Name: ______Date: ______Period: ______

Chapter 13: Water and Its Solutions Study Guide

Match the following properties to the description:

A.  Surface Tension

B.  Freezing point

C.  Boiling point

D.  Specific Heat

E.  Density

AB. Capillary Action

BC. Polar

1.  ______The energy required to raise the temperature of 1 gram of a substance 1 °C

2.  ______The temperature at which a substances freezes

3.  ______The temperature at which a substances boils

4.  ______The net force acting on the molecules on the surface of some liquids due to the cohesive forces of the molecules

5.  ______The amount of mass per unit of volume

6.  ______When a molecule has an uneven distribution of charge (one end is positive and the other is negative)

7.  ______The occurs when a liquid travels up a tube

8.  Describe 3 unique properties of water. You may use your labs to help support your examples

True or False. Place a T or F next to the following statements. Correct any false statements

9.  Water is the most common solvent among liquid solutions. ______

10. In a supersaturated solution, one way to make it saturated is by adding more solute. ______

11. A solution is made up of a solvent and solute. ______

12. In sugar water, sugar is the solvent. ______

13. The meniscus is a test tube of water is caused by surface tension. ______

14. Describe why oil and water don’t mix.

15. Describe how to make kool-aide using the words saturated, solute, solvent.

16. When we did the Solubility of a Salt lab (each group had one test tube), you heated the test tube to dissolve the solute. You removed it from the heat and waited for crystals to form. Why did crystals form?

Factors Affecting Rate of Solubility

Describe how the rate of solution formation is affected by each of the following:

17. Stirring

18. Particle size

19. Temperature

Solubility Curves

20. How many grams of solute are required to saturate 100 g of water in each of the following solutions?

a.  KCl at 80ºC

b.  KClO3 at 90ºC

c.  NaNO3 at 10ºC

d.  SO2 at 20 ºC

e.  NH4Cl at 70ºC

21. What is each of the solutions below: saturated, unsaturated or supersaturated? All of the solutes are mixed with 100 g of water.

a.  40 g of NaCl at 50ºC

b.  30 g of NH3 at 30ºC

c.  70 g of HCl at 20ºC

d.  80 g of KNO3 at 60ºC

e.  80 g of NH4Cl at 80ºC

22. If 50.0 g of NaCl is mixed with 100.0 g of water at 80.0oC, how much will not dissolve?

23. If a saturated solution of KCl at 90.0oC is cooled to 30.0oC, how much of the solid will precipitate?

24. What is the minimum temperature needed to dissolve 90.0 g of KNO3 in 100.0 g of water?

25. Which solute is least affected by the temperature changes?

26. Which three solutes show a decrease in solubility with increasing temperature?

27. How does the solubility of all “ionic solids” change with an increase in temperature? Explain.

28. You made two graphs for solubility in this unit. Make sure you can do it again on the test.

Molarity

29. Write the formula for Molarity.

30. What is the molarity of a solution containing 58.5 g NaCl in 4.00 L of solution?

31. How many moles of dextrose are dissolved in 0.333 L of a 0.300 M solution?

32. How many grams of NaCl are needed to make 1.50 L of a 0.200 M solution?

Complete all missing information:

Solute formula / Molar Mass / Solute mass / Moles of solute / Solution volume / Molarity
KClO3 / 122.5 g / ? / 1.0M
NH4Br / ? / 2.0 L / 0.50M
HNO3 / 20.0 g / .500 L / ?
HCl / ? / .750 L / 0.044M
(NH4)2SO4 / 44.2 g / .600 L / ?