Chapter 0g: Solutions

Question 1

• homogeneous mixtures of two or more substances
• form when there is sufficient attraction between the solute and solvent molecules

Answer 1

solutions

Question 2

two components of solutions

Answer 2

1. solvent
2. solute

Question 3

present in larger amount

Answer 3

solvent

Question 4

present in smaller amount

Answer 4

solute

Question 5

Solutes and solvents may be… ?

Answer 5

• liquid
• gas
• solid

Question 6

solutes are mixed with solvents so that they have the same __ __

Answer 6

physical state

Question 7

solutes in a solution cannot be separated by __, but can be separated by __

Answer 7

• filtration
• evaporation

Question 8

• one of the most common solvents in nature
• polar molecule due to polar O-H bonds
• molecules form hydrogen bonds

Answer 8

water

Question 9

what type of molecule is water

Answer 9

polar molecule (O-H bonds)

Question 10

How are solutions formed

Answer 10

solute-solvent interactions are large enough to overcome solute-solute interactions and solvent-solvent interactions

Question 11

what dissolves what

Answer 11

like dissolves like
(polar - polar)
(nonpolar - nonpolar)

Question 12

ex. of nonpolar molecules

Answer 12

1. iodine
2. oil
3. grease

Question 13

play an important role in maintaining proper function of cells and organs

Answer 13

electrolytes

Question 14

Types of electrolytes

Answer 14

1. strong electrolytes
2. weak electrolytes
3. nonelectrolytes

Question 15

• dissociate 100% in water
• produce positive and negative ions
• form solutions that conduct an electric current strong enough to light a bulb

Answer 15

strong electrolytes

Question 16

• dissociates only slightly in water
• forms a solution with a few ions and mostly undissociated molecules

Answer 16

weak electrolytes

Question 17

• dissolve as molecules in water
• do not produce ions in water
• do not conduct an electric current

Answer 17

nonelectrolytes

Question 18

Ex. of strong electrolyte formula

Answer 18

NaCl(s) –> Na+(aq) + Cl-(aq)

Question 19

Ex. of weak electrolyte formula

Answer 19

HF(aq) <–> H+(aq) + F-(aq)

Question 20

Ex. of nonelectrolyte formula

Answer 20

C12H22O11(s) –> C12H22O11(aq)

Question 21

Examples of strong electrolytes

Answer 21

• ionic compounds
• acids such as HCl, HBr, HI, HNO3, HClO4, H2SO4

Question 22

Examples of weak electrolytes

Answer 22

• HF
• H2O
• NH3
• HC2H3O2 (acetic acid)

Question 23

Examples of nonelectrolytes

Answer 23

carbon compounds
- methanol (CH3OH)
- ethanol (C2H5OH)
- sucrose (C12H22O11)
- urea (CH4N2O)

Question 24

amount of an electrolyte or an ion that provides 1 mole of electrical charge

Answer 24

equivalent (Eq)

Question 25

In solution, the charge of positive and negative ions are always __

Answer 25

balanced

Question 26

electrolytes in intravenous fluids are expressed in __

Answer 26

mEq/L

Question 27

maximum amount of solute that dissolves in a specific amount of solvent

Answer 27

solubility

Question 28

how is solubility expressed

Answer 28

g of solute / 100 g water

Question 29

Two types of solution

Answer 29

1. unsaturated solution 2. saturated solution

Question 30

- contain less than the maximum amount of solute - can dissolve more solute

Answer 30

unsaturated solutions

Question 31

- contain the maximum amount of solute that can dissolve - have undissolved solute at the bottom of the container - contain solute that dissolves as well as solute that recrystallizes in an equilibrium process

Answer 31

saturated solutions

Question 32

saturated solution formula

Answer 32

solute + solvent --> (solute dissolves) (solute recrystallizes) <-- saturated solution

Question 33

where does solubility depend

Answer 33

temperature

Question 34

solubility of solids: temperature increases

Answer 34

more soluble

Question 35

solubility of gases: temperature increases

Answer 35

less soluble

Question 36

- states that the solubility of a gas in a liquid is directly related to the pressure of that gas above the liquid - at higher pressures, more gas molecules dissolve in the liquid

Answer 36

Henry's law

Question 37

when the pressure of a gas above a solution decreases, what happens to the solubility of that gas in the solution

Answer 37

also decreases

Question 38

How are ionic compounds soluble in water

Answer 38

if they contain soluble cation or anion

Question 39

Soluble in Water: Positive ions

Answer 39

1. Li+ 2. Na+ 3. K+ 4. Rb+ 5. Cs+ 6. NH4+

Question 40

Soluble in Water: Negative ions

Answer 40

1. NO3 - 2. C2H3O2 - 3. Cl - 4. Br - 5. I - 6. SO4 2-

Question 41

Cl-, Br-, I- are insoluble when combined with...?

Answer 41

1. Ag+ 2. Pb 2+ 3. Hg2 2+

Question 42

SO4 2- is insoluble when combined with...?

Answer 42

1. Ba 2+ 2. Pb 2+ 3. Ca 2+ 4. Sr 2+ 5. Hg2 2+

Question 43

Ionic compounds that do not contai at least one of the soluble ions are usually __

Answer 43

insoluble

Question 44

used to enhance x-rays

Answer 44

BaSO4

Question 45

mass percent (m/m)

Answer 45

g/g

Question 46

volume percent (v/v)

Answer 46

mL/mL

Question 47

mass/volume percent (m/v)

Answer 47

g/mL

Question 48

When writing a net ionic equation, what is removed

Answer 48

spectator ions

Question 49

ions which do not participate in chemical reactions and present the same on both sides of the reactions

Answer 49

spectator ions

Question 50

a solvent, usually water, is added to a solution, which increases its volume and decreases the concentration of the solution

Answer 50

dilution

Question 51

what is added in a dilution

Answer 51

water

Question 52

what is the same in the initial and diluted solution

Answer 52

moles of solute

Question 53

equation that relate concentration and volumes

Answer 53

C1V1 = C2V2

Question 54

concentration, C, may be __ or __

Answer 54

- percent concentration - molarity

Question 55

Freezing point depression of water

Answer 55

1.86°C kg/mol

Question 56

Boiling point elevation of water

Answer 56

0.515°C kg/mol