Solutions

Question 1

Solution

Answer 1

A homogeneous mixture of two or more substances

Question 2

Solute

Answer 2

The substance that gets dissolved

Question 3

Solvent

Answer 3

The substance that does the dissolving

Question 4

Aqueous Solutions

Answer 4

Solutions that have water as the solvent

Question 5

If an ionic solute is dissolved in water →

Answer 5

conducts electricity (electrolyte)

Question 6

If a molecular solute is dissolved in water →

Answer 6

nonconductor (non electrolyte)

Question 7

Solubility

Answer 7

A measurement of how soluble a solute is in a specific solvent under certain conditions (ie temperature and pressure)

Question 8

Soluble

Answer 8

CAN dissolve in solvent

Question 9

Insoluble

Answer 9

CAN’T dissolve in solution

Question 10

In order for solutions to occur…

Answer 10

• The solute and solvent must be attracted to one another

- “Likes Dissolve Likes”

Question 11

What does “Likes Dissolve Likes” mean?

Answer 11

Polar solute can dissolve in polar solvents

Non-polar solute can dissolve in non-polar solvents

Question 12

Unsaturated

Answer 12

A solution that can still dissolve more solute

Question 13

Saturated

Answer 13

The solvent has dissolved the maximum amount of solute possible at a given temperature and pressure

Question 14

Supersaturated

Answer 14

A solution that contains more than could be dissolved by the solvent under normal circumstances

Question 15

Table G

Answer 15

• A point UNDER the line is an UNsaturated solution
• A point ON the line is a saturated solution
• A point ABOVE the line is a SUPERsaturated solution

Question 16

What will increase the solubility of a gas?

Answer 16

Increasing pressure and decreasing temperature

Question 17

How do you make a real gas behave like an ideal gas?

Answer 17

Decreasing pressure and increasing temperature

Question 18

Homogeneous

Answer 18

Looks the same all throughout

Question 19

How do you see if something’s a gas on Table G?

Answer 19

If the line DECREASES

Question 20

How do you see if something’s a solid on Table G?

Answer 20

If the line goes up

Question 21

Concentration

Answer 21

amount of solute per given amount of solvent

Question 22

Molarity

Answer 22

moles of solute per liters of solution

Question 23

Molarity Equation

Answer 23

M = moles solute
———————–
liters of solution

Question 24

Units for Molarity

Answer 24

M or mol/L

Question 25

Molarity TIPS

Answer 25

• Use liters in denominator (ml / 1000 = L)

* Use moles NOT grams

Question 26

Parts per Million

Answer 26

ppm = mass solute
——————— x 1 Million
mass solution

Question 27

PPM and % by Mass TIPS

Answer 27

solute / solute + solvent (solution)

*not over solvent! Over solution!

Question 28

Percent by Mass

Answer 28

mass solute
——————– x 100
mass solution

Question 29

Dilution

increasing the amount of solvent decreases concentration

Answer 29

M1 (V1) = M2 (V2)

• M = molarity
• V= volume

Question 30

Freezing Point Depression

Answer 30

• Solutions have lower freezing pts than water

- More solute = lower freezing pt

Question 31

Boiling Point Elevation

Answer 31

• Solutions have higher boiling points than pure water

- More solute = higher boiling pt

Question 32

Ionic vs Covalent Compounds

Answer 32

Since ionic compounds dissociate into ions, they create a greater concentration of particles!

Question 33

Factors that Affect Solubility

Answer 33

• Temperature
• Pressure
• Nature of solute/solvent

Question 34

Temperature affects solubility

Answer 34

Gases
-As temperature ↑, solubility ↓
Solids
-As temperature ↑, solubility ↑

Question 35

Pressure affects solubility

Answer 35

• ONLY AFFECTS GASES!

- As pressure ↑, solubility ↑

Question 36

Nature of Solute/Solvent

Answer 36

Likes Dissolve Likes