The experimenter uses 1.1059 g of oxalic acid to prepare the primary standard solution
Answers
The neutralisation reaction between an acid and a base can be very useful. If an acidic solution of known concentration (a standard solution) is added to a basic (alkaline) solution of unknown concentration until the solution is exactly neutralised (i.e. there is only salt and water), it is possible to calculate the exact concentration of the unknown solution. It is possible to do this because, at the exact point where the solution is neutralised, stoichiometrically equivalent mole amounts of acid and base have reacted with each other.concentration of a solution is measured in mol.dm−3mol.dm−3
moles (mol) == concentration (mol⋅dm−3mol·dm−3) ××volume (dm3dm3)
concentration =molesvolumeC(mol⋅dm−3)=n(mol)V(dm3)concentration =molesvolumeC(mol·dm−3)=n(mol)V(dm3)
remember to make sure all the units are correct in your calculations
Make sure that the equation is balanced
There are equal numbers of each type of atom on each side of the equation, so the equation is balanced.
Write down all the information you know about the reaction, converting to the correct units
NaOH: V = 2525 cm3cm3 ×0,001 dm31 cm3×0,001 dm31 cm3 = 0,0250,025 dm3dm3
HCl: V = 1515 cm3cm3 ×0,001 dm31 cm3×0,001 dm31 cm3 = 0,0150,015 dm3dm3
C = 0,20,2 mol.dm−3