Solutions Test REVIEW PACKET
I. Vocabulary: Must make flashcards
Boiling pt elevation
Colligative property
Colloid
Concentration
Freezing point depression
Immiscible
Insoluble
Miscible
Molarity
Saturated solution
Solubility
Soluble
Solute
Solvation/hydration
TEST: March 12th 2014
Solvent
Supersaturated solution
Suspension
Tyndall effect
Unsaturated solution
electrolytes
Graphs: Solubility Curve
Formulas:

Molarity

Dilution
II. Solutions
A. Fill in the following paragraph with terms from the word bank provided.
“Like dissolves like”
Homogeneous
Soluble
Solvation
Solvent
Solute
A substance that can be dissolved into a solution is __________________. Solutions are ________________ mixtures.
To make salt water, salt must dissolve in water. The salt is the ___________ because it is being dissolved. The water is
the ______________ which does the dissolving. For this dissolving to take place, the water molecules must surround
the sodium and chlorine ions in a process called _________________. This process occurred because ______________.
B. Describe the quickest way to make salt water. Express how the water molecules will surround the salt particles.
C. Solubility Curve-Answer the following questions using the graph provided.
1. 1. What is the solubility of potassium chloride at 10C?
2. What is the solubility of NH3 at 50C?
3. Is ammonia a solid or gas? What happens to the solubility of gases as
temperature increases?
4. At 90C, 10 g of potassium chlorate is dissolved in 100 g of water. Is this
solution saturated, unsaturated, or supersaturated?
5. A saturated solution of potassium chlorate is dissolved in 100 g of water. If
the saturated solution is cooled from 90C to 60C, how many grams of
precipitate will be formed?
6. What is the mass of sodium sulfate that will dissolve in 250 g of water at
30C?
III. Colligative Properties
A. Colligative properties are properties that are affected by the ________________ of particles but not the
_____________ of the dissolved solute particles.
B. Solutions that conduct an electric current are called ____________________.
C. Vapor pressure decreases as the number of solute particles ____________________.
D. The boiling point of a solution is ___________________ than the boiling point of the solution’s solvent.
E. The freezing point of a solution is ____________________ than the freezing point of the solution’s solvent.
IV. Mixtures
Mixture
Particle Size
Scatters Light
Settles
Separated by
Filtering
Solution
Colloid
Suspension
V. Concentration/Dilution Practice Problems
1. What is the molarity of a solution with 96 g of magnesium sulfide in 600mL of solution?
2. How many grams are needed to make a 12 M hydrochloric acid solution using only 100 mL of water?
Explain how to make this solution.
3. How many liters are needed to dilute 200 mL of a 2.5 M solution to a concentration of 1.6 M?
4. What is the molality of a solution with 62.5 g of potassium nitride in 100 g of water?
5. What is the starting concentration of a 500 mL solution that is diluted to 750 mL with a concentration
of 0.55 M?
6. How many liters are there in a 4.65 M solution containing 0.06 moles of sodium chloride?
7. If 48 g of carbon dioxide is dissolved in 600 g of soda, what is the molality of the solution?
8. What is the mass of lithium bromide dissolved in 450 g of water with a molality of 3.75 mol/kg?
9. How many grams of water are needed to dissolve 125 g of barium nitrate to make a 2.95 molal
solution?
10. If I have 300 mL of a sulfuric acid with a concentration of 3.45 M and added 250 mL of water to it, what
is the new concentration?
11. If 500 mL is added to a 3 M nitric acid solution to make 945 mL of a 0.75 M solution, what is the
original volume of the acid?
12. How many kilograms of water are required to dissolve 482 g of calcium oxide to make a 4.32 molal
solution?
13. What is the mass of lithium bromide required to make a 7.92 molal solution using 2500 g of water?
14. How many liters are needed to make a 2.65 molar cesium chloride solution using only 55 g of cesium
chloride?
15. What is the final concentration of a 300 mL solution that has an initial concentration of 5.21 M and
volume of 100 mL?