• Join over 1.2 million students every month
  • Accelerate your learning by 29%
  • Unlimited access from just £6.99 per month
  1. 1
  2. 2
  3. 3
  4. 4
  5. 5
  6. 6
  7. 7
  8. 8
  9. 9

Titration to analyse a solution of dilute sulphuric acid, and calculating the concentration of acid that it contains.

Extracts from this document...


Titration to analyse a solution of dilute sulphuric acid, and calculating the concentration of acid that it contains. Introduction/Aim: In this coursework my aim is to find out how much acid there is in a solution. I am going to use the technique of titration to analyse a solution of dilute sulphuric acid, and calculate the concentration of acid that it contains. This concentration is considerably greater than the concentration of acid in "acid rain", but the same method of analysis could be used to determine accurate values of PH for "acid rain" samples. I must find out the accurate concentration of acid, which is thought to have a concentration between 0.05 and 0.15 mol dm-3. The purpose of this experiment is to obtain an accurate concentration of sulphuric acid, which is found in solution. We are told that the sulphuric acid to be used has a concentration between 0.05 and 0.15 mol dm, but the task is to clarify the exact concentration using the method of titration. The indicators that I can use are either phenolphthalein or methyl orange this is because according to the titration curve for strong acid with strong base, the pH range for methyl orange (3.1-4.4) ...read more.


> Use a pipette and a pipette filler to transfer 10.0 cm3 of the acid rain sample to a 100 cm3 conical flask. > Add 3 drops of Methyl orange indicator. > Fill burette with 0.01 mol dm-3 sodium hydroxide solution. > Make sure the burette jet is also full of solution. > Record the volume reading in the burette before starting the titration. > Add sodium hydroxide solution in small volumes to the acid rain solution in the conical flask. > Gently swirl the flask after each addition. > The Methyl orange indicator should turn from a orange to a yellow colour. > Run in the small volumes of sodium hydroxide solution until there is a colour change from yellow to orange colour in the titration mixture. > This is the end point. > Record the final burette reading. > Now calculate the volume of hydroxide solution that has been used. > The 1st attempt that is done would be a rough titration. > From this rough attempt I should now have an idea of what the end point is. > After this rough titration I will do several more titrations until I record three volumes that agree to within 0.1 cm3. ...read more.


I feel it was best to have the acid placed in the burette rather than it in the conical flask, because it's easier to note the colour change from yellow to orange, than orange to yellow. I know that the errors that may have occurred during the experiment were minor and did not have a great impact on my final result, however I still feel that the main source of my error in carrying out the titration was where I had to distinguish where the indicator had changes colour. This is the reason for why I had to estimate an end point between the beginning and end point of the colour change. I used this method throughout all 3 of my titrations. If I was to ever do this experiment again I would make sure that I used a pH meter to distinguish the neutralization point. Even though by doing this it would not have a great impact on my titre, it will however make the investigation much more reliable and not subject to the choice of individual colour change. Also if I had more time to do this experiment I would do more titres rather than just 1 rough titre and three others. I would do several titres in order to compare them with one another. Ifrah Naz ...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

  1. Marked by a teacher

    Chem MC analysis. In which of the following cases may it obtain a complete ...

    5 star(s)

    misconception that compared with a strong acid of the same volume and concentration, a weak acid requires a smaller amount of alkali for complete neutralization, as a result, the alkali will be in excess,thus it is not a complete neutralization.

  2. Acid-Base titration of Sulphuric acid and Sodium Hydroxide

    I continued this process until the solution in the flask just turned colourless. I recorded the reading on the burette which showed me the approximate end-point. I repeated the experiment four times in order to get an average which is a more accurate reading.

  1. Planning of Titration

    * I will wash the beaker and glass rod 3 times to make sure that all the solution I will make goes in the Volumetric Flask. * I will rinse the burette once with water to get rid of any other chemicals or dirt in the burette and then 2

  2. Determine the concentration of sulphuric acid by acid-base titration.

    * White tile: used to make colour changes clearer. * Weighing bottle: to place the accurate amount anhydrous sodium carbonate. * 250cm3 beakers (2): used for mixing anhydrous sodium carbonate with distilled water. * Graduated volumetric flask: used to make up a solution of fixed volume very accurately * Electronic balance: used to weight the accurate amount anhydrous sodium carbonate.

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

    White tile - is necessary to identify the colour change and the eventual neutralisation point during the titration. Wash bottle - has a small in diameter nozzle, which can fit inside conical flask, beaker, etc and is used to store non-ionised water.

  2. Experiment to determine the concentration of sulphuric acid

    Safety Safety goggles will be worn to protect eyes from any splashes of irritants. Gloves will be used to protect hands from any contact with corrosive, irritant or toxic substances. Equipment 1g Magnesium carbonate Sulphuric acid ( 10 mol dm-� sulphuric acid.) Distilled water Divided flask Rubber delivery tube Pipette.

  1. The effect of Acid Rain on Seed Germination.

    The graph I obtained from my final results resembles that of the previous graph I had included in my prediction. My second graph also agrees with my prediction because the relationship between the concentration of the acid rain mixture and the complete length of the seed's growth is not directly proportional.

  2. Titration I will neutralize the sulphuric acid with a base, which will be Sodium ...

    this amount to work out the concentration of Sulphuric acid To calculate the concentration of sulphuric acid I first need to calculate the number of moles of sodium Carbonate used Volume x Concentration I have to find out the number of mols of Sodium Carbonate used (25/1000)

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