1. Solution Chemistry (Chp. 7)

2. Solutions Terms 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
soluble
insoluble
limiting reagent
excess reagent
actual yield
theoretical yield
decanting
pipetting
filtrate
precipitate
dynamic equilibrium

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 solution - is a homogeneous mixture
solute - the substance that dissolves OR the substance in lesser quantity
solvent - the substance which dissolves the solute OR the substance in greater quantity
concentrated - a large amount of solute relative to the amount of solvent
dilute - a small amount of solute relative to the amount of solvent

6. Terms
saturated – contains the maximum amount of dissolved solute at a given temperature and pressure
unsaturated – contains less than the maximum amount of dissolved solute at a given temperature and pressure
supersaturated – contains more than the maximum amount of dissolved solute for a given temperature and pressure

7. Terms miscible – liquids that dissolve in each other
immiscible – liquids that do not dissolve in each other
aqueous - the solvent is water
alloy - a solid solution of two or more metals

8. Terms
Solubility - the maximum amount of solute that can be dissolved under specific temperature and pressure conditions
eg. the solubility of HCl at 25 °C is 12.4 mol/L
eg mL of water at 25°C dissolves 36.2 g of sodium chloride

9. Terms soluble – solubility is greater than 1 g per 100 mL of solvent.
insoluble - solubility is less than 0.1 g per 100 mL of solvent.

10. 9 Types of Solution

11. 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

12. 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.

13. Solubility
small molecules are often more soluble than larger molecules.
solubility of solids increases with temperature.
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.

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

15. “Like Dissolves Like”
ionic solutes and polar covalent solutes both dissolve in polar solvents
non-polar solutes dissolve in non-polar solvents.
compounds with very strong ionic bonds, such as AgCl, tend to be less soluble in water than compounds with weak ionic bonds, such as NaCl.

16. Applications
1. An opened soft drink goes ‘flat’ faster if not refrigerated.
2. Thermal pollution (warming lake water) is not 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.

17. 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.

18. Molar Concentration
The terms concentrated and dilute are qualitative descriptions of solubility.
A quantitative measure of solubility uses numbers to describe how much solute is dissolved or the concentration of a solution.

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

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

22. eg. Calculate the molar concentration of:
4.65 mol of NaOH is dissolved to prepare 2.83 L of solution.
(1.64 mol/L)
15.50 g of NaOH is dissolved to prepare 475 mL of solution.
( mol → mol/L)
p # 19

23. eg. Calculate the following:
Rearranged
Formulas
eg. Calculate the following:
the number of moles in 4.68 L of mol/L KCl solution. (0.468 mol)
the mass of KCl in 268 mL of 2.50 mol/L KCl solution. (0.670 mol → g)
p #’s

24. 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.

25. 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

26. 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.

27. p #’s 25 – 27
p #’s 1, 2, 4, & 5
DON’T SHOW UP UNLESS
THIS IS DONE!!

28. Solution Preparation & Dilution
standard solution – a solution of known concentration
volumetric flask – a flat-bottomed glass vessel that is 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

29. 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

30. 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.

31. 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

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

33. p #’s 5 – 9
DSUUTID!!

34. p #’s 10 – 13
DSUUTID!!

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

37. 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

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

39. 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!!

40. Solution Stoichiometry
1. Write a balanced equation
2. Calculate moles given
n=m/M OR n=CV
3. Mole ratios
4. Calculate required quantity

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

42. Sample Problems
1. What mass of copper metal is needed to react with mL of mol/L silver nitrate solution?
2. Calculate the volume of 2.00 M HCl(aq) needed to neutralize 1.20 g of dissolved NaOH.
3. What volume of 3.00 mol/L HNO3(aq) is needed to neutralize mL of mol/L Sr(OH)2(aq)?

43. Sample Problem Solutions
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

44. Sample Problem Solutions
HCl(aq) + NaOH(aq) → NaCl(aq) + H2O(l)
Step 2 n = mol NaOH
Step 3 n = mol HCl
Step 4 V = L HCl

45. Sample Problem Solutions
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 = mol/L HNO3

46. 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)
Ca(NO3)2(s) → Ca2+(aq) NO3-(aq)

47. 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.

48. The Solution Process (p. 299)
Acids are also electrolytes.
Acids form ions when dissolved in water.
eg. H2SO4(aq) → 2 H+(aq) + SO42-(aq)
HCl(s) → H+(aq) + Cl-(aq)

49. The Solution Process (p. 299)
Molecular Compounds DO NOT dissociate in water.
eg. C12H22O11(s) → C12H22O11(aq)
Because they DO NOT conduct electric current in solution, molecular compounds are non-electrolytes.

50. 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

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