Exam 2 ch 13 Flashcards
(18 cards)
Solute
-Being dissolved
-Smaller
Solvent
-Dissolving in
-Larger
Why will chemicals dissolve in other chemicals
-Intermolecular interactions
Solutions that can be formed
-Solid in liquid
-Liquid in liquid (ethonol/water)
-Solid in solid (Metals -Au/Ag)
Intermolecular interactions
-H bonding
-Ion-dipole
-dipole-dipole
-dipole induced dipole
-dispersion
Role of intermolecular interactions
-Same intermolecular interaction means it can dissolve
Dissolution process and enthalpy diagrams
-Solute/solute breaks
-Solvent/solvent breaks
-Solute/solvent forms
Molarity
Moles solute/L solution
M
Molality
Moles solute/kilograms solvent
m
Mole fraction
Moles solute/Total moles in solution
no unit
Mass %
Mass solute / mass solution
Volume %
Volume solute / volume of solution
ppm
mass solute/mass solution *10^6
For every 1 million parts of solvent theres __ solute
Enthalpy diagram exothermic
solute-solute increases energy
solvent-solvent increases energy
solute-solvent decreases energy below starting value
delta H is -
Enthalp diagram endothermic
solute-solute increases energy
solvent-solvent increases energy
solute-solvent decreases energy less then starting value
delt H is postive
Solubilitiy of gases and temp
-Decreases as temp increases
-Solids normally increase but not predictable
Effect of pressure on solubility
-No effect on solids and liquids
-Big effect on gases
-More gas you put above a liquid, the more it dissolves
Henrys law
Solubility = K * P
K = contant specific to each gas
P = pressure of the gas above the liquid
-As press increases, more gas enters solution
-As press decreases, more gas leaves solution
-bigger k means less soluble
