Chemistry Study Guide
Chapter 13 - Water and the Properties of Liquids
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1. Define each of the following:
        a) sublimation
        b) vapor pressure
        c) basic anhydride
        d) acid anhydride
        e) boiling point
        f) melting point
        g) hydrate
        h) efflorescence
        i) evaporation
        j) deliquescence
        k) normal boiling point
        l) hygroscopic
        m) heat of fusion
        n) heat of vaporization

2. What is the specific heat of water?

3. What can cause the boiling point of a liquid to decrease? To increase?

4. Which molecules leave the system first in an evaporating liquid substance?

5. How does the freezing point of a substance compare to its melting point?

6. What causes the unusually high heat of vaporization of water?

7. What phase(s) does water exist in at 100EC and 1.00 atm pressure?

8. What does the boiling point of pure water depend on?

9. Under what conditions is the effect of hydrogen bonding the greatest?

10. What properties of water are affected by hydrogen bonding?

11. If you have one substance that boils at 95EC and another substance that boils at 75EC, which one would have the higher vapor pressure at their respective boiling points?

12. If given several samples of water at different temperatures, how could you tell which sample would have the highest vapor pressure?

13. Determine the anhydride of each of the following:
                HNO3                Fe(OH)2

14. What do solids that undergo sublimation have in common?

15. What will happen to the boiling point of water as atomospheric pressure decreases?

16. What will happen to the boiling point of water as the pressure above it increases?

17. What will happen to the vapor pressure of a substance as its temperature increases?

18. At what temperature can a liquid evaporate?

19. Name some substances that undergo sublimation.

20. What happens to a substance as it goes through the process of distillation?

21. Look at the graph on page 306, and determine the normal boiling point of each of the substances.

22. What is the percent of water by mass in SnCl2 @ 2 H2O?

23. How many joules of energy must be removed to change 87 g of water at 23EC to ice at 0EC? (Heat of crystallization of ice is 335 J/g.)

24. The heat of fusion of ice is 335 J/g. What is the number of joules required to melt 489 grams of ice at 0EC?

25. How many joules of energy are required to change 92.0 g of water at 37.0EC to steam at 100EC? (The heat of vaporization of water is 2.26 x 103 J/g.)

26. Draw a heating curve for a substance being heated while changing from the solid state to the gaseous state, and explain what is happening in each part of the curve.