Chapter 16 Solutions Review
1. The salt that is dissolved in water to make a solution is called the
2. The properties of a solution include all of the following except that
a. it is a homogeneous mixture if it has been well stirred.
b. dissolved particles will settle out upon standing.
c. it is clear and transparent with particles too small to be seen.
d. dissolved particles will pass through a piece of filter paper.
3. A drinking glass full of cold water is left standing on the table. After a few minutes bubbles appear in the water. This observation supports the generalization that
a. water is a polar solvent.
b. gases are attracted to glass.
c. water can be made to boil at any temperature.
d. gases are more soluble in cold water than in warm water.
4. The most common types of solutions are
a. gaseous solutions.
c. solid solutions.
5. The number of moles of chloride ions in 1 dm3 of 1.0 M solution of aluminum chloride, AlCl3, is
6. When substances are dissolved in water the effect is to
a. raise the boiling point and lower the freezing point of water.
b. raise both the boiling point and freezing point of water.
c. lower both the boiling point and freezing point of water.
d. lower the boiling point and raise the freezing point of water.
7. The amount of a substance that dissolves in another substance is affected by all of the following except
a. the nature of the substances.
b. the temperature.
c. the pressure.
8. An increase in temperature increases both the rate of dissolving and the amount that dissolves for most
a. solid solutes.
b. liquid solutes.
c. gaseous solutes.
d. all of the above.
9. A 1.0 molar solution of sucrose in water is prepared and divided intow two equal volumes, A and B. More sucrose is added to volume A and more water is added to volume B. Which of the folling statements is correct?
a. A is more concentrated than B.
d. A is more dilute than B.
c. A is less saturated than B.
d. A and B have the same molarity.
10. The process of dissolving a solid in a liquid incvolves separating particles in the solid from one another. As a result you would expect this process to be
12. The rate of solution of a particular substance is affected by
b. the temperature.
c. the size of particles,.
d. all of the above.
13. A solution is saturated when the solute in solution is
a. no longer visible to the naked eye.
b. starting to come out of solution as a solid.
c. in equilibrium with the undissolved solute.
d. no longer coming out of solution as a solid.
14. The procedure usually used to prepare a supersaturated solution is to
a. cool a saturated solution.
b. warm a saturated solution.
c. add crystals to a saturated solution.
d. pour a saturated solution through a filter.
15. The molarity of a solution refers to the number of moles of the solute in
a. a mole of solvent.
b. a mole of solution.
c. one cubic decimeter of the solvent.
d. one cubic decimeter of the solution.
16. The number of moles of a solute in solution can be determined from the
a. product of the molar mass and the molarity.
b. quotient of the molarity divided by the volume.
c. quotient of the volume divided by the molarity.
d. product of the volume and the molarity.
17. A homogeneous mixture should have
a. more than two substances present.
b. only two substances present.
c. the same properties throughout.
d. a separation of the mixture into layers.
18. To prepare a 1.0 molal solution from a 1.0 molar solution a chemis would have to
a. add more solvent.
b. add more solute.
c. heat the solution.
d. make no changes since they are equal.
19. When a gas dissolves in liquid water one would expect, since there is a phase change of the solute, that there would be an accompanying
a. temperature increase.
b. temperature decrease.
c. pressure increase.
d. pressure decrease.
21. Express the solubility of ammonium chloride (NH4Cl) per 100 g of water at 70˚C if 15.0 g of NH4Cl dissolve in 25 g of water at 70˚C.
22. What is the molarity of a solution that contains 12.0 g of sodium sulfate (Na2SO4) in 2.0 dm3 of a water solution?
23. What is the molality of a solution that is prepared by dissolving 5.0 g of potassium hydroxide (KOH) in 0.25 kg of water?
24. What is the advantage in describing the concentration of solutions in molarity rather than in number of grams of solute dissolved in 100 g of solvent?
25. The boiling point elevation depends on all of the following except the
a. nature of the solvent.
b. number of particles of the solute.
c. nature of the solvent.
d. amount of the solvent.
26. If the molal freezing point depression is -1.86°C/molal then the lowering of the freezing point in a 1 molal solution of iron(II) chloride would be closest to
a. -1.86°C x 1
b. -1.86°C x 2
c. -1.86°C x 3
d. -1.86°C x 4
27. The freezing point depression depends on the concentration of the solute particles rathe than on the kind of particles. This kind of property is called
28. Give that the molal freezing point depression constant (Kf) for water (H2O) is -1.86°C/molal, how much will the freezing point of water be lowered if 9.2 g of glycerine (C3H8O3) is added to 1.00 kg of water?
29. Given that the molal boiling point constant (Kb) for ethyl alcohol (C2H5OH) is 1.22°C/molal, what is the gram molecular mass of a nonelectrolyte if 50.0 g of the substance in 1.0 kg of ethyl alcohol raises the boiling temperature by 0.61°C?
30. What is the effect on the cooking times for vegetables if salt is added before boiling them? Explain your answer.
|If you have any questions, please email Ms. Cummings|