Solutions

Front 1

Nitrite

Back 1

NO2-

Front 2

Nitrate

Back 2

NO3-

Front 3

Sulfite

Back 3

(SO3)2-

Front 4

Sulfate

Back 4

(SO4)2-

Front 5

Hypochlorite

Back 5

ClO-

Front 6

Chlorite

Back 6

ClO3-

Front 7

Perchlorate

Back 7

ClO4-

Front 8

Carbonate

Back 8

(CO3)2-

Front 9

Bicarbonate

Back 9

(HCO3)-

Front 10

Phosphate

Back 10

(PO4)3-

Front 11

Group 1 salts

Back 11

Soluble

Front 12

Li+

Back 12

soluble

Front 13

Na+

Back 13

soluble

Front 14

K+

Back 14

soluble

Front 15

Rb+

Back 15

soluble

Front 16

Cs+

Back 16

soluble

Front 17

NO3- salts

Back 17

soluble

Front 18

(ClO4)- salts

Back 18

soluble

Front 19

(C2H3O2)- salts (acetate)

Back 19

soluble

Front 20

Ag+

Back 20

insoluble except for nitrates, perchlorates and acetates

Front 21

Pb2+/Pb4+

Back 21

insoluble except for nitrates, perchlorates, and aceates

Front 22

why is molality used in freezing point and boiling point calculations

Back 22

molality (moles of solute/kg of soln) does not change with temperature while molarity does

Front 23

colligative properties depend upon...

Back 23

number, not kind

Front 24

What are the colligative properties?

Back 24

1. boiling point elevation
2. freezing point depression
3. vapor pressure lowering
4. osmotic pressure

Front 25

molarity

Back 25

mols of solute/liters of solution

Front 26

molality

Back 26

mols of solute/kg of solvent

Front 27

mass of 1 Liter of water

Back 27

1 kg, thus molar and molal concentrations of dilute aqueous solutions are nearly the same

Front 28

van't Hoff factor (i)

Back 28

how many ions one unit of a substance will produce in a solution
NaCL -> Na+, Cl- i=2
CaCl2 -> Ca+, 2Cl- i=3

Front 29

when ionic substances dissolve they...

Back 29

dissociate into ions. Free ions are electolytes

Front 30

NH4+

Back 30

soluble

Front 31

group 1, ammonium, nitrate, perchlorate, and acetate
salts

Back 31

soluble

Front 32

Ag+, Pb+, Pb4+, (Hg2)2+, Hg2+
except when with acetate (C2H3O2)-, nitrate (NO3)-, perchlorate (ClO4)-

Back 32

insoluble

Front 33

How does solubility of solids in liquids respond to increasting temperature

Back 33

solubility increases (generally)

Front 34

Solubility of gases increases with

Back 34

increasing pressure, and decreasing temperature

Front 35

vapor pressure

Back 35

pressure exerted by the gaseous phase of a liquid that evaporated from the exposed surface of the liquid

Front 36

boiling point

Back 36

when atmospheric pressure equals vapor pressure

Front 37

vapor pressure depression

Back 37

added solute particles act as anchors to solvent molecules thus it makes them harder to enter the gas phase and thus the vapor pressure is lowered.
This means that the temperature will have to be increased to induce boiling

Front 38

partial pressure (Raoult's Law)

Back 38

the partial pressure of A is equal to its mol fraction (X) in the solution

Front 39

NH4+

Back 39

soluble

Front 40

group 1, ammonium, nitrate, perchlorate, and acetate
salts

Back 40

soluble

Front 41

Ag+, Pb+, Pb4+, (Hg2)2+, Hg2+
except when with acetate (C2H3O2)-, nitrate (NO3)-, perchlorate (ClO4)-

Back 41

insoluble

Front 42

How does solubility of solids in liquids respond to increasting temperature

Back 42

solubility increases (generally)

Front 43

Solubility of gases increases with

Back 43

increasing pressure, and decreasing temperature

Front 44

if intermolecular forces between two liquids (A and B) are weaker than those between A-A or B-B how will the solution deviate from Raoult's Law

Back 44

if the intermolecular forces are lower then their partial vapor pressures will be higher than predicted by Raoult's law. Opposite is true if A-B > A-A or B-B

Front 45

Vapor Pressure Depression

Back 45

Equation

Front 46

What happens to the boiling point when a non-volatile solute is added to solution

Back 46

it is elevated

solute anchors solvent particles and makes it harder for them to leave as gas-which lowers vapor pressure and thus more heat is needed for vap pressure to equal atmospheric pressure

Front 47

boiling pt. elevation equation

Back 47

eqn

Front 48

what happens if you add a volatile solute

Back 48

volatile solutes can increase vapor pressure and thus make the boiliong point go down

Front 49

What is more accurate for solvent in ideally dilute solution-Henry or Raoult's Law?

Back 49

raoult's law, solvent vapor partial pressure=mol fraction * vapor pressure as a pure liquid
each solvent surrounded by other solvent= pure liquid

Front 50

how does size affect gas solubility

Back 50

heavier, larger gases experience greater van Der Waals forces so they tend to be more soluble

Front 51

What will the affect be of adding a common ion to a SATURATED solution?

Back 51

It will shift equilibrium increasing precipitate. It DOES NOT affect Ksp

Front 52

What will the affect be of adding a common ion to an UNSATURATED solution?

Back 52

it will not shift the equilibrium because there is no equilibrium to shift