Q: A solution is prepared by diluting 45.0 mL of 8.25 M HNO$$_3 to a $$final volume of 135.0 mL. What is the final concentration?

$$C_2$$ = \frac{C_1V_1}{$$V_2$$} = \frac{8.25 \times 45.0}{135.0} = 2.75$$ M

Q: A hospital must prepare an IV solution that is isotonic with blood (osmotic pressure = 7.7 atm at 25°C). What molarity of glucose (C$$_6H$_{12}O$_6) $$should be used? ($$R = 0.08206 L$$·atm/mol·K, $$T = 298 K)$$

$$M = \frac{7.7}{0.08206 \times 298} = 0.316 M$$

Question 1

Which of the following statements best explains why entropy increases when a solution forms?

Accepted Answer

The mixing of solute and solvent leads to a more random distribution of particles.

Question 2

Which of the following is an example of a solid dissolved in a gas?

Accepted Answer

Naphthalene in air

Question 3

A solution is prepared by dissolving 36 g of NaCl in 100 g of water at 293 K. According to the solubility table, is this solution saturated, unsaturated, or supersaturated?

Accepted Answer

Saturated

Question 4

Which intermolecular force is primarily responsible for the solubility of ethanol (C$$_2H$_5OH) in $$water?

Accepted Answer

Hydrogen bonding

Question 5

Arrange the following compounds in order of increasing solubility in water: hexane, ethanol, 1-chloropentane, pentanol.

Accepted Answer

Hexane \u003c 1-chloropentane \u003c pentanol \u003c ethanol

Question 6

What is the general trend for the solubility of ionic compounds in water as temperature increases?

Accepted Answer

Solubility increases for most ionic compounds.

Question 7

Which of the following best describes the effect of temperature on the solubility of gases in water?

Accepted Answer

Solubility of gases decreases as temperature increases.

Question 8

A solution is prepared by diluting 45.0 mL of 8.25 M HNO$$_3 to a $$final volume of 135.0 mL. What is the final concentration?

Accepted Answer

$$C_2$$ = \frac{C_1V_1}{$$V_2$$} = \frac{8.25 	imes 45.0}{135.0} = 2.75$$ M

Question 9

Which equation is used to calculate the vapor pressure of a solution according to Raoult's Law?

Accepted Answer

$$P_{solution} = X_{solvent} P^0$_{solvent}$$

Question 10

If the vapor pressure of a solution is lower than that of the pure solvent, what happens to the boiling point of the solution?

Accepted Answer

The boiling point increases.

Question 11

Which of the following solutions will have the greatest freezing point depression?

Accepted Answer

0.15 m NaCl

Question 12

Calculate the van't Hoff factor ($$i) $$for CaCl$$_2.$$

Accepted Answer

$$i = 3$$

Question 13

Which formula is used to calculate the boiling point elevation of a solution?

Accepted Answer

$$\Delta T_b = i K_b m$$

Question 14

A solution is prepared by dissolving 291 g CaCl$$_2 (MM = 110.98) in $$water to a final volume of 1750 mL. What is the molarity of the solution?

Accepted Answer

$$M = \frac{291}{110.98} \div 1.75 = 1.52 M$$

Question 15

Which of the following best describes osmosis?

Accepted Answer

Solvent moves from higher solvent concentration to lower solvent concentration.

Question 16

What is the equation for osmotic pressure ($$\Pi) $$for a solution containing an electrolyte?

Accepted Answer

$$\Pi = iMRT$$

Question 17

A hospital must prepare an IV solution that is isotonic with blood (osmotic pressure = 7.7 atm at 25°C). What molarity of glucose (C$$_6H$_{12}O$_6) $$should be used? ($$R = 0.08206 L$$·atm/mol·K, $$T = 298 K)$$

Accepted Answer

$$M = \frac{7.7}{0.08206 	imes 298} = 0.316 M$$

Question 18

Which of the following statements about colligative properties is correct?

Accepted Answer

Colligative properties depend only on the number of solute particles.

Chapter 13: Solutions – General Chemistry Study Notes

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