1. Solution Chemistry (Chp. 7)

2. Topics Definitions/properties Molar Concentration (mol/L) Dilutions
% Concentration (pp. 255 – 263)
Solution Process
Solution Preparation
Solution Stoichiometry
Dissociation

3. Terms solution solvent solute concentrated dilute aqueous miscible
Immiscible
alloy
solubility
molar solubility
saturated
unsaturated
supersaturated
dissociation
electrolyte
non-electrolyte
filtrate
precipitate
limiting reagent
excess reagent
actual yield
theoretical yield
decanting
pipetting
dynamic equilibrium x

4. Define the terms in bold and italics from pp. 237 – 240.
Solids, liquids, and gases can combine to produce 9 different types of solution. Give an example of each type.
p #’s 5, 7, 9, & 10

5. Terms alloy solution solubility solvent molar solubility solute
saturated
unsaturated
supersaturated
dynamic equilibrium
solution
solvent
solute
concentrated
dilute
aqueous
miscible
immiscible x

6. Factors Affecting Solubility (pp.243 – 254)
List 3 factors that affect the rate of dissolving.
How does each of the following affect solubility?
particle size
temperature
pressure

7. Factors Affecting Solubility
What type of solvent will dissolve:
polar solutes
nonpolar solutes
ionic solutes
Why do some ionic compounds have low solubility in water?
p. 254 #’s 1, 2, 4 - 6

8. Section 7.2 (pp. 243 – 252)
State the generalizations regarding solubility and solutions (in italics)
Define terms (in bold)
ion-dipole attractions electrolyte
hydrated non-electrolyte

9. Rate of Dissolving
for most solids, the rate of dissolving is greater at higher temperatures
stirring a mixture or by shaking the container increases the rate of dissolving.
decreasing the size of the particles increases the rate of dissolving.

10. “Like Dissolves Like”
ionic solutes and polar covalent solutes both dissolve in polar solvents
non-polar solutes dissolve in non-polar solvents.

11. Solubility
small molecules are often more soluble than larger molecules.
the solubility of most solids increases with temperature while the solubility of most liquids is not affected by temperature.
the solubility of gases decreases as temperature increases
an increase in pressure increases the solubility of a gas in a liquid.

12. Applications
1. An opened soft drink goes ‘flat’ faster if not refrigerated.
2. Warming of pond water may not be healthy for the fish living in it.
3. After pouring 5 glasses of pop from a 2 litre container, Jonny stoppered the bottle and crushed it to prevent the remaining pop from going flat.

13. Molar Concentration Review: - Find the molar mass of Ca(OH)2
- How many moles in g of Ca(OH)2?
- Find the mass of mol of Ca(OH)2.

14. Molar Concentration
The terms concentrated and dilute are qualitative descriptions of solubility.
A quantitative measure of solubility uses numbers to describe the concentration of a solution.

15. Molar Concentration
The MOLAR CONCENTRATION of a solution is the number of moles of solute (n) per litre of solution (v).

17. V Molar Concentration FORMULA: Molar Concentration = number of moles
volume in litres
C = n V

18. eg. Calculate the molar concentration of:
4.65 mol of NaOH is dissolved to prepare 2.83 L of solution.
15.50 g of NaOH is dissolved to prepare 475 mL of solution.
p # 19

19. Eg. Calculate the following:
the number of moles in 4.68 L of mol/L KCl solution.
the mass of KCl in 268 mL of 2.50 mol/L KCl solution.

20. the volume of 6. 00 mol/L HCl(aq) that can be made using 0
the volume of 6.00 mol/L HCl(aq) that can be made using mol of HCl.
the volume of 1.60 mol/L HCl(aq) that can be made using 20.0 g of HCl.
p #’s20-24

21. Dilution (p. 272) The number of moles remains the same
Number of moles before dilution
When a solution is diluted:
The concentration decreases
The volume increases
The number of moles remains the same
ni = nf
Number of moles after dilution

22. Ci Vi = Cf Vf Dilution (p. 272) ni = nf
eg. Calculate the molar concentration of a vinegar solution prepared by diluting 10.0 mL of a 17.4 mol/L solution to a final volume of 3.50 L.

23. DON’T SHOW UP UNLESS THIS IS DONE!!
p #’s 25 – 27
p #’s 1, 2, 4, & 5
DON’T SHOW UP UNLESS
THIS IS DONE!!
Homework NOT done: Brandon, Chris, Maria, Marisa, Ryan

24. Solution Preparation & Dilution
standard solution – a solution of known concentration
volumetric flask – a flat-bottomed glass vessel used to prepare a standard solution
delivery pipet – pipets that accurately measure one volume
graduated pipet – pipets that have a series of lines that can be use to measure many different volumes

25. To prepare a standard solution:
1. calculate the mass of solute needed
2. weigh out the desired mass
3. dissolve the solute in a beaker using less than the desired volume
4. transfer the solution to a volumetric flask (rinse the beaker into the flask)
5. add water until the bottom of the meniscus is at the etched line

26. To dilute a standard solution:
1. Rinse the pipet several times with deionized water.
2. Rinse the pipet twice with the standard solution.
3. Use the pipet to transfer the required volume.
4. Add enough water to bring the solution to its final volume.

