# The Behavior of Gases s1

Unit 12: Solutions

Practice Test

Objective 1: Solution properties (p. 453 – 458)

Determine whether the statements about the observable properties of solutions are TRUE (T) or FALSE (F)

___ 1.  Solutions are also known as homogeneous mixtures.

___ 2.  Solutions can be filtered to collect the solute.

___ 3.  A saturated solution is an example of a dynamic equilibrium process.

___ 4.  If solid potassium chloride dissolved in water, water would be considered the solute.

Select the best choice.

___ 5.  Which of the following is NOT an electrolyte?

A)  Sodium chloride B) hydrogen chloride C) sugar D) potassium chloride

___ 6.  Oil dissolves in carbon tetrachloride. Oil would be considered:

A)  Soluble B) miscible C) immiscible D) insoluble

___ 7.  Sugar in water is an example of which solute-solvent combination?

A)  gas-liquid B) liquid-liquid C) solid-liquid D) liquid solid

___ 8.  Which of the following usually makes a substance dissolve faster in a solvent?

A)  Agitating the solution B) increasing the particle size C) Lowering the temperature 9. Explain the orientation of the water molecules around the sodium and chloride ions seen in the diagram above.

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Score box / □ A= 9/9 (100) / □ B= 8/9 (89) / □ NY

Objective 2: Solubility and Interpreting Solubility curves. (p. 457-459)

Directions: Using the solubility curve, answer the following questions.

1.  Which compound is least soluble in water at 50ºC? ______

2.  How many grams of KNO₃ can be dissolved in 100g H₂O at 60ºC? ______

3.  At 20ºC, 20 grams of KCl is added to 100 g of H2O water. Is the solution saturated, unsaturated, or supersaturated? ______

4.  At 80ºC, how much NH₃ can be dissolved in 200 g. H₂O? ______

5.  90 g of NaNO3 is added to 100 g H2O at 0C. To what temperature must the solution be raised to in order to produce a saturated solution? ______

6.  If 100 grams of NH4Cl is added to 100 grams of water at 90ºC, how many grams will not dissolve? ______

______

___7. All the KBr that will dissolve in a solution has dissolved and several undissolved crystals remain at the

bottom. The solution is:

A)  Saturated B) Unsaturated

C) Supersaturated D) At the incorrect pressure t dissolve the solid

___ 8. How can you best increase the solubility of a gas in a liquid?

A)  Increase both the temperature and pressure

B)  Decrease both the temperature and pressure

C)  Increase the temperature and decrease the pressure

D)  Decrease the temperature and increase the pressure

___ 9. A substance that is not soluble in a polar solvent is

A)  Nonpolar B) Ionic C) Polar D) Hydrogen bonded

Score box / □  A= 9/9 (100) / □  B= 8/9 (89) / □  NY

Objective 3: Determine the concentration of solutions using molarity and describe how to prepare molar solutions. (p. 464- 466)

Directions: Solve the following problems, including all WORK, FORMULAS, UNITS, and SIG FIGS. Place a BOX around your final answer.

1. What is the molarity of a solution of KOH if 1.30 liters of the solution contains 0.56 moles of KOH? (1)

2. You have a 3.5 L solution that contains 60.0 grams of KCl. What is the molarity of the solution? (2)

3. To what volume should 5.0 g Na2SO4 be diluted in order to prepare a .25M Na2SO4 solution?(2)

4. You want to make 400.0 mL of a KF solution with a concentration of 0.500 M. How many grams of

KF do you need?(3)

5. Describe in words how you would make the solution found in problem 4.(1)

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6. If you have 355 mL of a 2 M solution of NaBr, what will its new concentration be if I add 600 mL of water to the

solution?

7. If I dilute a 100.0 mL sample of 1.00 M sodium acetate to a volume of 750.0 mL, what will the resulting solution’s

new concentration be?

Score box / □  A= 9/9 (100) / □  B= 8/9 (89) / □  NY