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12 Cards in this Set

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MOLES
the unit for amountof substance. one mole of ion,atom or molecule is around 6 × 1023, same number of carbon. Shown as mol

RELATIVE ATOMIC MASS


(AR)

the average mass of one atom of an element to 1/12 of the mass of an atom of carbon-12
MOLAR MASS
the relative formula mass of a substance in grams (measured in g/mol).
EMPIRICAL FORMULA
of a compound is the simplest whole number ratio of each type of atom in a compound. It can be the same as the compound’s molecular formula - but not always.
VOLUME

measured in cubic centimetres, cm3, or in cubic decimetres, dm3.


1000 cm3 = 1 dm3




cm3 to dm3 … divide by 1000


dm3 to cm3 … multiply by 1000

CONCENTRATION

amount of solute per volume of solvent


The more concentrated a solution is, the more solute particles there are in a given volume of solution.


commonly measured in g/dm3 or in mol/dm3.

PH CURVES

A graph of pH (on the vertical axis) against total volume of acid or alkali added (on the horizontal axis)

TITRE
The difference between the reading at the start and the final reading gives the volume of acid (or alkali) added.

LIMITING REACTANT


REACTANT IN EXCESS

the limiting reactant is the one that is all used up at the end of the reaction




the reactant in excess is still there at the end of the reaction (although in a smaller amount than at the start)

how the volume of gas in dm3 at rtp is related to the number of moles?
volume of gas at rtp = number of moles × 24
EQUILIBRUM
the condition existing when a chemical reaction and its reverse reaction proceed at equal rates.

is an ion that is present in reactant and a product in a chemical equation but does not take part in the reaction