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Solubility Review

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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Solubility Review

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  1. Solubility Review

  2. 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

  3. 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)

  4. 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)

  5. 3. PbCl2(s)⇌ Pb2+ + 2Cl- Ksp = 4s3

  6. 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

  7. 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

  8. 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-

  9. 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

  10. 8. Ionic Solutions:NaCl HCl NH4NO3 Molecular Solutions:C12H22O11 9. What is the answer? A. NaCl B. CaCl2 C. AgCl D. AgBr

  11. 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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