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Online Study Guide - Chem 2 - Solutions


Multiple Choice
Identify the letter of the choice that best completes the statement or answers the question.
 

 1. 
What term describes a solution in which the dissolved solute is in equilibrium with the undissolved solute?
a.
dilute solution
c.
supersaturated solution
b.
saturated solution
d.
unsaturated solution
 

 2. 
Which of the following compounds provides the most solute particles when completely dissociated in water?
a.
MgCl2
c.
NaCl
b.
KBr
d.
Na3PO3
 
 
Data related to aqueous solutions of sodium chloride (NaCl) and aqueous solutions of ethanol (C2H5OH) are provided in the table below. Use the table to answer the following questions. Choose the letter of the choice that best answers the question.

 
Mass (g)
 
Volume (mL)
Solution
NaCl
H2O
Solution
C2H5OH
H2O
1
3.0
100.0
5
2.0
100.0
2
3.0
200.0
6
5.0
100.0
3
3.0
300.0
7
9.0
100.0
4
3.0
400.0
8
15.0
100.0
 

 3. 
What is the percent by mass of NaCl in solution 1?
a.
0.030%
c.
3.0%
b.
2.9%
d.
33%
 

 4. 
Which of the following solutions is the most dilute?
a.
Solution 1
c.
Solution 3
b.
Solution 2
d.
Solution 4
 

 5. 
What is the percent by volume of C2H5OH in Solution 5?
a.
0.2%
c.
2.0%
b.
1.9%
d.
22%
 

 6. 
Which of the following solutions is the most concentrated?
a.
Solution 5
c.
Solution 7
b.
Solution 6
d.
Solution 8
 

 7. 
Increasing temperature always increases the solubility of a solute in a solvent.
a.
true
b.
false
 

 8. 
If two liquids are not soluble in each other, they are siad to be _____.
a.
soluble
c.
miscible
b.
insoluble
d.
immiscible
 

 9. 
The substance in a solution that dissolves another substance is called ___.
a.
solute
c.
electrolyte
b.
solvent
d.
nonelectrolyte
 

 10. 
Which of the following is NOT a way to increase the rate of solution?
a.
stir the solution
c.
increase the surface area
b.
decrease the surface area
d.
increase the temperature
 

 11. 
A solution is made by dissolving 17.0 g of Lithium iodide in enough water to make 500.0 mL of solution. What is the molarity of the solution?
a.
34 M
c.
0.25 M
b.
0.034 M
d.
2.54 x 10-4
 

 12. 
Calculate the molarity of a water soluiton of CaCl2  made by dissolving 612 g of CaCl2 in 5.04 L of solution.
a.
1.09 M
c.
0.775 M
b.
22.0 M
d.
1.88 M
 

 13. 
The solubility of a gas is 2.0 g/L at 50.0 KPa. How much gas will dissolve in 1.6 L at a pressure of 10.0 KPa?
a.
0.40 g
c.
0.27 g
b.
0.60 g
d.
0.99 g
 

 14. 
At a pressure of 1.0 atm the solubility of  agas is 1.72 g/L. What will the solubility of that gas be at 1.35 atm?
a.
2.32 g/L
c.
0.785 g/L
b.
1.27 g/L
d.
0.431 g/L
 

 15. 
The label on a 250.0 mL stock bottle reads 21.5% alcohol by volume. How many mL of alcohol does the bottle contain?
a.
196 mL
c.
241 mL
b.
8.60 mL
d.
54.0 mL
 

 16. 
Calculate the percent by mass of 3.55 g of NaCl dissolved in 88 g of water.
a.
4.03%
c.
15.6%
b.
3.87%
d.
21.2%
 

 17. 
How many grams of solute are in 64.3 mL of 0.0238 M KOH?
a.
0.371 g
c.
0.0859 g
b.
56.6 g
d.
0.588 g
 

 18. 
WHat is the molarity of 0.96 g of magnesium chloride in 500.0 mL of solution?
a.
0.020 M
c.
2.0 x 10-5
b.
0.032 M
d.
3.2 x 10-5
 

 19. 
How many mL of 2.55 M NaOH are needed to make 125 mL of 0.75 M NaOH?
a.
430
c.
92
b.
0.015
d.
37
 

 20. 
20.0 mL of 6.0 M HCl is diluted to 100.0 mL. What is the final molarity of the solution?
a.
30 M
c.
2.4 M
b.
15 M
d.
1.2 M
 

 21. 
All of the following are colligative properties EXCEPT ___.
a.
boiling point elevation
c.
vapor pressure increasing
b.
freezing point depression
d.
osmotic pressure
 

 22. 
Stirring ____________________ the speed of dissolving of a solid in a liquid.
a.
increases
c.
has no effect on
b.
desreases
 

 23. 
Decreasing temperature ____________________ the speed of dissolving for a gas in a liquid.
a.
decreases
c.
has no effect on
b.
increases
 

 24. 
How many grams of strontium nitrate Sr(NO3)2 are required to make 2.00 L of a 0.400M ?
a.
415
c.
169
b.
221
d.
245
 

 25. 
How many grams of  cobalt(II) acetate, Co(C2H3O2)2 would you need to make 3.50 L of a 1.25M solution?
a.
169
c.
774
b.
618
d.
238
 

