Solubility
A measure of the maximum amount of solute that can dissolve per amount of solvent under specified conditions of temperature and pressure
Henry’s Law
At a fixed temperature the amount of a given gas that dissolves in a given liquid is directly proportional to the partial pressure of that gas in equilibrium with that liquid
gas comes out of solution when pressure reduces through effervescent bubbles (think opening fizzy drink can)
Mixture
2+ substances dispersed through eachother but retain their original identity
Do NOT combine chemically (non-homogenous)
eg flour & water
Suspension
Mixtures which eventually separate out over a varying amount of time
eg mud & water
Colloid
Mixture where a substance is dispersed evenly through another.
Does NOT settle under influence of gravity.
Internal phase: dispersed substance of small diameter particles
External phase: in which the internal phase is dispersed
eg smoke in air
Emulsions
Colloid mixture of two or more immiscible liquids
Raoult’s Law
The overall vapour pressure of a solution depends on the vapour pressure of each component in solution
Solution
A homogenous mix of two or more substances
Osmosis
A physical process by which a solvent (liquid) moves across a semi-permeable membrane, from a hypOtonic solution to a hypERtonic solution
hypOtonic = lots of water, little salt
hypERtonic = lots of salt, little water
Moves from dilute to concentrated solution
Osmotic pressure
The hydrostatic pressure exerted within a container of solution separated by a semi-permeable membrane
Osmole
The number of moles of a compound contributing to the total osmotic pressure
Diffusion
The process by which there is movement of a substance from an area of high concentration of that substance to an area of lower concentration
Specific heat capacity
Amount of heat energy required to raise the temperature of 1kg of a substance by 1K
Pascals principle
Pressure is transmitted equally and undiminished through a compressed fluid
Isomerism
Existence of two or more substances composed of the same atoms in the same proportions but with variations in the arrangements of the atoms
Mechanical equivalent of heat
Mechanical work may be transformed into heat, and conversely heat into work, the magnitude of one always proportional to the other
Zeroth Law of Thermodynamics
If two thermodynamic systems are separately in equilibrium with a third system, they must also be in equilibrium with eachother
First Law of Thermodynamics
Energy can neither be created nor destroyed
Second Law of Thermodynamics
Entropy tends to increase with time
(entropy = measure of disorganisation or chaos)
Can also be thought of as a measure of unavailable energy
Third Law of Thermodynamics
As a system approaches absolute zero, all processes cease and the entropy of the system approaches a minimum value
Capacitance
The ability of an object to store electrical charge
Measured in farads (F)
Radioactive decay
Process where an unstable nucleus loses energy by emitting radiation (alpha, beta, gamma)
