Solutions


Your test will be on Chapter 15 Water and Chapter 16 Solutions. We will NOT be testing on the last section of Ch16: colligative properties. This review has several practice questions for you to complete as a study tool. It also has several online practice quizzes to give you more practice and immediate feedback to answers.

Use the following links as additional online practice:

The following questions will help you study for your unit test on Ch15 and Ch16:

1.
Why is a water molecule polar?
2.
Many properties of water are the result of ________
3.
The fact that ice is less dense than water is related to the fact that ____.
4.
A substance that dissolves in a water to form a solution that conducts an electric current is said to be an:
5.
What causes water's low vapor pressure?
6.
What causes the surface of water in a graduated cylinder to be concave instead of straight
7.
Nonpolar substances like hexane tend to be (soluble or insoluble) in water.


Use the solubility graph from your textbook to answer questions 8-12
Reference: sat

8.
75 g KNO3 in 50mL of water at 50oC
9.
20 g NaCl in 100 g water at 25oC
10.
Which of the following substances is less soluble in hot water than in cold water?
A.
KNO3
B.
KCl
C.
NaCl
D.
HCl
11.
A beaker containing 65 grams of ammonium chloride, NH4Cl, in 100 grams of water has a temperature of 70 ºC. Approximately how many grams of the salt are undissolved on the bottom of the beaker?
12.
Which salt is LEAST soluble at 50oC?
A.
KNO3
B.
KClO3
C.
NaCl
D.
NH4Cl


13.
Which of the following salts are considered to be soluble in water? (Use the solubility chart from your textbook)
A.
BaSO4
B.
NH4Cl
C.
AgI
D.
PbS
14.
Explain why a bottle of warm soda fizzes more than a bottle of cold soda when opened
15.
What will increase the solubility of a gas in water?
16.
For a given substance, what will influence how fast it dissolves?
17.
In a solution of sugar and water, what is the solute and what is the solvent?
18.
In a saturated solution containing undissolved solute, solute is continuously dissolving, but the concentration of the solution remains __________.
19.
A solution of seawater contains 7.5 g salt in 92.5 g of water. What is the percent concentration?
20.
You are given 100 grams of a 25% sugar solution by mass. This solution contains how many grams of solute? solvent?
21.
2000 mL of 70% alcohol by volume contains ___ mL of the alcohol.
22.
What is the formula for percent by volume? percent by mass?
23.
The molarity of a solution containing 7.50 mol of acetic acid, HC2H3O2 in 390. mL of solution is ___.
24.
How many grams of K2SO4 are contained in 200. mL of 0.400 M K2SO4 solution?
25.
Diluting a solution changes ___ but not the amount of _____.
26.
If 200 mL of a 2.50M NaCl solution is diluted to 500 mL, what is the new concentration of NaCl?
27.
To make a 1M aqueous solution of NaCl, 58.4 grams of NaCl are dissolved in
28.
How many moles of NaCl are present in 75. mL of 0.80 M solution?
29.
Which of the following operations yields the number of moles of solute?
A.
molarity x moles of solution
B.
molarity x mass of solution
C.
molarity x liters of solution
D.
moles of solution / volume of solution

 

The following questions are EXTRA CREDIT on your test since they are from the section that we are skipping from Ch16:

30.
When a solute like magnesium chloride is dissolved in a solvent, the freezing point of the solution will be ____ than that of the pure solvent.
31.
Which of the following solutions, each made by dissolving 1mole of solute in 1 L of water, will have the highest boiling temperature? Which one will have the lowest freezing point?
A.
sodium phosphate, Na2PO4
B.
glucose, C6H12O6
C.
sodium chloride, NaCl
D.
aluminum chloride, AlCl3