Solubility Workbook
Period Worksheets Quiz
· 1. Solubility and Saturated Solutions. WS 1 1
· 2. Ion Concentration Calculations and Ionic Equations. WS 2-3 2
· 3. Solubility to Ksp. WS 4 3
· 4. Ksp to Solubilty and Size of Ksp. WS 5 4
· 5. Trial Ksp. WS 6 5
· 6. Separating Ions WS 7 6
· 7. Common Ion Effect and WS 8 7
· 8. Titrations and Max Ion Concentration WS 9 8
· 9. Review Web Review Practice Test 1
· 10. Review Practice Test 2
· 11. Test
The following workbook is designed to ensure that you can demonstrate your understanding of all aspects of the solubility unit. Ask yourself, “do I want to do well in this class?” If you are determined to be successful the minimum expectation that you should have for yourself is that you do all of these questions by the due dates given by your teacher. There are other things that you should do to prepare for the test at the end of the unit. Remember, what you put into this course is what you will get out. There is no substitute for consistent effort and hard work. If you can’t do a question, get some help before the end of the unit, you need to know, understand, and remember everything. Good luck! I know you can do well in this unit. Keep up the great work!
Worksheet # 1 Solubility and Saturated Solutions
1. Define and give units for solubility.
2. Describe the relationship between the rate of dissolving and the rate of crystallization when a small amount of solute is added to an unsaturated solution.
3. Describe the relationship between the rate of dissolving and the rate of crystallization when a small amount of solute is added to a saturated solution.
4. Describe the relationship between the rate of dissolving and the rate of crystallization when a small amount of solute is added to a supersaturated solution.
5. Which of the above solutions would need to be prepared in order to determine the solubility of an ionic solution.
6. 2.65 g of Ba(OH)2 is dissolved in 70.0 mL of water to produce a saturated solution at 20 oC. Calculate the solubility in units of g/100 mL; g/L ; and M.
7. A beaker containing 100.0 mL of saturated BaCO3 solution weighs 159.60 g. The beaker is evaporated to dryness and weighs 56.36 g. The empty beaker weighs 24.33 g. Calculate the solubility in units of g/100 mL; g/ L; and M.
8. Write dissociation equations to represent the equilibrium present for a saturated solution of each ionic compound. Write the solubility product (Ksp expression) for each of the equilibrium systems. The first one is done.
a) Al2(SO4)3 ⇄ 2Al3+ + SO42- Ksp = [Al3+]2 [SO42-]3
b) FeCO3
c) Co2(SO4)3
d) Na3PO4
9. Write formula, complete ionic, and net ionic equations for each.
a) H2SO4(aq) + 2NaOH(aq) → Na2SO4 + 2HOH(l)
2H+ + SO42- + 2Na+ + 2OH- → 2Na+ + SO42- + 2HOH(l)
H+ + OH- → HOH(l)
b) Mg(NO3)2(aq) + Na2CO3(aq) →
c) Al(NO3)3(aq) + (NH4)3PO4(aq) →
d) H3PO4(aq) + Ca(OH)2(aq) →
Worksheet # 2 Solubility
1. What is the concentration of each ion in a 10.5 M sodium silicate solution?
2. What is the concentration of each ion in the solution formed when 94.5 g of
nickel (III) sulphate is dissolved into 850.0 mL of water?
3. If 3.78 L of 0.960 M sodium fluoride solution is added to 6.36 L of 0.550 M calcium nitrate solution, what is the resulting concentration of [Ca+2] and [F-]?
4. What is the concentration of each ion in the solution formed when 94.78 g of
iron (III) sulphate is dissolved into 550.0 mL of water?
5. If the [F-] = 0.200 M, calculate the number of grams AlF3 that would be dissolved in 2.00 L of water.
6. If the [SO42-] = 0.200 M in 2.0 L of Al2(SO4)3, determine the [Al3+] and the molarity of the solution.
Dissociation Equations Write dissociation equations for any chemicals, which dissociate when dissolved in water:
1. HCl (aq) → H+ + Cl- ionic compounds dissociate
2. C6H12O6(S) → C6H12O6(aq) molecular compounds do not dissociate
3. Na2S (s)
4. Al(CH3COO)3 (s)
5. MgBr2 (s)
6. Na2CO3 (s)
7. C12H22O11 (s)
8. K3PO4 (s)
9. CH3OH (l)
Net Ionic Equations
Write chemical equations, total ionic equations and net ionic equations for each reaction. The first one is done for you. (assume that all reactions occur):
1. Magnesium metal is placed in hydrochloric acid
Mg (s) + 2 HCl (aq) → MgCl2 (aq) + H2 (g)
Mg (s) + 2 H+ (aq) + 2 Cl- (aq) → Mg2+ (aq) + 2Cl- (aq) + H2 (g)
Mg (s) + 2 H+ (aq) → Mg2+ (aq) + H2 (g)
