Solubility Lesson 7 Changing solubility

SolubilityLesson 7

Changing solubility

When to and When not to Multiply the Molarity 1. The molar solubility of Ba(OH)2 is 2. Equal volumes of 0.0010 M Ba(NO3)2 and 0.0010 M. Ksp = ? 0.0010 M NaOH are mixed. Will a

precipitate occur?

Ba(OH)2(s) ⇌ Ba2+ + 2OH- Ba(OH)2(s) ⇌ Ba2+ + 2OH-

s s 2s 10.0010 1 0.0010 M 2 2

0.00050 M 0.00050 M

Multiply by 2 because of Ba(OH)2(s) Do not multiply by 2 because of NaOH

Ksp = [Ba2+][OH-]2 TIP = [Ba2+][OH-]2

Ksp = [s][2s]2 TIP = [0.00050][0.00050]2

Ksp = 4s3

Ksp = 4[0.0010]3 TIP = 1.25 x 10-10

Ksp = 4.0 x 10-9 TIP < Ksp No ppt.

3. AgNO3(s) is added to 1.0 L of a solution containing Cl- in order to precipitate out the Cl- as AgCl(s). After the AgCl(s) is filtered out what is the remaining concentration of Cl-?

AgCl(s) ⇌ Ag+ +Cl-

Ksp = s2

1.8 x 10-10 = s2

s = [Cl-] = 1.3 x 10-5 M

Changing the Solubilty of a Salt

energy + AgCl(s) ⇄ Ag+ + Cl-

The molar solubility is the amount of AgCl(s) in moles per litre that dissolves into ions to form a saturated solution.

The molar solubility is the amount of AgCl(s) in moles per litre that dissolves into ions to form a saturated solution. If this equilibrium shifts to the right, the molar solubility increases.

The molar solubility is the amount of AgCl(s) in moles per litre that dissolves into ions to form a saturated solution. If this equilibrium shifts to the right, the molar solubility increases. If this equilibrium shifts to the left, the molar solubility decreases.

The molar solubility is the amount of AgCl(s) in moles per litre that dissolves into ions to form a saturated solution. If this equilibrium shifts to the right, the molar solubility increases. If this equilibrium shifts to the left, the molar solubility decreases. Like all equilibriums, only changing the temperature changes the Ksp.

The molar solubility is the amount of AgCl(s) in moles per litre that dissolves into ions to form a saturated solution. If this equilibrium shifts to the right, the molar solubility increases. If this equilibrium shifts to the left, the molar solubility decreases. Like all equilibriums, only changing the temperature changes the Ksp. Most solid equilibriums are endothermic.

Changing the Solubility of a Salt

Substance Added Effect on Molar Solubility Effect on Ksp AgNO3

Increases the [Ag+] and shifts the equilibrium left

Substance Added Effect on Molar Solubility Effect on Ksp AgNO3 Decrease none

Increases the [Cl-] and shifts the equilibrium left

NaCl Decrease none

Na2SIncreases the [Cl-] and shifts the equilibrium left

NaCl Decrease none

Na2S S2- is low solubility with Ag+ so they react and [Ag+] decreases

NaCl Decrease none

Na2S Increase none

Pb(NO3)2

NaCl Decrease none

Na2S Increase none

Pb(NO3)2Pb2+ is low solubility with Cl- so they react and [Cl-] decreases

NaCl Decrease none

Na2S Increase none

Pb(NO3)2 Increase none

NaCl Decrease none

Na2S Increase none

H2OThe molar solubility is the number moles per litre and therefore does not change when more water is added.

NaCl Decrease none

Na2S Increase none

H2O none none

NaCl Decrease none

Na2S Increase none

H2O none none

AgCl is a solid that the solution is already saturated with and it does not change the solubility

NaCl Decrease none

Na2S Increase none

H2O none none

AgCl none none

Increase Temperature

NaCl Decrease none

Na2S Increase none

H2O none none

AgCl none none

Shifts to the right and increases the ksp

NaCl Decrease none

Na2S Increase none

H2O none none

AgCl none none

Increase Temperature Increase Increase

Decrease Temperature

NaCl Decrease none

Na2S Increase none

H2O none none

AgCl none none

NaCl Decrease none

Na2S Increase none

H2O none none

AgCl none none

Decrease Temperature Decrease Decrease

Ca(OH)2(s) ⇄ Ca2+ + 2OH- Substance Added Effect on Molar Solubility Effect on Ksp Ca(NO3)2

Ca(OH)2(s) ⇄ Ca2+ + 2OH- Substance Added Effect on Molar Solubility Effect on Ksp Ca(NO3)2 Decrease none

Na2SO4

Na2SO4 Increase none

NaOH Decrease none

HCl Increase none

NaOH Decrease none

HCl Increase none

NaCl none none

Ca(OH)2

NaOH Decrease none

HCl Increase none

NaCl none none

Ca(OH)2 none none

NaOH Decrease none

HCl Increase none

NaCl none none

Ca(OH)2 none none

NaOH Decrease none

HCl Increase none

NaCl none none

Ca(OH)2 none none

Decrease Temperature Decrease Decrease

Solubility Lesson 7 Changing solubility

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