (aq) + Br¯ (aq)

The Ksp expression is:

Ksp = [Ag+] [Br¯]

There is a 1:1 molar ratio between the AgBr that dissolves and Ag+ that is in solution. In like manner, there is a 1:1 molar ratio between dissolved AgBr and Br¯ in solution. This means that, when 5.71 x 10¯7 mole per liter of AgBr dissolves, it produces 5.71 x 10¯7 mole per liter of Ag+ and 5.71 x 10¯7 mole per liter of Br¯ in solution.

Putting the values into the Ksp expression, we obtain:

Ksp = (5.71 x 10¯7) (5.71 x 10¯7) = 3.26 x 10¯13

Ksp = (5.71 x 10¯7) (5.71 x 10¯7) = 3.26 x 10¯13

(b) PbF2 , 2.1 x 10 - 3 mole/L

PbF2 (s) ⇌ Pb2+ (aq) + 2F¯ (aq)

The Ksp expression is:

Ksp = [ Pb2+] [F¯]2

      = (2.1 x 10-3) (4.41 x 10¯3)2 =

Ksp = 4.0841 x 10-8

(d) Ag 2CrO 4 , 4.3 x 10 - 2 g//L

Ag 2CrO 4 (s) ⇌ 2Ag+ (aq) + CrO4¯ (aq)

Ksp = [ Ag+]2 [CrO4¯]

       = [8.6 x 10-2]2 [4.3 x 10- 2]

Ksp= 3.18 x 10-5


Related Solutions

9. Calculate the solubility product of each of the following ions from the solubility given: (a)...
9. Calculate the solubility product of each of the following ions from the solubility given: (a) AgBr, 5.7 x 10 - 7 mole/L (b) PbF2 , 2.1 x 10 - 3 mole/L (d) Ag 2CrO 4 , 4.3 x 10 - 2 g//L
± Introduction to Solubility and the Solubility Product Constant Learning Goal: To learn how to calculate...
± Introduction to Solubility and the Solubility Product Constant Learning Goal: To learn how to calculate the solubility from Kspand vice versa. Consider the following equilibrium between a solid salt and its dissolved form (ions) in a saturated solution: CaF2(s)⇌Ca2+(aq)+2F−(aq) At equilibrium, the ion concentrations remain constant because the rate of dissolution of solid CaF2 equals the rate of the ion crystallization. The equilibrium constant for the dissolution reaction is Ksp=[Ca2+][F−]2 Ksp is called the solubility product and can be...
DQ 11: Given that the solubility product of PbI2 is expressed as Ksp = [Pb2+][I–]2, calculate...
DQ 11: Given that the solubility product of PbI2 is expressed as Ksp = [Pb2+][I–]2, calculate the Ksp of PbI2 from the concentration of Pb2+ found in Step 6 of the Data Analysis. (Hint: Think about the stoichiometry involved when PbI2 was initially formed… how much I– was left unreacted?) Is PbI2 a soluble or insoluble salt? Explain. 3mL of 0.05M KI was used and 1mL of 0.05 Pb(NO3)2 was used to make the PbI2 solution/yellow precipitate All work must...
Calculate the molar solubility of Ag2CrO4(s) in (Solubility Product Ksp at 25 °C is 9.0 ×...
Calculate the molar solubility of Ag2CrO4(s) in (Solubility Product Ksp at 25 °C is 9.0 × 10−12) A) pure water B) in 0.500 L of a solution containing 0.950 g K2CrO4
The molar solubility of Cu3PO4 is 1.59 ⋅ 10^− 3 M. Calculate the solubility of each...
The molar solubility of Cu3PO4 is 1.59 ⋅ 10^− 3 M. Calculate the solubility of each ion in a saturated solution:
Calculate the molar solubility and the solubility in g/L of each salt at 25oC: a) PbF2...
Calculate the molar solubility and the solubility in g/L of each salt at 25oC: a) PbF2 Ksp = 4.0 x 10-8 b) Ag2CO3 Ksp = 8.1 x 10-12 c) Bi2S3 Ksp = 1.6 x 10-72
Calculate the solubility of Copper (II) Phosphate salt at equilibrium in aqueous solution. Solubility product constant...
Calculate the solubility of Copper (II) Phosphate salt at equilibrium in aqueous solution. Solubility product constant (Ksp) of Copper (II) Phosphate is 2.4 * 10-15mol/L at 25°C
Calculate the concentration of all ions present in each of the following solutions of strong electrolytes....
Calculate the concentration of all ions present in each of the following solutions of strong electrolytes. 0.800 mole of Ca(NO3)2 in 600.0 mL of solution MCa2+ = ______  M MNo3- = _______ M
Calculate the concentration of all ions present in each of the following solutions of strong electrolytes....
Calculate the concentration of all ions present in each of the following solutions of strong electrolytes. (a) 0.260 mole of Ca(NO3)2 in 100.0 mL of solution Ca2+ M? NO3− ?M (b) 5.5 moles of Na2SO4 in 1.25 L of solution Na+? M SO42− ? M (c) 5.00 g of NH4Cl in 490.0 mL of solution NH4+? M Cl − ?M (d) 1.00 g K3PO4 in 300.0 mL of solution K + ? M PO43− ? M
Calculate the molar solubility of CaO (Ksp = 1.27x10-36) in each of the following liquids or...
Calculate the molar solubility of CaO (Ksp = 1.27x10-36) in each of the following liquids or solutions. a) pure water b) 0.25 M CaCl2 c) 0.20 M Na2O
ADVERTISEMENT
ADVERTISEMENT
ADVERTISEMENT