solutions and their behavior

Question 1

a homogeneous mixture that consists of one or more solutes uniformly dispersed at the molecular or ionic level throughout a medium known as the solvent

Answer 1

solution

Question 2

solvent

Answer 2

the larger amt

Question 3

solute

Answer 3

the smaller amt

Question 4

molality (m) deals with

Answer 4

kg solvent

Question 5

molarity (M) deals with

Answer 5

L solution

Question 6

what does it mean if something is saturated

Answer 6

contains the max amt of solute, as defined by its solubility

Question 7

supersaturated

Answer 7

a solution contains more solute than allowed by the solubility

Question 8

clinical application for saturated

Answer 8

when gases reach equilibrium

Question 9

miscible

Answer 9

two liquids are miscible if they are soluble in each other in all proportions

Question 10

lattice energy (LE)

Answer 10

the energy released when molecules or ions settle into a crystalline lattice. it is inherently exothermic

Question 11

solvation (hydration) energy (SE)

Answer 11

the energy released when an ion (or molecules) settles into a sphere of solvent molecules

Question 12

solvation is inherently

Answer 12

exothermic

Question 13

henrys law

Answer 13

pressure increases, solubility increases. “the amt of nonreacting gas which dissolves in liquid is directly proportional to the partial pressure of the gas, provided the temp remains constant.

Question 14

as temp increases, solubility

Answer 14

decreases

Question 15

in liquid and solid solutes, pressure has ___ effect on solubility

Answer 15

negligible

Question 16

in liquid and solid solutes as T increases, solubility

Answer 16

increases

Question 17

the amt of gas dissolved is ___ proportional to the temp

Answer 17

inversely

Question 18

the colder the liquid, the __ gas that will dissolve in the liquid

Answer 18

more

Question 19

henry’s law applied to patient

Answer 19

temp has an affect on the amt of gas taken up by the body and how long it takes to wake them back up, particularly if they are cold.

Question 20

colligative properties of solutions

Answer 20

depends only on the number of solute particles, not the identity of the solute particles

Question 21

examples of colligative properties

Answer 21

vapor pressure decreasing, boiling point elevation, freezing point depression, osmotic pressure increase

Question 22

raoult’s law describes

Answer 22

vapor pressure of a solution

Question 23

as vapor pressure goes down, boiling point goes

Answer 23

up

Question 24

freezing point depression

Answer 24

lowers the temp at which water freezes (like why we use salt for ice cream or on ice on the roads)

Question 25

osmosis

Answer 25

diffusion of water through a semipermeable membrane

Question 26

osmotic pressure results from

Answer 26

the potential drive for the concentration of water to equalize.

Question 27

colloids

Answer 27

not true solutions. large particle size. colloidal particles cannot be filtered and do not settle out of solution.