27. Percent Concentration
Concentration may also be given as a %.
The amount of solute is a percentage of the total volume/mass of solution.
liquids in liquids - % v/v
solids in liquids - % m/v
solids in solids - % m/m

28. Percent Concentration
p #’s 1 – DSUUTID!!

29. p #’s 5 – 9
DSUUTID!!

30. p #’s 10 – 13
DSUUTID!!
Brandon & Chris

31. Concentration in ppm and ppb
Parts per million (ppm) and parts per billion (ppb) are used for extremely small concentrations

33. eg. 5. 00 mg of NaF is dissolved in 100. 0 kg of solution
eg mg of NaF is dissolved in kg of solution. Calculate the concentration in:
a) ppm
b) ppb

34. ppm = g x 106
100,000 g
= 0.05 ppm
ppb = g x 109
= 50.0 ppb

35. DON’T SHOW UP UNLESS THIS IS DONE!!
p #’s 15 – 17
pp. 277, 278
#’s 11, 13, 15 – 18, 20
DON’T SHOW UP UNLESS
THIS IS DONE!!

36. Solution Stoichiometry
1. Write a balanced equation
2. Calculate moles given
OR n=CV
3. Mole ratio
4. Calculate required quantity

37. Solution Stoichiometry
eg mL of a HCl(aq) solution is used to neutralize 30.0 mL of a 2.48 mol/L Ca(OH)2 solution.
Calculate the molar concentration of the HCl(aq) solution.
p. 304: #’s 16, 17, & 18
Worksheet

38. Sample Problems
What mass of copper metal is needed to react with mL of mol/L silver nitrate solution? (0.794 g Cu)
Cu(s) + 2 AgNO3(aq) → 2 Ag(s) + Cu(NO3)2(aq)
Step 2 n = mol AgNO3
Step 3 n = mol Cu
Step 4 m = g Cu

39. HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
2. Calculate the volume of 2.00 M HCl(aq) needed to neutralize 1.20 g of dissolved NaOH. ( L HCl)
HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
Step 2 n = mol NaOH
Step 3 n = mol HCl
Step 4 V = L HCl

40. 2 HNO3(aq) + Sr(OH)2(aq) → 2 H2O(l) + Sr(NO3)2(aq)
3. What volume of 3.00 mol/L HNO3(aq) is needed to neutralize mL of mol/L Sr(OH)2(aq)? ( L HNO3)
2 HNO3(aq) + Sr(OH)2(aq) → 2 H2O(l) + Sr(NO3)2(aq)
Step 2 n = mol Sr(OH)2
Step 3 n = mol HNO3
Step 4 V = L HNO3

41. The Solution Process (p. 299)
Dissociation occurs when an ionic compound breaks into ions as it dissolves in water.
A dissociation equation shows what happens to an ionic compound in water.
eg. NaCl(s) → Na+(aq) + Cl-(aq)
K2SO4(s) → 2 K+(aq) + SO42-(aq)

42. The Solution Process (p. 299)
Solutions of ionic compounds conduct electric current.
A solute that conducts an electric current in an aqueous solution is called an electrolyte.

43. The Solution Process (p. 299)
Acids are also electrolytes.
6 strong acids:
perchloric acid - HClO4(aq)
hydrochloric acid – HCl(aq)
hydroiodic acid - HI(aq)
hydrobromic acid – HBr(aq)
nitric acid – HNO3(aq)
sulfuric acid – H2SO4(aq)
eg. H2SO4(aq) → 2 H+(aq) + SO42-(aq)
HCl(s) → H+(aq) + Cl-(aq)
All other acids are weak electrolytes
(poor conductors)

44. The Solution Process (p. 299)
eg. H2SO4(aq) → 2 H+(aq) + SO42-(aq)
HCl(s) → H+(aq) + Cl-(aq)
Molecular Compounds DO NOT dissociate in water.
eg. C12H22O11(s) → C12H22O11(aq)

45. The Solution Process (p. 299)
Because they DO NOT conduct electric current in solution, molecular compounds are non-electrolytes.
Low solubility compounds are weak electrolytes due to their low solubility in water.
eg. AgBr BaSO4 PbI2

46. The Solution Process (p. 299)
The molar concentration of any dissolved ion is calculated using the ratio from the dissociation equation.
eq. What is the molar concentration of each ion in a 5.00 mol/L MgCl2(aq) solution:
5.00 mol/L
5.00 mol/L
10.00 mol/L

47. The Solution Process (p. 299)
eg. Calculate the concentration of Al(NO3)3 in a solution with a nitrate ion concentration equal to mol/L.

48. The Solution Process (p. 299)
eg. Calculate the molar concentration of chloride ions in a solution prepared by dissolving 10.0 g of FeCl3 to make mL of solution

49. The Solution Process (p. 299)
eg. Calculate the mass of Na2SO4 needed to prepare mL of solution with a sodium ion concentration equal to mol/L.

50. eg. What mass of calcium chloride is required to prepare 2. 00 L of 0
eg. What mass of calcium chloride is required to prepare 2.00 L of mol/L Cl-(aq) solution?

51. p #’s 7 – 9
What mass of calcium chloride is required to prepare 2.00 L of mol/L Cl-(aq) solution?
p # 14
p #’s 11, 12, 16, & 18