4.2 acid-base titrations Flashcards
what is a standard solution
is a solution of known concentration
what do we use to make a standard solution accurately
a volumetric flask (either 250cm3 or 100cm3)
how do you prepare a standard solution
1.the solid is weighed accurately
2.the solid is dissolved in a a beaker with less dissolved water than necessary to fill the volumetric flask
3.the solution is transfered to the flask and the last traces from a glass rod and beaker are rinsed with dissolved water
4.then the flask is filled drop at a time of distilled water until the bottom of the meniscus is exactly on the line
5.the volumetric flask is inverted to ensure the solution thoroughly mixed
why do you invert the volumetric flask?
the mixing would be uneven. Inverting alows uniform mixing and an equal concentration throughout the solution
whats the tolerance of the volumetric flask
100cm3 +- 0.2
250cm3 +- 0.3
how to carry out a titration
- fill a burette with acid of a known concentration
- record the volume of acid in a burette
- measure a known volume of alkali into a conical flask
4.add a suitable indicator
5.add acid from the burette to the conical flask slowly
6.stop adding acid when the end point is reached
7.record the volume of acid used
8.repeat until you get concordant results within 0.1cm3 - calculate the conc of alkali
what are the three indicators
methyl orange: red in acid yellow in alkali
phenalthaline: colourless in acid pink in alkali
litmus: red acid blue in alkali
mean titre is
within 0.1 ‘concordant’
if this is not taken into acount you loose accuracy of the titration
what is the uncertainty of pipette of 20cm3 25cm3 and a burette of 50cm3?
pipette 10- +_ 0.04
pipette 25 +_ 0.06
burette +_ 0.1
read from the ….. of the meniscus
bottom
to make biurette readings more accurate
read to 0.05 not 0.1
percentage uncertainty
100 x absolute uncertainty/calculated value