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Solubility Review. 1. Solubility is a measure of the maximum amount of solid that will dissolve in a volume of water. Units: g/L mol/L g/100mL Or even: mL/L for CO 2(g) in water Ksp Solubility Product Saturated solutions No Units Only Changes with Temperature No ICE!

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1. Solubility is a measure of the maximum amount of solid that will dissolve in a volume of water.

Units: g/Lmol/Lg/100mL

Or even: mL/L for CO2(g) in water

Ksp

Solubility Product

Saturated solutions

No Units

Only Changes with Temperature

No ICE!

Step #1 Write a dissociation equation for the low solubility salt

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2. The solubility (s) of BaCO3 is 5.1 x 10-5 M @ 250 C. Calculate the solubility product or Ksp.

Dissociation net ionic BaCO3(s)⇌ Ba2+ + CO32-

s s s

Ksp = [Ba2+][CO32-]

Ksp = s2

Ksp = (5.1 x 10-5)2

Ksp = 2.6 x 10-9

Adding BaCO3does notincrease [Ba2+] or [CO32-] but it does increase the rate of dissolving and crystallization.

Formation Net Ionic: Ba2+ + CO32- BaCO3(s)

Ba2+

CO32-

BaCO3(s)

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2. The solubility (s) of BaCO3 is 5.1 x 10-5 M @ 250 C. Calculate the solubility product or Ksp.

BaCO3(s)⇌ Ba2+ + CO32-

s s s

Ksp = [Ba2+][CO32-]

Ksp = s2

Ksp = (5.1 x 10-5)2

Ksp = 2.6 x 10-9

Adding BaCO3does notincrease [Ba2+] or [CO32-] but it does increase the rate of dissolving and crystallization.

Formation Net Ionic:Ba2+ + CO32- BaCO3(s)

Ba2+

CO32-

BaCO3(s)

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4. 200.0 mL 0.10 M Pb(NO3)2 is mixed with 300.0 mL of 0.20 M NaCl, will a precipitate occur?

PbCl2(s)⇌ Pb2+ + 2Cl-

200 0.10 M 300 0.20 M 500 500

0.040 M 0.12 M

TIP = [Pb2+][Cl-]2

TIP = [0.040][0.12] 2

= 5.8 x 10-4

Ksp = 1.2 x 10-5 TIP > Ksp ppt forms

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5. Changing the Solubility of a Salt

E +Ca(OH)2(s)⇄ Ca2+ + 2OH-

Substance Added Effect on Molar Solubility Effect on Ksp

Ca(NO3)2Decrease none

Na2SO4Increase none

NaOHDecrease none

HCl Increase none

NaCl none none

Ca(OH)2none none

Increase Temperature Increase Increase

Decrease TemperatureDecrease Decrease

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6. Mg(OH)2 will have the greatest solubility in:

Mg(OH)2(s) ⇌ Mg2+ + 2OH-

A. NaOH OH- lowers solubility

B. Mg(NO3)2 Mg2+ lowers solubility

C. H2O No effect solubility

D. AgNO3Ag+ increases solubility by reacting with OH-

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7. Calculate the maximum number of grams BaCl2 that will dissolve in 0.50 L of 0.20 M AgNO3 solution.

AgCl(s)⇄ Ag+ + Cl-

0.20 M

Ksp = [Ag+][Cl-]

1.8 x 10-10 = [0.20][Cl-]

[Cl-] = 9.0 x 10-10 M

BaCl2(s)⇄ Ba2+ + 2Cl-

4.5 x 10-10 M9.0 x 10-10 M

0.50 L x 4.5 x 10-10mole x 208.3 g = 4.7 x 10-8 g

1 L mole

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8. Ionic Solutions:NaCl HCl NH4NO3

Molecular Solutions:C12H22O11

9. What is the answer?

A. NaCl

B. CaCl2

C. AgCl

D. AgBr

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10. Ionic Solutions: NaCl HCl NH4NO3

Molecular Solutions: C12H22O11

11. What is the answer?

A. NaCl High

B. CaCl2 High

C. AgCl Low 1.8 x 10-12

D. AgBrLow 5.4 x 10-13

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