week 11

Question 1

insoluble - concentrations

Answer 1

will be very small

equilibrium positioned on left hand side

Question 2

solubility product

Answer 2

is the equilbrium constant of a ionic compound

Question 3

lower the solubility constant

Answer 3

less soluble the salt

Question 4

ksp < 10^-5

Answer 4

low solubility

Question 5

dissolution

Answer 5

when a solid compound is embedded is embedded in a matrix of solvent

Question 6

dissociation

Answer 6

when an electrolyte is disassembled to form individual ions

Question 7

solubility

Answer 7

m (solute) / v (solution)

Question 8

molar solubility

Answer 8

Nsat(solute)/ V (solution)

Question 9

solubility

Answer 9

the amount of solute that is required to yield a saturated solution

Question 10

molar solubility in Ksp

Answer 10

can be used assuming that all the salt dissociates

Question 11

ionic product

Answer 11

Qsp
calculate the same way as Ksp
values of molar concentrations used are the actual concentrations given

Question 12

Qsp > Ksp

Answer 12

a precipitate is formed

Question 13

Qsp < Ksp

Answer 13

no precipitate is formed

Question 14

common ion effect

Answer 14

any ionic salt is less soluble in the presence of a common ion

Question 15

solution

Answer 15

homogenous mixture of two or more pure substances

Question 16

solvent

Answer 16

liquid of a liquid solution

Question 17

solute

Answer 17

dissolved substance in liquid solution

Question 18

dissolution

Answer 18

process of dissolving a solute in a solvent to give a homogenous solution

Question 19

saturated solution

Answer 19

solution in which no more solute will dissolve

Question 20

gas mixing

Answer 20

mixes completely with other gases

mix spontaneously

Question 21

alpha mix of G

Answer 21

the mixing process constant

negative

Question 22

two gases mix

Answer 22

enthalpy change is small

intermolecular forces are tiny and gas molecules are far apart

Question 23

mixing gases

Answer 23

large increase in entropy so there is negative delta mix G

Question 24

gas mixing process

Answer 24

spontaneous

entropy driven

Question 25

gas liquid solutions

Answer 25

intermoleculare forces between solvent arent negligible

Question 26

non polar solvents

Answer 26

delta H of solution >0

Question 27

polar solvents with H bonding

Answer 27

delta H of solution < 0

Question 28

gas liquid - temp

Answer 28

varies with temp and

less soluble as temp increases

Question 29

gas liquid - pressure

Answer 29

varies with pressure

more soluble as pressure increases

Question 30

Henry’s Law

Answer 30

concentration of a gas dissolved in a liquid at a particular temperature is proportional to the partial pressure of a gas

Question 31

molar concentration of gas

Answer 31

KH x Pgas at constant T

where pgas is partial pressure of gas and KH is the henry’s law constant

Question 32

miscible

Answer 32

liquid mix completely in all proportions

Question 33

immiscible

Answer 33

liquids form 2 layers upon addition of one to the other

Question 34

like dissolves like rule

Answer 34

two liquids with similar polarities tend to be miscible

polar solute dissolves in polar solvent

Question 35

solvation

Answer 35

state where solute molecules are surrounded by solvent molecules

Question 36

Hydration

Answer 36

when solutes becomes surrounded by water molecules

Question 37

molar lattice enthalpy

Answer 37

enthaply required to transform 1 mol of crystalline substance to gaseous particles

Question 38

molar solvation (hydration) enthalpy

Answer 38

enthalpy change when 1 mol of gaseous particles are hydrated

Question 39

molar enthalpy of solution

Answer 39

enthalpy change when 1 mol of crystalline particles are hydrated
molar lattice enthalpy + molar solvation enthalpy

Question 40

liquid to solid enthalpy of solution

Answer 40

calculated by a 2 step model of lattice vapourisation and solvation