Unit 8 – Solutions and Solubility Test, Version A
1. Which of the following Lewis structures best represents the geometry of a water molecule?
B.
C.
D.
A.
2. Unlike most other substances, water becomes denser when it melts because
A. water molecules increase in mass when ice melts to water.
B. water molecules in ice are in a random arrangement that changes to a tight geometric arrangement when ice
melts.
C. the arrangement of water molecules in water is more ordered than the arrangement of water molecules in ice
is.
D. water molecules in ice are arranged in an open pattern that collapses when ice melts.
3. Why doesn’t water in lakes and ponds of temperate climates freeze solid during the winter and kill nearly all
the living things it contains?
A. water has a cooling effect
B. ice floats and insulates the water underneath
C. the air above the water keeps it warm
D. salt water contains too much salt to allow freezing
4. Crystals of ammonium chloride, NH4Cl, seem to disappear when mixed with water. The resulting clear liquid
containing ammonium chloride and water is a
A. heterogeneous mixture.
B. compound.
C. homogeneous mixture.
D. new substance.
5. Mixtures that exhibit the Tyndall effect are
A. alloys.
B. solutions.
C. colloids.
D. homogeneous mixtures.
6. Saltwater is an electrolyte because it contains
A. suspended particles
B. no solvent.
C. water molecules.
D. dissociated ions.
7. Substances that are electrolytes
A. always conduct an electric current when dissolved in water
B. are always composed of molecules.
C. always form neutral particles when dissolved in water.
D.. are always composed of salts.
8. Which of the following substances is an electrolyte?
A. sugar
B. potassium chloride, KCl
C. water
D. salad oil
9. Crushing a solid substance increases the rate at which the substance dissolves because crushing
A. causes the particles of the substance to become disarranged.
B. increases the surface area of solute that is exposed to solvent.
C. decreases the concentration of the substance.
D. increases the kinetic energy of the particles of the solute.
10. Stirring or shaking a mixture of solid solute and solvent increases the rate of dissolving by
A. increasing the kinetic energy within the mixture.
B. increasing the surface area of the undissolved solute to the solvent.
C. allowing air bubbles to move the solvent more vigorously.
D. constantly bringing fresh solvent into contact with undissolved solute.
11. Which of these is true about alloys?
A. alloys are homogeneous mixtures of two or more metals that combine their properties
B. alloys are polar compounds of metals that demonstrate the “like dissolves like” property
C. alloys produce the Tyndall effect when mixed with water and lit with a flashlight
D. alloys are usually more expensive and more precious than the individual metals
12. Consider the possibility of each of the following substances dissolving in water. Which of these substances
best demonstrates the principle "like dissolves like"?
A. potassium bromide
B. sulfur
C. olive oil
D. oxygen gas
13. As temperature increases, the solubility of gases
A. increases.
B. decreases.
C. stays the same.
D. is not affected.
14. A dilute solution is a solution that
A. contains a small amount of dissolved solute.
B. contains a small amount of dissolved solvent.
C. is concentrated.
D. is saturated.
15. A certain solution contains 38.75 g of nickel (II) iodide, NiI2, in 1.50 L of solution. What is the molarity of
the solution?
A. 25.8 M
B. 0.0827 M
C. 0.124 M
D. 0.0888 M
16. Jonathan is reading the solubility chart and finds that KNO3 is soluble. What symbol would he use in his
chemical equation to show this?
A. (s)
B. (l)
C. (aq)
D. (g)
17. What mass of NaOH is dissolved in 25.00 mL of a 4.500 M solution of NaOH?
A. 4.444 g NaOH
B. 0.1125 g NaOH
C. 0.2222 g NaOH
D. 4.500 g NaOH
18. If you were making a 0.500M solution of hydrochloric acid in a 3.00L bottle, how many liters of 6.00M HCl
would need to be added?
A. 0.300L
B. 0.25L
C. 1.00L
D. 6.00L
19. If 80 mL of an 8.0M acetic acid solution was diluted into a 1.00L container, what would the new
concentration be?
A. 640 M
B. 10.0 M
C. 0.64 M
D. 0.001 M
20. Which properties below are correctly matched?
A. solids are more soluble in liquids at lower pressures and lower temperatures
B. solids are more soluble in liquids at higher pressures and lower temperatures
C. gases are more soluble in liquids at higher pressures and lower temperatures
D. gases are more soluble in liquids at lower pressures and higher temperatures
21. What is the formula for Copper (II) Chloride?
A. CuCl
B. CuCl2
C. Cu2Cl
22. How many grams are present in 56 moles of copper (II) fluoride? (express your
A. 5684 g
B. 5700g
C. 57g
D. 56g
23. According to VSEPR theory the shape of NH3 is _____________________
A. Linear
B. Pyramidal
C. Tetrahedral
D. Triangular planer
24. According to the solubility curves, a
temperature change of 30OC to 90 oC has the
least effect on the solubility curve of
a. KNO3
b. HCl
c. NaCl
d. NaNO3
25. Which saturated solution has the most
amount of solute dissolved in solution?
a. KNO3 at 70oC
b. KI at 0 oC
c. NH3 at 100 oC
d. NaNO3 at 80 oC
26. While writing electron configuration we must fill the lower energy orbitals before filling higher energy
orbitals is the rule given by
A. Hund
B. Pauli
C. Aufbau
27. Which of the following element is most electronegative: F, Cl, Na, Mg?
A. F
B. Cl
C. Mg
D. Na
28. Which of the following is the correct name for the compound Fe2O3?
A. Iron Oxide
B. Iron (II) Oxide
C. Iron (III) oxide
29. Using a periodic table, predict which period has the largest radius?
A. 1
B. 3
C. 6
D. 7
30. What is the percentage by mass of Na in a formula unit of NaHCO3
A. 44.2%
B. 37.7%
C. 27.4%
D. 16.7%
31. Which of the following salt is soluble?
A. BaSO4
B. CaCO3
C. Fe (OH) 2
D. K3PO4
32. Water molecules cling with each other because of the following property of water
A. Cohesion
B. Adhesion
C. Surface tension
D. High specific heat capacity
E. Capillary action
33. Water molecules stick with the walls of the container because of the following property of water
A. Cohesion
B. Adhesion
C. Surface tension
D. High specific heat capacity
E. Capillary action
34. Water rises up the in the shoots when the roots are watered because of the following property of water
A. Cohesion
B. Adhesion
C. Surface tension
D. High specific heat capacity
E. Capillary action
35. Big cruise ships travel on water because of the following property of water
A. Cohesion
B. Adhesion
C. Surface tension
D. High specific heat capacity
E. Capillary action
36. On a hot summer day when everything else is hot but water is still cold, is because of the following property
of water
A. Cohesion
B. Adhesion
C. Surface tension
D. High specific heat capacity
E. Capillary action
37. When two liquids completely mix with each other, they are called
A. Immiscible
B. Miscible
C. Dilute
D. Concentrated
38. A Solution which can dissolve extra solute with an increase in temperature is called a________________
solution
A. Saturated
B. Unsaturated
C. Supersaturated
39. Which of the following property is intensive
A. Mass
B. Density
C. Volume
D. Heat
40. Water is a universal solvent because it is
A. Linear
B. Polar
C. Non Polar
D. Has a bond angle of 120.
Name
Period
Unit 11 – Solutions and Solubility Test