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Instructions and guidelines for carrying out quantitative analysis in chemistry through titrations using burettes and pipettes. It covers topics such as reading burette scales, rinsing and using pipettes, selecting data, and calculating concentrations. Students are expected to achieve specific titre values within a certain range to meet assessment requirements.
What you will learn
Typology: Study notes
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liquid needed in a reaction
the meniscus – you can read to 0.05 mL (half way between the 0.1 mL divisions. Eye is level with the bottom of the curve. Some say you can read to 0.02 mL with care and
practice!
(the titre) is the difference between the last scale reading and the first (initial) scale reading. Answers must not be negative!
Example
Rough 1st 2nd 3rd Final volume (mL)
15.30 30.
Initial Volume (mL)
0.00 15.
Volume used (mL)
Record volumes to 2 decimal places. Your initial reading does not have to start at 0.00 mL You are aiming for 3 results within 0.20 mL of each other. It should be possible to get them within 0. mL. These will then be classed as concordant results. You use concordant results to calculate the average titre.
solution and deliver into a conical flask.
Make sure you are familiar with the type of pipette that you will use in your assessment.
You rinse a pipette before use with a little of the solution you will be using it with.
into a conical flask
Rinse the burette with some of the solution that you are going to use in your titration. Don’t use water!
Don’t forget to check that there are no air gaps below the tap – drain some of the liquid through until all air has gone! Eye is too low in the first picture and too high on the third. The middle gives correct reading of 25.65 (mL)
Keep pipette vertical Use a slow smooth action Have your eye level with the bottom of the meniscus. Touch tip of pipette on side of conical flask at end of delivery. Avoid having unexpected air bubbles when drawing up the liquid.
You are looking for 3 concordant results – i.e. values that differ from each other by 0.10 mL – if not then choose the 3 closest values
13.80 13.20 13.40 13.60 13.
In this case a good choice would be to select the following data values: 13.20 mL, 13.30 mL and 13. mL
This would give an average titre of 13.30 mL to use in our calculation.
In this example it is advisable to do another titration – can you see why?
Remember that c = n/V c = concentration in mol L - n = amount of a substance in mol V = volume of solution used in Litres (L) Rearrange to give n=cV when required.
Steps involved
To convert mL to L divide by 1000 or multiply by 10-3^ e.g. 18.0 mL = 18.0 x 10-3^ L Don’t forget to do this!
Eg 20.0 mL of unknown concentration of NaOH(aq) was reacted with 10.0 mL of a solution of 0.150 mol L -1^ HCl (aq) Equation NaOH + HCl NaCl + H 2 O
A M or E? Achievement Achievement with Merit
Achievement with Excellence
Quantitative analysis involves collecting primary data from an acid-base titration, and processing both primary and secondary data to solve quantitative problems.
Titre values will be 15.70 ; 14.90; 15.60;
still need 3 within 15.10 and 15.30 mL -
0.10 mL