1. Intro to General Chemistry

2. Atoms & Elements

3. Chemical Reactions

4. BONUS: Lab Techniques and Procedures

5. BONUS: Mathematical Operations and Functions

6. Chemical Quantities & Aqueous Reactions

7. Gases

8. Thermochemistry

9. Quantum Mechanics

10. Periodic Properties of the Elements

11. Bonding & Molecular Structure

12. Molecular Shapes & Valence Bond Theory

13. Liquids, Solids & Intermolecular Forces

14. Solutions

15. Chemical Kinetics

16. Chemical Equilibrium

17. Acid and Base Equilibrium

18. Aqueous Equilibrium

19. Chemical Thermodynamics

20. Electrochemistry

21. Nuclear Chemistry

22. Organic Chemistry

23. Chemistry of the Nonmetals

24. Transition Metals and Coordination Compounds

[BOOK CHEM] Clutch Version

Which of the following solutions has the lowest vapor pres- sure? (Assume complete dissociation for ionic compounds.) (LO 13.10)
(a) An aqueous solution of 0.25 m Ca1NO322
(b) An aqueous solution of 0.30 m sodium chloride (NaCl)
(c) A mixture of 50 mL of water and 50 mL of ethanol
1CH3CH2OH2
(d) A mixture of 25 mL of water and 50 mL of ethanol
1CH3CH2OH2

13.122 When salt is spread on snow-covered roads at - 2 °C, the snow melts. When salt is spread on snow-covered roads at
- 30 °C, nothing happens. Explain.

Colligative Properties Explained

The Colligative Properties

Colligative Properties - Boiling Point Elevation, Freezing Point Depression & Osmotic Pressure

A solution contains 50.0 g of heptane (C7H16) and 50.0 g of
octane (C8H18) at 25 °C. The vapor pressures of pure heptane
and pure octane at 25 °C are 45.8 torr and 10.9 torr, respectively.
Assuming ideal behavior, answer the following:
d. Why is the composition of the vapor different from the composition of the solution?

Which of the following compound will have the highest vapor pressure?

The Colligative Properties Example 2

The Colligative Properties Concept 1

You make a solution of a nonvolatile solute with a liquid
solvent. Indicate if each of the following statements is true
or false. (d) The boiling point of the solution increases in 
proportion to the concentration of the solute.

List the following aqueous solutions in order of increasing boiling point: 0.120 m glucose, 0.050 m LiBr, 0.050 m
Zn1NO322.

You make a solution of a nonvolatile solute with a liquid
solvent. Indicate if each of the following statements is true
or false. (b) The solid that forms as the 
solution freezes is nearly pure solute.

If cost per gram were not a concern, which of the following substances would be the most efficient per unit mass for melting snow from sidewalks and roads: glucose 1C6H12O62, LiCl, NaCl, or CaCl2? Explain.

The Colligative Properties Practice 2

You make a solution of a nonvolatile solute with a liquid
solvent. Indicate if each of the following statements is true
or false. (a) The freezing point of the solution is unchanged
by addition of the solvent.

When 1 mL of toluene is added to 100 mL of benzene (bp 80.1 °C), the boiling point of the benzene solution rises, but when 1 mL of benzene is added to 100 mL of toluene (bp
110.6 °C), the boiling point of the toluene solution falls. Explain.

The Colligative Properties Concept 2

Molality and Colligative Properties

The Colligative Properties Example 1

13 - Solutions and Colligative Properties

Some Colligative Properties will increase and others will decrease with the addition of solute to a pure solvent.

Assuming equal concentrations and complete dissociation, arrange these aqueous solutions by their freezing points.

(a) Does a 0.10 m aqueous solution of NaCl have a higher 
boiling point, a lower boiling point, or the same boiling 
point as a 0.10 m aqueous solution of C6H12O6?

