Chemistry
Name: ____________________________
Date: ________ Block: _______
Solutions Review
1.
Refer to Figure 18 to answer the following questions:
a. What mass of potassium nitrate, KNO3, must be dissolved in
100g of water at 50°C to make a saturated solution?
b. We put 50 g potassium nitrate in 100g of water at 30 °C. Is
this solution saturated, unsaturated, or supersaturated? How would you
describe the same solution if it were heated to 60 °C?
2. Rank the substances in Figure 18 from the most soluble to the least
soluble at:
A. 20°C
B. 80°C
3. If the solubility of sugar in water is 2.0 g/mL at room temperature,
what is the maximum mass of sugar that will dissolve in
A. 100 mL of water
B. 355 mL(12 oz can) of water
C. 946mL (1 quart bottle) of water
4. Explain why three teaspoons of sugar will completely dissolve in a serving of heat tea, but not in an equally
sized serving of iced tea.
5. You are given a solution of KNO3 of unknown concentration. What will happen when you add a crystal of KNO3
if the solution is
A. unsaturated?
B. saturated?
C. Supersaturated?
6. A 35-g sample of ethanol dissolved in 115g of water. What is the concentration of the ethanol, expressed as:
A. a percent
B. in pph
C. in ppm
7. Calculate the masses of water and sugar in a 55g sugar solution that is labeled 20%.
8. Distinguish between the terms saturated and unsaturated.
9. Explain the phrase “like dissolves like”.
10. What ion is found in many bases?
11. What element is found in most acids?
12. Distinguish between polar and non-polar molecules.
13. Why does table salt dissolve in water but not in cooking oil?
14. Explain why a bottle of warm soda produces more “fizz” when opened than a bottle of cold soda.
15. How does oxygen get into water?
16.
17.
18.
19.
With increasing water temperature, how does the solubility of oxygen change?
What 2 things is the solubility of a gas in liquid dependent on? Describe the trend for each.
What do bubbles in pop represent?
What affects the rate of bubbling in pop? How does it affect it?
Molarity
1. What is molarity?
2. Find the molarity of a solution that contains 1.5mol of NaOH in 2L of solution.
Find the number of moles present in 1.5L of a .75M solution.
3. Find the volume occupied by 1.5 mol of a 1.25M NaOH.
4. Find the number of grams necessary to create a 1.5L of a 2M solution of NaOH.
5. How many milliliters of 3.0M solution do you need to obtain .75L of 1.5M solution?
3.0M solution
Distilled Water
.75L
1.5M
Acids, Base, pH
1. What is the net ionic equation for an acid/base titration?
2. A weak base has a pH around what? A weak acid has a pH around what?
3. Show how H2SO4 (strong acid) & KOH (strong base) forms ions in solution.
4. Write a total ionic equation for a neutralization reaction of H2SO4 & KOH. Write the net
ionic equation for this neutralization reaction.
5. What is true about the acid and the base when the pH is 7?
6. A solution with a pH of 8 is _____ more basic/less basic than a solution with a pH of 13.
7. Blue litmus paper turns red, this indicates the presence of what? Red litmus paper turns blue, this indicates the
presence of what?
Titration/Neutralization Calculations (Section C)
1. How many milliliters of .24 M H2SO4 would be required to neutralize 20.1 mL of .35M Mg(OH)2?
2. The following data was collected during the titration of a base with a molarity of .34M and an
acid of an unknown molarity. The volume of acid was 16.7 mL and the volume of base used was
27.9 mL. What is the molarity of the acid?
Acid Rain (Section C)
1. What is acid rain?
2. What is the normal pH of rain?
3. Give the reactions that are believed to responsible for acid rain.