Ch.13

Question 1

Solution

Answer 1

A homogenous mixture with at least two components.

Ex. Ocean Water (Salt and Water)

Question 2

Solvent

Answer 2

The majority component in a solution; what the other component mixes into.
*The liquid is almost always the solvent regardless of ratio
CO2- Solute
H2O- Solvent

Question 3

Solute

Answer 3

The minority component of the solution that ‘mixes in’.

Question 4

Aqueous Solution

Answer 4

A solution with water as the solvent.

*Water is the most common solvent because of it’s abundance on Earth.

Question 5

Like Dissolves Like

Answer 5

Polar solvents (such as water), dissolve other polar solute, while nonpolar solvents dissolve other nonpolar solutes.

Question 6

Insoluble

Answer 6

Compounds, molecules etc. that do not dissolve in solvents.

Ex. Calcium Carbonate

Question 7

How do solids dissolve in water?

Answer 7

The solvent-solute attraction must overcome that of the solvent-solvent and solute-solute attractions (usually intermolecular forces).
The negatively charged ions are attracted to positively charged dipoles and vice versa.

Question 8

Solubility

Answer 8

The amount of the compound, in grams, that dissolves in a certain amount of liquid.

Question 9

Saturated Solution

Answer 9

The maximum amount of solute is held, more solute added will not dissolve.

Question 10

Unsaturated Solution

Answer 10

Less than the maximum amount of solute is held and more can be added.

Question 11

Supersaturated solution

Answer 11

More than normal amount of solute is held and the solute will precipitate.

Question 12

Electrolyte Solutions

Answer 12

Hold dissolved ions, charged particles, and conduct electricity.

Question 13

Non-electrolyte Solution

Answer 13

Hold dissolved molecules, neutral particles, and do not conduct electricity.

Question 14

Solubility of Solids and Temp.

Answer 14

The solubility of solids in a liquid is directly proportional to temp. As temperature rises, so does solubility.

Question 15

Recrystallization

Answer 15

Solid is added to solvent at high temperature enough to make a saturated solution then allowed to cool slowly, reducing solubility steadily, causing the solid to precipitate as pure crystals.

Question 16

Solubility of Gases and Temp.

Answer 16

The solubility of gas and temperature is inversely proportional, as temperature increases, solubility decreases.
Ex. Warm soda fizzes much more than cold soda.

Question 17

Henry’s Law

Answer 17

The higher the pressure of gas above a liquid, the higher the solubility.
Ex. This is why soda pops when opened. Pressure is released decreasing solubility and causing co2 to bubble out of the solution.

Question 18

Mass Percent

Answer 18

Concentration of a solution or the number of grams of solute per 100g of solution.

Question 19

Mass Percent Equation

Answer 19

Mass percent=
Mass Solute / (mass of solute + mass of solvent) x 100%.

Or

Mass Percent = g solute/ 100g solution

Question 20

Molarity

Answer 20

The number of moles of solute over liter of solution.

Molarity (M) = Moles of Solute/ Liters of Solution

Question 21

Concentration of a solution containing a Molecular Compound

Answer 21

Reflects the concentration of the solute as it actually exists in the solution.

Question 22

Concentration of a solution containing an Ionic Compound

Answer 22

Reflects the concentration of the solute before it is dissolved in the solution.

Question 23

Dilution

Answer 23

Adding water to a stock solution to make it less concentrated.

Question 24

Dilution Equation

Answer 24

M1V1=M2V2

Where M is molarity and V is volume.

Question 25

Colligative Properties

Answer 25

Properties that depend on the number of dissolved solute particles and not the type of solute particles.

Question 26

Non-volatile solute

Answer 26

A solute that does not readily evaporate.

Question 27

Freezing Point Depression

Answer 27

Adding a non-volatile solute to a solution in order to lower its freezing point.

Question 28

Boiling Point Elevation

Answer 28

Adding a non-volatile solute to a solution to make it's boiling point higher.

Question 29

Molality (m)

Answer 29

Used to express the concentration of solution with freezing point depression and boiling point elevation. Reflects the number of moles of solute per kilogram of SOLVENT.

Question 30

Freezing Point Depression Quantification

Answer 30

^Tf = m x Kf Where: ^T is he change in temp. In C. M is the molality Kf is the constant 1.86 Ckg solvent/mol solute

Question 31

Boiling Point Elevation Quantification

Answer 31

^Tb=m x Kb Kb= 0.512 Ckg solvent/mol solute

Question 32

Osmosis

Answer 32

The flow of solvent from a less concentrated solution to a more concentrated solutions.

Question 33

Osmotic Pressure

Answer 33

The pressure created when enough excess fluid crosses the semipermeable membrane. A colligative property; the more concentrated a solution to greater the osmotic pressure.

Question 34

Hypoosmotic

Answer 34

Solutions having osmotic pressures less than that of bodily fluids. Pump water into cells.

Question 35

Hyperosmotic

Answer 35

Solutions that have osmotic pressures greater than that of bodily fluids. Pump water out of cells.

Question 36

Isoosmotic

Answer 36

Solutions that have osmotic pressure equal to bodily fluids.