• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

Assessed Practical: Titration

Extracts from this document...


Assessed Practical: Titration Planning assessment The apparatus to be used: * Beaker * 250cm 3 volumetric flask * Funnel * Burette * Pipette * White tile * Conical Flask * Balance * Spatula * Weighing bottle * Glass rod Method Making a standard solution: A weighing bottle was accurately weighed and approximately 5g of anhydrous sodium carbonate was added and the weight of the bottle plus the solid recorded. The anhydrous sodium carbonate was then transferred into a 100cm3 clean beaker. The bottle was carefully rinsed out two or three times with water and the washings were transferred to the beaker each time. About 25cm3 of water was poured into the beaker and stirred with a glass rod until the solid had completely dissolved. This solution was then added to a 250cm3 volumetric flask using a funnel. The beaker and funnel were swilled thoroughly using a small amount of water these washing were then added to the volumetric flask. Water was then added to the volumetric flask until it was about 1cm below the graduation mark. The water was then added slowly from a clean pipette so that at eye level the bottom of the meniscus was just touching the graduation mark. ...read more.


The solution was released from the burette drop by drop when the end point was near to find the exact drop at which the sulphuric (VI) acid stops reacting with the sodium carbonate solution. If it were let out very quickly there would be a larger percentage error, as the readings would have a large difference in values. The experiment was repeated until concordant results were obtained so that reliable and accurate readings were acquired. Approximately 5cm of the anhydrous sodium carbonate was used as this was a logical amount; not too much so that it would not completely dissolve, but not too little so that only a small amount of the sulphuric (VI) acid would be needed to neutralise it as a smaller reading gives a larger percentage error. 250cm3 standard solution of sodium carbonate was made so that the same solution could be used when doing repeats because this ensures that the concentration of the sodium carbonate solution used for each titration is the same. 25.0cm3 of sodium carbonate was used for the titration as this was a reasonable amount; enough to be able to stir it and see a colour change, not too much so that large amounts of sulphuric (VI) ...read more.


If spilt in the lab, wash the area thoroughly. Sulphuric (VI) acid is a corrosive and can cause burns to the skin so a lab coat must be worn at all times. If swallowed, wash out mouth and have a glass or two of water. Do not induce vomiting and seek medical attention as soon as possible. If splashed into the eye flood eye with gently running tap water for 10 minutes and seek medical attention. If the acid is spilt onto skin or clothes remove the contaminated clothing and quickly wipe as much liquid off the skin as possible with a dry cloth before drenching the area with a large excess of water. If a large area is affected or blistering occurs seek medical attention. If spilt in the laboratory wear eye protection and gloves. Cover with mineral absorbent and scoop it into a bucket. Add anhydrous sodium carbonate over the mixture and leave to react, and then add lots of cold water. Rinse the area of the spill several times with water. Sources of information AS Chemistry At Esher College Work Book 1 "The Elements of Life" and "Developing Fuels", pg. 4-5 Hazcards, Cards 98, 95 and 32 http://www.chemistry-react.org/go/Faq/Faq_8219.html Aoife Gaffney ...read more.

The above preview is unformatted text

This student written piece of work is one of many that can be found in our GCSE Aqueous Chemistry section.

Found what you're looking for?

  • Start learning 29% faster today
  • 150,000+ documents available
  • Just £6.99 a month

Not the one? Search for your essay title...
  • Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month

See related essaysSee related essays

Related GCSE Aqueous Chemistry essays


    The measuring equipments were set up before using them the buffer was connected to the pH meter and Ph paper was ready. Experimental errors in the experiment can be that the buffer wasn't washed every time using it. Another error can be that incorrect labelling the pH solutions.

  2. copper practical

    Electrolysis allows you to gain a higher percentage of pure copper as opposed to having impure copper. When aqueous copper sulphate solute is electrolysed on copper electrodes, the copper is deposited on the cathode (which contains pure copper) and the anode loses weight (the anode has the impure copper on it).

  1. In this experiment I am finding out how much sulphuric acid is present in ...

    Meniscus Errors When recording down my end point of the titration (i.e. the volume). I did not look properly at the point of the meniscus, therefore gaining a very minimal percentage error of about 0.10%. It is very important that the lowest point of the meniscus is observed very carefully

  2. In order to find out the exact concentration of sulphuric acid, I will have ...

    This would have had some sort of effect on the accuracy of the results. Also I noticed that during my second and fourth titration, the size of the methyl drops added to the solution appeared to be twice the size compared to normal ones and this might have contributed to

  1. The flood

    I grabbed the nearest towel and tossed it over the variety of boxes of cereal mum stored out here. Pandemonium filled the air, the sound of wet feet slopping through a couple of inches of water, the electric fuse box so close I dared not look at it for fear

  2. Investigation of the carbonate - bicarbonate system

    Table (2) shows the value that was obtained. Results The investigation of carbonate and bicarbonate in the water sample can first be described by the following reactions: (a) H2CO3 (aq) H+ (aq) + HCO3-(aq) (b) HCO3-(aq) H+ (aq)

  1. To carry out a titration between a strong acid and a weak alkali, to ...

    It will change from green to clear.) * 2.65g of sodium carbonate (this will be turned into a solution by adding 250cm3 of distilled water).The concentration of the sodium carbonate solution: 0.1 mol dm-3 * A small pipette to accurately add the distilled water to the graduated volumetric flask, and

  2. Sodium Carbonate, Sulphuric Acid and Methyl Orange Assessed Practical

    Transfer this into a conical flask. * The burette should be attached to the clamp, leaving space at the nozzle to the conical flash and white tile can be put underneath it. * The white tile and the conical flask should be placed underneath the burette.

  • Over 160,000 pieces
    of student written work
  • Annotated by
    experienced teachers
  • Ideas and feedback to
    improve your own work