 26. 
Henry’s Law states that the solubility of a gas is __________ to its pressure.
a.
indirectly proportional
c.
not related
b.
directly proportional
d.
dependant upon the gas
 

 27. 
Which one of the following is a correct expression for molarity?
a.
mol solute/L solution
c.
mmol solute/L solution
b.
mol solute/mL solvent
d.
mol solute/kg solvent
 

 28. 
What is the concentration (M) of NaCl in a solution made by mixing 25.0 mL of 0.100 M NaCl with 50.0 mL of 0.100 M NaCl?
a.
0.100
c.
0.0333
b.
0.0500
d.
0.0250
 

 29. 
What is the concentration (M) of CH3OH in a solution prepared by dissolving 11.7 g of CH3OH in sufficient water to give 230 mL of solution?
a.
11.9
c.
0.0841
b.
1.59 x 10-3
d.
1.59
 

 30. 
How many grams of H3PO4 are in 175 mL of a 3.5 M solution of H3PO4?
a.
0.61
c.
20
b.
60
d.
4.9
 

 31. 
What is the concentration (M) of a NaCl solution prepared by dissolving 9.3 g of NaCl in sufficient water to give 350 mL of solution?
a.
18
c.
0.45
b.
0.16
d.
27
 

 32. 
How many grams of NaOH (MW = 40.0) are there in 500.0 mL of a 0.175 M NaOH solution?
a.
2.19 x 10-3
c.
14.0
b.
114
d.
3.50
 

 33. 
How many grams of CH3OH must be added to water to prepare 150 mL of a solution that is 2.0 M CH3OH?
a.
9.6 x 103
c.
2.4
b.
4.3 x 102
d.
9.6
 

 34. 
What is the molarity of an aqueous solution containing 22.5 g of sucrose (C12H22O11) in 35.5 mL of solution?
a.
0.0657
c.
1.85
b.
1.85 x 10-3
d.
3.52
 

 35. 
What is the molarity of an aqueous solution containing 52.5 g of sucrose (C12H22O11) in 35.5 mL of solution?
a.
5.46
c.
0.104
b.
1.48
d.
4.32
 

 36. 
What is the molarity of an aqueous solution containing 22.5 g of glucose (C6H12O6) in 35.5 mL of solution?
a.
0.634
c.
0.197
b.
3.52
d.
0.125
 

 37. 
What is the molarity of an aqueous solution containing 75.3 g of glucose(C6H12O6) in 35.5 mL of solution?
a.
1.85
c.
11.8
b.
2.12
d.
3.52
 

 38. 
What mass (g) of sodium chloride are there in 55.0 mL of a 1.90 M aqueous solution of sodium chloride?
a.
0.105
c.
3.21
b.
6.11
d.
11.5
 

 39. 
What mass (g) of sodium chloride are there in 550 mL of a 1.90 M aqueous solution of sodium chloride?
a.
61.1
c.
11.5
b.
1.05
d.
17.9
 

 40. 
What volume (mL) of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to 200 mL to make a 1.50 M solution of sodium hydroxide?
a.
0.05
c.
45
b.
50.0
d.
800
 

 41. 
What is the molarity of a solution prepared by diluting 43.72 mL of 1.005 M aqueous K2Cr2O7 to 500 mL?
a.
0.0879
c.
0.0218
b.
87.9
d.
0.0115
 

 42. 
What is the molarity of a solution prepared by diluting 43.72 mL of 5.005 M aqueous K2Cr2O7 to 500 mL?
a.
57.2
c.
0.438
b.
0.0044
d.
0.0879
 

 43. 
What is the molarity of an aqueous solution containing 0.1 grams of glucose (C6H12O6) in 50mL?
a.
0.011
c.
0.028
b.
1.11
d.
28.0
 

 44. 
How many grams of sodium chloride are there in 500 mL  of a 0.01 M aqueous solution of sodium chloride?
a.
0.115
c.
0.005
b.
0.292
d.
292.2
 

 45. 
How many milliliters of a concentrated solution of sodium hydroxide (6.00 M) must be diluted to 150 mL to make a 0.2 M solution of sodium hydroxide?
a.
20
c.
0.05
b.
0.250
d.
0.8
 

 46. 
The boiling point of a pure substance is _______ than that of a mixture.
a.
lower
c.
the same
b.
higher
d.
has no effect
 

 47. 
The freezing point of a mixture is ________ than that of a pure substance.
a.
lower
c.
the same
b.
higher
d.
it has no effect
 

 48. 
What is the molality of a solution conaining 0.25 g of C6H4Cl2 dissolved in 10.0 g of C6H12?
a.
0.17
c.
0.025
b.
0.014
d.
0.00017
 

 49. 
What happens to solubility of a solid in a liquid as temperature increases?
a.
goes up
c.
stays the same
b.
goes down
d.
has no effect
 

 50. 
What are the correct units for molality?
a.
mol/L
c.
mol/kg
b.
g/Kg
d.
mol/g
 



 
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