Name _____________Hr____
CH 15 REVIEW
solute immiscible suspension Henry’s law
solvent solvation saturated colloid
soluble dissociation supersaturated Tyndall effect
1. List the factors that affect how much solute will dissolve.
2. What factors influence the rate (how fast) a solute dissolves?
3. What is the key difference between solutions, colloids, and suspensions. Give an example of each.
4. Explain why baby oil does not wash off your hands with just water.
5. Do all “saturated” solutions contain the same amount of solute?
6. An increase in temp does what to solubility : _______ for solid solutes, ________ for gases
An increase in pressure does what to solubility: ______ for solids, _________ for gases
7. Explain why a solution has a lower vapor pressure than its pure solvent.
8. Explain why boiling point is raised and freezing point lowered by the addition of a solute.
Solubility Problems (use the chart on p 457 or the graph on p 458)
9. What mass of Al2(SO4)3 will dissolve in 100g of H2O at 60oC? How much dissolves in 325g of water?
10. If 100 g AgNO3 were added to 50 g of H2O at 20oC, would the solution be unsaturated, saturated,
or supersaturated?
11. Using the graph p 458, estimate the solubility of KClO3 at 35o , 65o, 85o C
12. If 110 g of KCl were added to 200 g H2O, how hot would you have to heat the mixture to get all the
KCl to dissolve?
CONCENTRATION Problems %mass, % volume, Molarity, molality, dilutions
13. What is the % concentration of:
a) 75.0 g CuSO4 in 325 g H2O
b) 36.5 mL H2O2 in 100.0 mL H2O
14. 202.2 g of KNO3 is dissolved in H2O to form 1.00 L of solution. What is the Molarity?
15. In 2.00L of a 0.75 M solution of NaCl how many moles of salt are dissolved? How many grams is this?
16. A solution is prepared by dissolving 2.50 g of K2CrO4 in 23.2 g H2O. What is the molality?
17. A lab requires 500.0 mL of 2.50 M NaOH. A stock solution is available with a concentration of 6.80 M.
How many mL of the stock are required? How much water will be added to dilute it?