The Molecular Formula of Succinic Acid
The relative formula mass is the mass of 1 molecule of succinic acid
compared with 1/12th of the mass of an atom of carbon-12. This is
obtained by adding together the relative atomic masses of the atoms
within the molecule according to its written formula. However we do
not know the exact formula:
HOOC(CH )nCOOH Where n is a whole number
between 1 and 4
So to calculate the relative formula mass I must use the formula m = n
×Mr and rearrange it to make Mr the subject Mr = m
n
However I do not know the number of moles for a given mass. I can
calculate this by preparing a standard solution of the acid and
performing a titration experiment.
Firstly I would like to calculate a likely value of the relative
formula mass given the information above.
Suppose n = 3 then HOOC(CH ) COOH and Mr = 1+(2 x
16)+12+(3x12)+(3x2)+12+(2x16)+1
= 132
To perform the titration I have chosen to use equal concentrations of
acid and alkali at 0.1mols/dm³. This is a low concentration as the
more concentrated the solution, the more rapidly the reaction takes
place. This can be explained by the collision theory as increasing the
concentration of the reactants increases the number of particles
resulting in an increased number of collisions. If the reaction takes
place too rapidly then it will be difficult to identify the exact
point at which the alkali is neutralised and the results will become
less accurate.
To prepare my acid solution I must dissolve an accurately weighed
amount of anhydrous succinic acid to 250cm³/0.25dm³ of water to
achieve a concentration of 0.1mols/dm³. What mass of acid is required
to achieve this concentration?
m= 10km2 x 1000m x 1000m = 107m2 107m2 x 15= 1.5 x 1.8m3 = 1.5 x 1011kg
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