Chapter 8 - Solutions

Question 0

What’s a Solvent?

Answer 0

Does the dissolving.

Question 1

What are homogenous mixtures?

Answer 1

They have uniform properties and components through out.

Question 2

What’s a Solute?

Answer 2

Is dissolved.

Question 3

What is a Saturated Solution?

Answer 3

It is a solution in which no more solute will dissolve under the existing conditions of temperature and pressure.

Question 4

What is an Unsaturated Solution?

Answer 4

A solution that contains less than the quantity of solute needed to saturate it under the existing conditions.

Question 5

What is a supersaturated solution?

Answer 5

It is a solution in which contains more solute than a saturated solution would normally hold under the existing conditions of temperature and pressure.

Question 6

How do you create a supersaturated solution?

Answer 6

Prepare a saturated solution at high temperatures and then cool it back to room temperature. Toffee

Question 7

Like dissolves Like

Answer 7

Polar substances will dissolve in polar solvents and Non-Polar substances will dissolve in Non-Polar solutes.

Question 8

What happens to gases in liquids when the temperature increases?

Answer 8

The solubilities of gases in liquids decrease with increasing temperature. This explains the bubbles that first appear when water is being heated.

Question 9

How does the increase in temperature and the decrease in the solubility of gases affect the environment?

Answer 9

Is the temperature of the water in rivers, lakes and oceans increases slightly, then it will contain less oxygen - possible not enough oxygen to support aquatic life.

Question 10

When pressure increases …

Answer 10

The solubility of the gas increases.

Question 11

What is dissociation?

Answer 11

Dissociation is the process involving the breaking apart of an ionic lattice into separated ions.

Question 12

What are Electrolytes?

Answer 12

Electrolytes are substances that produce ions in solution (water).

Question 13

Ionic compounds are Strong Electrolytes why?

Answer 13

They COMPLETELY break up into ions when they dissolve in water.

Question 14

What are Non-Electrolytes?

Answer 14

Non-electrolytes are substances that have molecules that remain intact during the formation of the aqueous solution.

Question 15

What is Ionisation?

Answer 15

Ionisation is the process in which a neutral species form on or more ions.

Question 16

What are Weak Electrolytes?

Answer 16

Where only some of the dissolved molecules form ions.

Question 17

Strong Acids

Answer 17

HNO3 - Nitric Acid
H2SO4 - Sulfuric Acid 
HCL -Hydrochloric Acid 
HBr - Hydrobromic Acid 
HI - Hydroiodic Acid 
HCLO4 - Perchloric Acid

Question 18

Weak Acid

Answer 18

CH3COOH - Acetic Acid 
HF - Hydrofluoric Acid
H3PO4 - Phosphoric Acid
H2SO3 - Sulfurous Acid
HNO2 - Nitrous Acid
HCLO - Hypochlorous Acid 
H2CO3 - Carbonic Acid 
HCN - Hydrogen Cyanide 
H2S - Hydrogen Sulfide
CH3CH(OH)COOH - Lactic Acid 
C6H8O7 - Citric Acid 
NH4+ - Ammonium Ion 
HSO4 - Hydrogensulfate ion

Question 19

Strong Bases

Answer 19

Metal Hydroxides

NaOH
KOH
Ca(OH)2

Question 20

Weak bases

Answer 20

NH3 - Ammonia 
HCO3 - Hydrogencarbonate ion
CO3^-2 - Carbonate Ion
S^-2 - Sulfide Ion 
PO4^-3 - Phosphate Ion 
CH3COO^- - Acetate Ion 
F- - Fluoride Ion

Question 21

What is Concentration?

Answer 21

Concentration is the amount of solute in a given amount of solution or solvent.

Question 22

What is a Concentrated Solution?

Answer 22

A Concentrated Solution is one in which a large amount of solute is dissolved in a relatively small volume of solvent.

Question 23

What is Dilution?

Answer 23

Dilution is the process of adding more solvent to a solution.

Question 24

Solutions of strong electrolytes have high electrical conductivities.

2 exceptions to this is:

Answer 24

1. If the solution of the strong electrolyte is extremely dilute, it’s conductivity will be low.
2. If the solubility if the strong electrolyte is small, then the conductivity of its solution will be low.

Question 25

Soluble Strong Electrolyte

Answer 25

High Concentration = High conductivity

Eg. NaCl, HCl

Question 26

Insoluble Strong Electrolyte

Answer 26

High Solubility = High Conductivity

Eg. AgCl

Question 27

Soluble Weak Electrolyte

Answer 27

High Concentration = High Conductivity

Eg. CH3COOH

Question 28

Soluble Non-Electrolyte

Answer 28

Non-Conducting

Eg. C12H22O11

Question 29

What are Colligative Properties?

Answer 29

They are properties that change depending on the ratio of the number of particles of solute - not the type of particles - for the number of particles of solvent in the solution.

Question 30

What are the 3 Colligative properties?

Answer 30

1. Vapor Pressure
2. Melting Temperature
3. Boiling Temperature

Question 31

Increase in number of dissolved particles =

Answer 31

Decrease in Vapor Pressure

Question 32

Vapour Pressure and Temperature

Answer 32

If the Vapour pressure is lowered by addition of a solute, then the solution will need to be heated to a higher temperature than that required for the pure solvent, in order for the Vapour pressure to equal the prevailing atmospheric pressure.

Question 33

Freezing Temperature Depression

Answer 33

The presence of dissolved solute interferes with the crystallization process, this requiring that the temperature of the solution be lowered below the freezing point of the pure solvent in order for freezing to occur.

Question 34

Define Chemical Changes.

Answer 34

New substances with different compositions and properties are formed.

Question 35

Define Physical Changes.

Answer 35

Occur with altering the composition of the particular substance (shape, volume or change in state, such as melting and boiling)