Unit 3: Solutions and Mixtures

Question 1

What is a solution

Answer 1

Homogeneous mixture of a substance, composed of at least 1 solute and 1 solvent

Question 2

What is a Solute?

Answer 2

the substance that is dissolved.

Question 3

What is a solvent?

Answer 3

Medium in which the solute is dissolved; more of it; often water (universal solvent)

Question 4

what is a homogeneous mixture?

Answer 4

Theoretically - uniform at the atomic and molecular level.

Where most liquid and gas state solutions are transparent

However, there are solutions that are colored as well (mostly with solids/metals)

Question 5

what is a heterogeneous mixtures?

Answer 5

contain undissolved particles, are opaque or translucent.

Question 6

add chart on phone

Question 7

What does all aqueous solutions have? (three things)

Answer 7

They have water as a solvent

they may be coloured or colourless (Most useless piece of information but oh well)

are electrolytes (can conduct electricity

Question 8

Recall: molecular and ionic compounds, and acids… are they electrolytes?

Answer 8

ionic = yes
molecular = mostly no
acids = yes

Question 9

How to test the conductivity of electrolytes or solutions?

Answer 9

Ohmmeter

Question 10

what are electrolytes?

Answer 10

Conduct electricity in aqueous form.

Question 11

What is litmus paper used for?

Answer 11

To classify solutes as acids, bases or neutral substances.

Question 12

What does the subscript (alc) mean?

Answer 12

Dissolved in alcohol (any alcohol)

Question 13

what did Svante Arrhenius do 1887?

Answer 13

explain electrolytes

proposed that when a substance dissolves, particles separate and disperse.

Question 14

What makes ionic compounds electrolytes?

Answer 14

Because they are electrolytes, they have electrically charged particles that split away from each other when it dissociates.

Question 15

what do non-electrolytes do in a solution?

Answer 15

They stay in the same compound and won’t go into Ions.

Question 16

Define dissociation?

Answer 16

The separation of ions occurs when an IONIC compound dissolves in water.

Question 16

Define dissociation?

Answer 16

The separation of ions occurs when an IONIC compound dissolves in water.

Question 17

What is dissolving?

Answer 17

the process where a polar solute (any state or type) dissolved in a solvent to form a solution

Question 18

What is low solubility?

Answer 18

Non-polar molecules or low soluble ionic compounds that have a low solubility.

Question 19

What is ionization?

Answer 19

the process by which an acid produces h+(aq) and an anion

Question 20

What does acids do in Arrhenius’ Theory

Answer 20

Ionize to produce H ions that react with OH ions to produce water

Question 21

What do biases do in Arrhenius’ Hypothesis

Answer 21

Ionic hydroxides (OH) dissociate and then reacts with H ions to produce water

Question 22

What is the definition of endothermic?

Answer 22

Absorbing energy from surroundings

Question 23

What is the definition of exothermic?

Answer 23

Release energy from to the surroundings

Question 24

Does breaking bonds or forming bonds release or require energy

Answer 24

Breaking bonds = uses energy. Forming bonds = releases energy.

Question 25

What is concentration?

Answer 25

The ratio of solute to solvent

Question 26

What is the definition of a dilute solution?

Answer 26

Has a relatively small quantity of solute per unit volume of solvent

Question 27

What is the definition of a concentrated solution?

Answer 27

Has a relatively large quantity of solute per unit volume of solvent.

Question 28

How to do volume by volume concentration

Answer 28

V solute. *100% = V% V solution Make sure you say v/v at the end Make sure the units are the same

Question 29

How to do % concentration mass by volume?

Answer 29

M solute *100 = concentration V solution Make sure you say m/v at the end Make sure that the units are the same

Question 30

How to do concentration mass by mass

Answer 30

M solute *100 = concentration M solvent Make sure units are the same

Question 31

What is molarity of a solution?

Answer 31

M/L Always in moles per litre.

Question 32

What does M mean?

Answer 32

Moles per litre.

Question 33

How to do parts per million concentration

Answer 33

(Miligram)/kg = ppm Miligram/L = ppm

Question 34

What is parts per billion and parts per trillion ratio

Answer 34

1 : 10 to the nine | 1 : 10 to the twelve

Question 35

How can solutions be prepared?

Answer 35

``` Solid solute Dilution method (oj from frozen concentrate) ```

Question 36

What is a standard solution?

Answer 36

Solution of accurate concentration used in and prepared for labs and industry

Question 37

What are the two pieces of equipment necessary to prepare a solution from a solid?

Answer 37

Electronic balances, volumetric flasks

Question 38

How to prepare a dilution solution

Answer 38

Start with the stock solution (concentrated samples taken for dilution) Then decide if you want it to be dilute (less than 0.1 mol/L) or concentrated (more than 1 mol/L) Add solvent

Question 39

What is the solution formula?

Answer 39

CV = C2V2 Where C is the concentration And V is volume (V can be any unit as long as it's the same)

Question 40

Why should you dilute a solution?

Answer 40

To slow down a reaction

Question 41

What is the equipment necessary to dilute a solution?

Answer 41

Graduated pipette, and volumetric pipette, volumetric flask

Question 42

What type of relationship does concentration and volume

Answer 42

A INVERSE RELATIONSHIP!

Question 43

What is Ion concentration? What is a mole ratio?

Answer 43

of ions in a solution as a ratio One mol of [CaCl2] Equals one mol of [Ca 2+] And two mol of [Cl -] to create a 1:1:2 ratio (compound, cation, anion)

Question 44

How to find ion concentration

Answer 44

Concentration • number of ion mol's / number of mol's in solution Ex 0.500mol/L of CaCl2 • 2/1 = 1mol/L of Cl2

Question 45

What is an unsaturated solution?

Answer 45

More solute can be added. Test by adding more solute

Question 46

What is a saturated solution?

Answer 46

Max amount of solute in a given temp. Test by adding more solute and it will not dissolve

Question 47

What is a supersaturated solution?

Answer 47

More than the max amount of solute is dissolved at given conditions (by heating and cooling it) The test is adding more solute and the solution crystalizes

Question 48

What is dynamic equilibrium?

Answer 48

When two opposite processes happen at the same rate. Ex The rate of dissolving is equal to the crystallization process.

Question 49

What is BCE?

Answer 49

Balanced chemical equation

Question 50

What is TIE?

Answer 50

Total ionic equation

Question 51

What is NIE?

Answer 51

Net ionic equation

Question 52

What is a ppt?

Answer 52

Precipitate

Question 53

What is a spectator ion?

Answer 53

an ion that exists as a reactant and a product in a chemical equation. Removed for the NIE

Question 54

When are solids more soluble in water?

Answer 54

When the water temp. Is higher

Question 55

When are gasses more soluble in water

Answer 55

Lower temp, higher pressure.

Question 56

What is the relationship between the solubility of gas as temp increases

Answer 56

AN INVERSE RELATIONSHIP

Question 57

What increases the solubility of polar substances?

Answer 57

Higher temp.

Question 58

What happens if you try to dissolve any amount of polar molecules with h bonding?

Answer 58

ALL OF IT gets dissolved. (Can NEVER become a saturated solution)

Question 59

Do elements dissolve? What are the edge cases? What reacts with water?

Answer 59

No Halogens and oxygen gas (Halogens and alkali metals)