2. Zinc metal is placed in silver nitrate solution
3. Barium chloride solution is added to lead (II) nitrate solution.
4. Sulphuric acid is added to strontium hydroxide solution.
5. Sodium carbonate solution is added to nickel (III) nitrate solution.
6. Aqueous chlorine is added to sodium bromide solution.
7. Nitric acid is added to strontium hydroxide solution.
Worksheet # 3 Solubility
1. Classify each as an ionic or molecular (covalent) solution.
NaCl (aq) ______NH3 (aq) ______
CoCl2 (aq) ______AgCl (aq) ______
CH3OH (aq) ______HCl (aq) ______
NH4OH (aq) ______I2 (aq) ______
2. Define each:
a) unsaturated solution:
b) saturated solution:
c) solubility:
3. Describe how you would prepare a saturated solution.
4. Describe how you would determine the solubility of NaCl in water at 20oC.
5. In terms of equilibrium describe the difference between a saturated and unsaturated solution.
6. What is the effect of temperature on solubility?
7. 200.0 g of CoCl2 is dissolved in 500.0 mL of water at 0oC to form a saturated solution. What is the solubility of CoCl2 at 0oC in three different units?
8. In a saturated solution of CaCl2, a small amount of solid is present. Write a net ionic equation showing the equilibrium reaction. Write the solubility product (Ksp expression)
9. If you were given a saturated, unsaturated and supersaturated solution, how would you distinguish one from another?
a) Unsaturated solution:
b) Saturated solution:
c) Supersaturated solution:
10. Write the equilibrium equation and solubility product Ksp for each salt. The first one is done.
a) Ca(OH)2 (s) → Ca2+ + 2OH- Ksp = [Ca2+] [OH-]2
b) AgCl (s)
c) Na3PO4 (s)
d) (NH4)3PO4 (s)
e) Cu2SO4 (s)
f) Al(CH3COO)3 (s)
g) Ca3(PO4)2 (s)
Worksheet # 4 Solubility to Ksp
The Ksp is a measure of the solubility of an ionic salt. The larger the value of the Ksp, the greater is the solubility of the salt. You can only calculate a Ksp if the solution is saturated. Only saturated salt solutions are in equilibrium. You can calculate the Ksp from the solubility of a salt, since the solubility represents the concentration required to saturate a solution.
1. Calculate the Ksp for CaCl2 if 200.0g of CaCl2 is required to saturate 100.0 mL of solution.
2. Calculate the Ksp for AlCl3 if 100.0g is required to saturate 150.0 mL of a solution.
3. The solubility of SrF2 is 2.83 x 10-5 M. Calculate the Ksp.
4. The solubility of GaBr3 is 15.8 g per 100.0 mL. Calculate the Ksp.
5. The solubility of Ag2SO4 is 1.33 x 10-7g per 100.0 mL. Calculate the Ksp.
6. If 2.9 x 10-3 g of Ca(OH)2 is needed to saturate 250.0 mL of solution, what is the Ksp?
7. At a certain temperature, a 40.00 mL sample of a saturated solution of barium hydroxide, is neutralized by 29.10 mL of 0.300 M HCl. Calculate the Ksp of Ba(OH)2.
Calculate the concentrations of all ions in each solution.
8. 0.50 M Al2(SO4)3(aq)
9. 25.7 g (NH4)3PO4(aq) in 250.0mL H2O.
10. 210. g CoCl2 • 6H2O in 800.0 mL H2O.
Worksheet # 5 Ksp to Solubility
Calculate the solubility in M and g/L for each. Use the Ksp values found in your chart.
1. BaCO3
2. Fe(OH)2
3. PbCl2
4. How many grams of Mg(OH)2 are required to completely saturate 1.5 L of solution?
Review
1. If 200.0 g of MgCl2 is required to saturate 1.5 L of solution at 20 oC, calculate the Ksp.
2. If the Ksp for Al2O3 is 2.8 x 10-8, calculate [Al3+] and [O-2] in mol/L.
Worksheet # 6 Trial Ksp
1. Will a precipitate form if 200.0 mL 0.00020M Ca(NO3)2 is mixed 300.0 mL of 0.00030M Na2C03?
2. Will a precipitate form if 25.0 mL of .0020M Pb(NO3)2 is mixed with 25.0 mL of 0.040M NaBr.
3. Will a precipitate form if equal volumes of 0.00020M Ca(NO3)2 is mixed with 0.00030M Na2C03?
4. Co(OH)2 Solubility = 3.0 x 10-3 g/L Calculate the Ksp at 250 C.
5. Ag2C2O4 Solubility = 8.3 x 10-4 M Ksp=?
6. SrF2 Calculate the solubility in (M).
7. Cu(IO3)2 Solubility Calculate the solubility in (g/L).
Worksheet # 7 Separation Positive Ions: Work from top to bottom of solubility chart!!
