solutions

Question 1

solute

Answer 1

dissolved in solvent

Question 2

factors that determine rate with solute dissolves

Answer 2

agitation, temperature, particle size of solute

Question 3

moles —–> grams

Answer 3

multiply by molar mass

Question 4

grams —–> moles

Answer 4

divide by molar mass

Question 5

mole fraction

Answer 5

mole of component/total moles

Question 6

unsaturated

Answer 6

contains LESS than maximum amount of solute at a given temp

Question 7

saturated

Answer 7

contains maximum amount of solute at a given temp

Question 8

super-saturated

Answer 8

contains MORE than maximum amount of solute at given temp

Question 9

dilution equation

Answer 9

M1V1=M2V2

Question 10

percent solution equation (v/v)

Answer 10

(volume solute/volume solution) x 100

Question 11

percent solution equation (m/m)

Answer 11

(mass solute/mass solution) x 100

Question 12

colligative properties

Answer 12

-vapor pressure depression
-freezing point depression
-boiling point elevation
-osmosis

Question 13

vapor pressure depression

Answer 13

more solute, lower vapor pressure

Question 14

freezing point depression

Answer 14

more solute, lower freezing point

Question 15

boiling point elevation

Answer 15

more solute, higher boiling point

Question 16

osmosis

Answer 16

the movement of solvent towards the solution with a higher concentation of solute

Question 17

colligative properties (pt.2)

Answer 17

colligative properties are based on number of solute particles, NOT type.

Question 18

solute particles can be…

Answer 18

…atoms, ions, or molecules

Question 19

ionic compounds _______ break into ions when dissolved in water

Answer 19

will

Question 20

henrys law

Answer 20

Sg = k * Pg

Sg= solubility of gas (aka molarity)
k= henry’s law constant ([mol *L]/atm)
Pg= partial pressure of gas (atm)

Question 21

freezing point depression

Answer 21

Tf=Kf*m

Question 22

boiling point elevation

Answer 22

Tb=Kb*m

Question 23

Molarity def

Answer 23

number of moles of solute dissolved in 1 liter of solution

Question 24

Molality

Answer 24

moles of solute/ kilograms of solvent

Question 25

when will you use effective molality? (multiply number of particles by molality)

Answer 25

In a freezing point/boiling point problem, and the solute is ionic.

Question 26

ionic def

Answer 26

metal+nonmetal

Question 27

another way to write henry’s law

Answer 27

S1/P1=S2/P2

Question 28

what information will a henry’s law problem provide?

Answer 28

-solubility (measured in Molarity)
-henry’s law constant
-partial pressure of gas(es)

Question 29

what information will a freezing point depression/boiling point elevation provide?

Answer 29

-the mass of solute
-mass of solvent
-specific point of solvent
-specific point constant
-change in specific point

Question 30

miscible

Answer 30

WILL disolve

Question 31

immiscibile

Answer 31

will NOT dissolve

Question 32

sitrring/agitation does what to a solution?

Answer 32

accelerates speed of dissolution by bringing it into contact with all of the solvent particles

Question 33

temperature does what to a solution?

Answer 33

causes the particles to move faster so they dissolve quicker

Question 34

particle size does what to a solution?

Answer 34

smaller the particles, the more surface area the solvent can dissolve because dissolution only occurs on the surface of the particle.

Question 35

molarity equation

Answer 35

M=moles of solute/liters of solution

Question 36

When not given the amount (in grams) of solution, what do you assume it is?

Answer 36

100 grams