Two beakers, one with pure water (blue) and the other with a solution of NaCl in water (green), are placed in a closed container as represented by drawing (a). Which of the draw- ings (b)–(d) represents what the beakers will look like after a substantial amount of time has passed?<img src="https://lightcat-files.s3.amazonaws.com/problem_images/bce4689786660d41-1671659970651.jpg" alt="" /><img src="https://lightcat-files.s3.amazonaws.com/problem_images/306a4d40f9f0a8a5-1671660528095.jpg" alt="" />

The following phase diagram shows part of the vapor- pressure curves for a pure liquid (green curve) and a solution of the first liquid with a second volatile liquid (red curve).<img src="https://lightcat-files.s3.amazonaws.com/problem_images/a36a442ab0590c29-1671640162672.jpg" alt="" /> (a) Is the boiling point of the second liquid higher or lower than that of the first liquid?

Assume that you have a liquid in a cylinder equipped with a movable piston. There is no air in the cylinder, the volume of space above the liquid is 200 mL, and the equilibrium vapor pressure above the liquid is 28.0 mm Hg. What is the equilibrium pressure above the liquid when the volume of space is decreased from 200 mL to 100 mL at constant temperature?

Two beakers are placed in a sealed box at 25 °C. One beaker
contains 30.0 mL of a 0.050 M aqueous solution of a nonvolatile nonelectrolyte. The other beaker contains 30.0 mL
of a 0.035 M aqueous solution of NaCl. The water vapor
from the two solutions reaches equilibrium. (a) In which
beaker does the solution level rise, and in which one does
it fall?

The Colligative Properties Practice 1

A solution concentration must be expressed in molality when considering boiling-point elevation or freezing-point depression but can be expressed in molarity when consider- ing osmotic pressure. Why?

The Colligative Properties Concept 3

Which of the following compounds will have the highest boiling point?

The Colligative Properties Example 3

Which solution has the highest vapor pressure?
a. 20.0 g of glucose (C6H12O6) in 100.0 mL of water
b. 20.0 g of sucrose (C12H22O11) in 100.0 mL of water
c. 10.0 g of potassium acetate KC2H3O2 in 100.0 mL of water

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Types of Aqueous Solutions

When an ionic solid dissolves, ions leave the solid and become dispersed in the solvent. Three possible aqueous solutions can be formed:saturated, unsaturated and supersaturated.

Boiling Point Elevation

Boiling Point Elevation is the phenomenon when adding a solute to a pure solvent results in increased boiling point of the solvent.

Intro to Henry's Law

According to&nbsp;Henry's Law, at a constant temperature the amount of a gas dissolved in a solvent is directly proportional to its partial pressure when it is in equilibrium with its liquid phase.&nbsp;

Osmotic Pressure

Osmotic Pressure is the force that drives Osmosis from higher concentration to lower concentration.

Mole Fraction

Mole Fraction (X) relates the moles of solute and solvent within a solution.&nbsp;

The&nbsp;Colligative Properties&nbsp;explain what happens to a pure solvent as it transitions to a solution.

Molality

Molality (m)&nbsp;represents the number of moles of solute dissolved per kilogram of solvent.&nbsp;

Freezing Point Depression

Freezing Point Depression is the phenomenon when adding a solute to a pure solvent results in decreased freezing point of the solvent.

Solutions: Solubility and Intermolecular Forces

Solutions are homogeneous mixtures that result from the dissolving of a solute by a solvent.

Vapor Pressure Lowering (Raoult's Law)

Vapor Pressure is the pressure exerted by a gas at equilibrium with its liquid phase at a specific temperature in a closed system.

Henry's Law Calculations

To calculate solubility of a dissolves gas, Henry's Law Constant and partial pressure are used.

Solutions: Mass Percent

Mass Percent represents grams of solute per grams of solution, multiplied by 100.

Osmosis

Osmosis is the net movement of solvent across a semipermeable membrane.

Parts per Million (ppm)

<div dir="auto"><div contenteditable="true"dir="auto"spellcheck="true">Parts per Million (ppm) and Parts per Billion (ppb) are used to express extremely dilute solution concentrations.</div></div>

Classification of Matter (1)

Classification of Matter (2)

Classification of Matter - Example

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