1. Ag+ Mg2+ Ba2+
i) Add: Filter Out: Net Ionic equation:
ii) Add: Filter Out: Net Ionic equation:
iii) Add: Filter Out: Net Ionic equation:
2. Pb2+ Ba2+ Sr2+
i) Add: Filter Out: Net Ionic equation:
ii) Add: Filter Out: Net Ionic equation:
iii) Add: Filter Out: Net Ionic equation:
3. Cu+ Ca2+ Sr2+
i) Add: Filter Out: Net Ionic equation:
ii) Add: Filter Out: Net Ionic equation:
iii) Add: Filter Out: Net Ionic equation:
4. Be2+ Sr2+ Ag+
i) Add: Filter Out: Net Ionic equation:
ii) Add: Filter Out: Net Ionic equation:
iii) Add: Filter Out: Net Ionic equation:
5. Be2+ Ca2+ Pb2+
i) Add: Filter Out: Net Ionic equation:
ii) Add: Filter Out: Net Ionic equation:
iii) Add: Filter Out: Net Ionic equation:
6. Calculate the Ksp for CaCl2, if 50.0 g is required to saturate 25.0 mL of water.
7. Calculate the molar solubility of Mg(OH)2.
8. Will a precipitate form if equal volumes of 0.00020 M Na2CO3 is mixed with
0.00020 M MgCl2.
9. Write the formula, complete, and net ionic equation.
Formula Equation: CaCl2(aq) + AgNO3(aq) →
Complete Ionic:
Net Ionic:
Separation of Negative Ions: Work from bottom to top of solubility chart!!
1. SO32- OH- I-
i) Add: Filter Out: Net Ionic equation:
ii) Add: Filter Out: Net Ionic equation:
iii) Add: Filter Out: Net Ionic equation:
2. CO32- OH-
i) Add: Filter Out: Net Ionic equation:
ii) Add: Filter Out: Net Ionic equation:
3. Br- S2- PO43-
i) Add: Filter Out: Net Ionic equation:
ii) Add: Filter Out: Net Ionic equation:
iii) Add: Filter Out: Net Ionic equation:
4. PO43- OH- S2-
i) Add: Filter Out: Net Ionic equation:
ii) Add: Filter Out: Net Ionic equation:
iii) Add: Filter Out: Net Ionic equation:
5. OH- S2- SO42-
i) Add: Filter Out: Net Ionic equation:
ii) Add: Filter Out: Net Ionic equation:
iii) Add: Filter Out: Net Ionic equation:
6. S2- SO42- Cl-
i) Add: Filter Out: Net Ionic equation: ii) Add: Filter Out: Net Ionic equation:
iii) Add: Filter Out: Net Ionic equation:
Common Ion Effect Worksheet # 8
Consider the following equilibrium system. PbCl2(s) ⇄ Pb2+(aq) + 2 Cl-(aq)
Describe what happens to the solubility of PbCl2 after each of the changes.
Solubility
1. PbCl2(s) is added
2. Pb(NO3)2 is added
3. NaCl is added
4. H2O is added
5. AgNO3 is added
6. NaBr is added
Consider the following equilibrium system. AgBr(s) ⇄ Ag+(aq) + Br-(aq)
Describe what happens to the solubility of AgBr after each of the changes are made.
Solubilty
7. AgBr(s) is added
8. Pb(NO3)2 is added
9. NaCl is added
10. H2O is added
11. AgNO3 is added
12. NaBr is added
13. Explain why more Zn(OH)2 dissolves when 3 M HCl is added to a saturated solution of Zn(OH)2. Start by writing the correct equilibrium equation.
14. In an experiment, 0.1 M AgNO3 is added to 0.1 M NaCl, resulting in the formation of a white precipitate. When 0.1 M NaI is added to this mixture, the white precipitate dissolves and a yellow precipitate forms.
The formula for the white precipitate is
The formula for the yellow precipitate is
The net ionic equation for the first equilibrium is
The net ionic equation for the formation of the yellow precipitate is
Explain why the white precipitate dissolves. Start by writing the equilibrium equation for the white precipitate, then, explain how adding NaI affects this equilibrium.
Titrations and Maximum Ion Concentration Worksheet # 9
1. In a titration 25.0 ml of a 0.250 M AgNO3 solution was used to precipitate out all of the Br- in a 200.0 ml sample. Calculate [Br-].
2. In a titration 26.5ml of 0.100M Pb(NO3)2 was used to precipitate out all of the Cl- in a 30.0 ml sample of water. Calculate [Cl-].
Maximum Ion Concentration
3. Calculate the maximum concentration of OH- that can exist in a 0.200M Mg(N03)2 solution.
4. Calculate the maximum concentration of CO3-2 that can exist in a 0.500M AgNO3 solution.
5. Calculate the maximum concentration of IO3- that can exist in a 0.200M Cu(N03)2 solution.
6. Calculate the maximum concentration of Ca2+ that can exist in a 0.200 M Na2C03 solution.
7. Calculate the minimum number of moles of Pb(NO3)2 required to start precipitation in 50.0 mL of 0.15 M ZnCl2.
8. In a titration 12.5 mL of 2.00 x 10-5 M HCl is required to neutralize 250.0 mL of saturated AgOH solution. Calculate the [OH-] and then determine the Ksp for AgOH.