Unit 3: Outcome 1

Question 1

Solute

Answer 1

a substance that is
dissolved

Question 2

Solvent

Answer 2

the medium in which a
solute is dissolved

Question 3

what is an example of a solute

Answer 3

sugar,salt

Question 4

what is an example of a solvent

Answer 4

water

Question 5

What does aqueous mean

Answer 5

dissolved in water

Question 6

Aqueous solutions can be classified as what

Answer 6

electrolytes or non electrolytes

Question 7

Dissociation

Answer 7

the separation of an ionic compound into its ions when in water

Question 8

What is an example of a chemical reaction that shows Dissociation?

Answer 8

Salt water, Sodium Sulfate and water, Barium Sulfate in water

Question 9

Ionization

Answer 9

– process by which a molecule is converted into an ion or ions

Question 10

Are Acids molecular or ionic compounds?

Answer 10

Acids are molecular compounds that, when placed in water, ionize to form a hydrogen ion (H+) and a
negative ion (X-) Ionization equations show the formation of ions from a compound that is not made up of ions

Question 11

What’s an example of ionization

Answer 11

HCl(g) in water

Question 12

When A bond breaks what happens to the energy?

Answer 12

When bonds break, energy must be absorbed from the
surroundings in order to separate atoms that are held together

Question 13

What kind of reaction is the breakage of bonds

Answer 13

Endothermic

Question 14

When bonds form, energy is released into the surroundings, what happens to the surroundings

Answer 14

The surroundings heat up

Question 15

When bonds break, energy must be absorbed from the
surroundings

Answer 15

The surroundings cool down

Question 16

What kind of reaction is the formation of bonds

Answer 16

Exothermic

Question 17

Energy involved in creating a solution

Answer 17

1.Bonds break within the substance dissociated or ionized

2.Energy ireleased when bonds between water molecules and the separated ion form

Question 18

Concentration

Answer 18

the ratio of the quantity of the solute to the quantity of the solution.

concentration = quantity of solute/quantity of solution

Question 19

Dilute solution

Answer 19

relatively small quantity of solute when compared to the volume of solution

Question 20

Concentrated solution

Answer 20

relatively large quantity of solute when compared to the volume of solution

Question 21

How can concentration be expressed

Answer 21

Percentage by volume (%V/V)
Percentage weight by volume (%W/V)
Percentage weight by weight (%W/W)
Parts per million concentration (PPM)
Amount concentration (molarity)

Question 22

When do we use PPM

Answer 22

We use ppm to
report these very small concentrations.
e.g:For example 11 ppm of chlorine in pool water means there is 11 mg of
chlorine in every liter of pool water.

Question 23

Amount Concentration

Answer 23

the number of moles of solute dissolved in one liter of solution.

Question 24

Amount

Answer 24

the number of moles of a substance
Does not refer to mass or volume of a substance

Question 25

Amount Concentration formula

Answer 25

c=n/v

Question 26

Unit for Amount Concentration

Answer 26

mol/L

Question 27

Saturated solution

Answer 27

Saturated solution

Question 28

Solubility

Answer 28

concentration of a saturated solution

Question 29

Solids

Answer 29

Solid solutes have higher solubility in water at higher temperatures

Question 30

Gases

Answer 30

Gases have higher solubility at lower temps Gases have higher solubility at higher pressures

Question 31

Liquids

Answer 31

Difficult to make generalizations for liquid solutes Liquids that mix with water are called miscible Liquids that don’t mix with water are considered immiscible

Question 32

Elements

Answer 32

Elements have low solubility in water

Question 33

What are two key things to remember about solubility

Answer 33

Units for solubility can be the same as the ones for concentration Every solubility must be accompanied by a temperature value because solubility changes with temperature

Question 34

When an ionic compound is in solution, it

Answer 34

dissociates into its ions.

Question 35

In many industries it is important to know the what of the individual ions and not the compound

Answer 35

concentration

Question 36

How do we determine concentrations in ion solutions

Answer 36

we use the dissociation/ionization equations

Question 37

What is a key thing to remember about ion concentration

Answer 37

Ion concentration is always equal to a whole number multiple of the compound concentration.

Question 38

A solution that has a known, accurate concentration is a

Answer 38

standard solution.

Question 39

There are 2 ways to create a standard solution

Answer 39

By dissolving a solid By diluting a more concentrated solution

Question 40

Preparing a standard solution from a solid

Answer 40

Step 1: Calculate what mass of solid is needed to make the required volume and concentration of solution n = cv m = nM Step 2: Measure out the mass of solid using an electronic scale Step 3: Dissolve the solid in half of the required volume of water Step 4: Transfer dissolved solid into a volumetric flask (make sure the volumetric flask is the size needed) Step 5: Fill the volumetric flask to the marking for the volume of the solution needed Step 6: Place top on volumetric flask and invert to mix.

Question 41

Preparing a standard solution by dilution

Answer 41

A stock solution is an initial, usually concentrated, solution from which samples are taken for a dilution. We can prepare solutions by diluting an existing solution to a desired concentration. Formula: C1 = initial concentration C2 = final concentration V1 = initial volume V2 = final volume

Question 42

Entropy

Answer 42

disorder

Question 43

Solution

Answer 43

A _homeogenous_________ mixture composed of at least one solvent and one solute

Question 44

Solvent

Answer 44

the thing that does the dissolving____

Question 45

Aqueous Solutions can be - Classified as

Answer 45

1. _____unsaturated ________ or ____saturated_________ 2. Acid, Base, or ___netural_______ solutions

Question 46

Molecular compounds are

Answer 46

nonelectrolytes

Question 47

What are some strong electrolytes

Answer 47

HCI,NaOH,KOH

Question 48

What are some examples of electrolytes

Answer 48

Calcium, Chloride, Magnesium, Phosphorus, Potassium, Sodium

Question 49

What are some non electrolytes

Answer 49

Glucose, Sucrose, Ethanol.