Chapter G: Solutions

Question 1

• may be a liquid, gas, or solid.
• are spread evenly throughout the solution
• mix with solvents so the solute and solvent have the same physical state.
• cannot be separated by filtration, but they can be separated by evaporation.
• are not visible, but they can give a color to the solution

Answer 1

Solutes

Question 2

Solutes cannot be separated by ____, but they can separated by ____.

Answer 2

• Filtration
• Evaporation

Question 3

• is one of the most common solvents in nature.
• is a polar molecule due to polar O–H bonds.
• molecules form hydrogen bonds important in many biological compounds.

Answer 3

Water

Question 4

How does solutions form?

Answer 4

When solute-solvent interactions are lare enough to overcome solute-solute and solvent-solvent interactions

Question 5

Solute: Polar

Answer 5

Solvent: polar

Question 6

Solute: non polar

Answer 6

Solvent: nonpolar

Question 7

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

Answer 7

Electrolytes

Question 8

Examples of Electrolytes

Answer 8

Sodium, Potassium, Chloride, Bicarbonate

Question 9

dissociate 100% in water, producing positive and negative ions

Answer 9

Strong electrolytes

Question 10

form solutions that conduct an electric current strong enough to light a bulb.

Answer 10

Strong electrolytes

Question 11

dissociates only slightly in water.

Answer 11

Weak electrolyte

Question 12

forms a solution with a few ions and mostly undissociated molecules

Answer 12

Weak electrolyte

Question 13

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

Answer 13

Nonelectrolytes

Question 14

Examples of Strong electrolyte

Answer 14

Ionic compounds such as;
- NaCl, KBr, MgCl2, Nano3-
Bases such as:
- NaOh, KOH
Acids such as:
- HCl, HBr, HI, HNO3, HClO4 H2SO4

Question 15

Examples of Weak electrolyte

Answer 15

HF, H2O, NH3, acetic acid

Question 16

Examples of Nonelectrolytes

Answer 16

Carbon compounds such as Methanol, Ethanol, Sucrose, Urea

Question 17

NaCl

Answer 17

Strong electrolyte

Question 18

KBr

Answer 18

Strong electrolyte

Question 19

MgCl2

Answer 19

Strong electrolyte

Question 20

NaNO3

Answer 20

Strong electrolyte

Question 21

NaOH

Answer 21

Strong electrolyte

Question 22

KOH

Answer 22

Strong electrolyte

Question 23

HCl

Answer 23

Strong electrolyte

Question 24

HBr

Answer 24

Strong electrolyte

Question 25

HI

Answer 25

Strong electrolyte

Question 26

HNO3

Answer 26

Strong electrolyte

Question 27

HClO4

Answer 27

Strong electrolyte

Question 28

H2SO4

Answer 28

Strong electrolyte

Question 29

HF

Answer 29

Weak Electrolyte

Question 30

H2O

Answer 30

Weak Electrolyte

Question 31

NH3

Answer 31

Weak Electrolyte

Question 32

HC2H3O2(Acetic acid)

Answer 32

Weak Electrolyte

Question 33

CH3OH (methanol

Answer 33

Nonelectrolyte

Question 34

C2H5OH(ethanol)

Answer 34

Nonelectrolyte

Question 35

C12H22O11(Sucrose)

Answer 35

Nonelectrolyte

Question 36

CH4N2O (urea)

Answer 36

Nonelectrolyte

Question 37

Types of particles in solution: Strong electrolyte

Answer 37

Ions Only

Question 38

Types of Particles in solution: weak electrolyte

Answer 38

Mostly molecules and a few ideas

Question 39

Types of particles in Solution: nonelectrolyte

Answer 39

Molecules Only

Question 40

is the amount of an electrolyte or an ion that provides 1 mole of electrical charge (+ or −)

Answer 40

Equivalent (Eq)

Question 41

1Eq = ?

Answer 41

1000 mEq

Question 42

* contain less than the maximum amount of solute. * can dissolve more solute.

Answer 42

Unsaturated solutions

Question 43

* contain the maximum amount of solute that can dissolve. * have undissolved solute at the bottom of the container.

Answer 43

Saturated Solutions

Question 44

Effect of temperature on solubility

Answer 44

- Solubility of solids increase as temperature increase - Solubility of gases decreases as temperature increase

Question 45

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 45

Henry's Law

Question 46

Henry's Law: * the solubility of a gas in a liquid is directly ____ to the ____ of that gas above the ____.

Answer 46

- related - pressure - liquid

Question 47

Henry's Law: * at ____ ____, more gas molecules dissolve in the _____.

Answer 47

- higher pressures - liquid

Question 48

Soluble ionic compounds

Answer 48

Sulfates, (SO4^2-) are soluble unless combines with - Ba2+, - Pb2+, - Ca2+, - Sr2+, - Hg2^2+

Question 49

an insoluble ionic compound, is used to enhance X-rays

Answer 49

Barium Sulfate (BaSO4)

Question 50

an insoluble solid that emerges from a liquid solution

Answer 50

precipitate

Question 51

- Water is added - the volume of the solution increases - concentration decreases

Answer 51

Dilution

Question 52

Formula for concentrations and volumes are related

Answer 52

C1V1=C2V2

Question 53

- When water is added to the concentrated solution, there is no change in number of particles. - The solute particles spread as the volume of the solution increases

Answer 53

Dilution of a Solution