Unit Seven

Question 1

Heterogeneous mixture

Answer 1

Do not have uniform composition (can see different parts)

Ex sand and water

Question 2

Homogeneous mixture

Answer 2

Have uniform composition throughout (can’t see different parts)
Another name for a homogeneous mixture is a solution
Ex sugar and water

Question 3

Aqueous

Answer 3

When substances are in a solution with water

Question 4

Universal solvent

Answer 4

Water is the most common solvent used in the world, referred to as universal solvent

Question 5

Distillation

Answer 5

Separates liquids based on boiling points

Question 6

Centrifuge

Answer 6

Rapid spinning of a mixture to separate particles by density

Question 7

Decant

Answer 7

Pouring a liquid off a solid

Question 8

Filtration

Answer 8

Using a porous barrier to separate components of a mixture

Question 9

Chromatography

Answer 9

Ability to run across a surface

Question 10

Suspension

Answer 10

A dispersion of large particles that are temporarily suspended and settle out naturally over time
Ex orange juice with pulp

Question 11

Colloid

Answer 11

Consists of two phases of matter and are only heterogeneous on a microscopic level (can’t see different parts with naked eye)
Cloudy
Ex milk

Question 12

Major differences between suspension and colloids

Answer 12

Suspension do not have uniform composition, colloids have uniform composition
Colloids have much smaller particles than suspensions do
Because colloids don’t settle out, they are considered stable, suspensions are not stable because over time the parts of the mixture will separate

Question 13

Solute

Answer 13

The substance that is being dissolved

Ex salt in salt and water

Question 14

Solvent

Answer 14

The substance doing the dissolving

Ex water in salt and water

Question 15

How to tell apart colloids and solutions

Answer 15

Colloids are cloudy

Solutions are clear

Question 16

Solubility

Answer 16

The amount of solute that dissolves in a given amount of solvent

Question 17

Factors affecting solubility (dissolving a solid solute in a liquid solvent)

Answer 17

Temperature: increasing the temperature will increase solubility
Agitation: stirring the solution helps increase the solubility
Surface area: the smaller the particles the more quickly they will dissolve

Question 18

Saturated solution

Answer 18

Contains the maximum amount of solute for a given amount of solvent at a constant temperature

Question 19

Unsaturated solution

Answer 19

Contains less solute than a given amount of solvent can dissolve

Question 20

Supersaturated solution

Answer 20

Contains more than the maximum amount of solute that a given amount of solvent can dissolve

Question 21

How can you make a supersaturated solution?

Answer 21

Create a saturated solution
Heat up the solution
Add more solute
Cool to room temperature

Question 22

Above line
On line
Below line

Answer 22

Supersaturated
Saturated
Undersaturated

Question 23

Mixture

Answer 23

Two or more pure substances physically combined, components retain properties

Question 24

Soluble/insoluble

Answer 24

Used to describe when a solid/gas solute does/does not dissolve

Question 25

Miscible

Answer 25

Two liquids that can dissolve in one another Ex water and ethanol For liquids only

Question 26

Immiscible

Answer 26

Two liquids that cannot dissolve one another Ex oil and water Only for liquids

Question 27

Factors affecting solubility of gases

Answer 27

Agitation up, solubility down Temperature up, solubility down Pressure up, solubility up

Question 28

Solubility rule

Answer 28

Like dissolves like | Polar substances dissolve other polar substances, nonpolar substances dissolve other nonpolar substances

Question 29

Solvation

Answer 29

The surrounding of solute particles by solvent particles (dissolving) Ionic compounds dissociate or break apart in water. Water molecules are attracted to ions on the surface of the crystal. Gradually, the water molecules surround each individual ion. This reduces the attraction of the ions for each other, and they are no longer held in the crystalline structure. The ions gradually break apart and move into solution.

Question 30

Electrolytes

Answer 30

Solutions that have the ability to conduct electricity

Question 31

PRACTICE WITH SOLUBILITY CURVES GRAPH ON P3 OF CLASSWORK

Answer 31

OKAY

Question 32

Concentration

Answer 32

A measure of the amount of solute that is dissolved in a given amount of solvent

Question 33

Dissociate

Answer 33

When ionic compounds break apart in water

Question 34

Diluted solution

Answer 34

Contains a low ratio of solute to solution (small concentration of solute)

Question 35

Concentrated solution

Answer 35

Contains a high ratio of solute to solution (high concentration of solute)

Question 36

Molarity (M)

Answer 36

The number of moles of solute dissolved per liter of solution Say a solution is molar (ex 0.5 molar) Most important unit of concentration in chemistry

Question 37

Molarity equation

Answer 37

M = moles/liters = n/L = mol/L

Question 38

In diluting solutions, the concentration is

Answer 38

Lowered | However, the total number of moles of solute remains unchanged

Question 39

Dilution/concentration equation

Answer 39

M1V1 = M2V2