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

To determine the concentration of a solution of ethandioic (oxalic) acid

Extracts from this document...

Introduction

To determine the concentration of a solution of ethandioic (oxalic) acid The aim of this experiment is to find the concentration of a sample of ethandioic acid in? g/dm3.i am require to design my own experiment and choose a range of appropriate equipment and apparatus. And think of the indicator as well. I am provided with 250cm3 ethandioic acid .the concentration is too much though so it is necessary to dilute it. The apparatus, equipment and chemicals that I will use are as follows: Equipment and apparatus: 1.pipette 25cm3 2.conical flask 250cm3 3.two burettes 4.white tile 5.clamp and stand 6.funnel 7.beaker 8.filler 9.distilled water 10.volumetric flask Chemicals: 1.indicator (phenolphthalein) 2.Ethandioic acid 3.sodium hydroxide In order to reduce errors it is necessary to choose accurate and reliable equipment. That is why I have chosen the pipette, and burette. All of these instruments have an accuracy of +0.1cm3,which is suitable for my experiment and should produce accurate and reliable results. ...read more.

Middle

2 + 2H2 O The sodium hydroxide needs to be diluted to give a titration, which has matched solution, i.e. in which 25cm3 pipette will react with approx 25cm3 from the burette Ethandioic: 2g/dm3 is of concentration 2/126=0.01587mol/ dm3 I.e. approx 0.016 mol/ dm3 To match this solution the ethandioic needs to be approx 0.032-mol/ dm3 The volumetric flask used for dilution has volume 250 cm3, let the volume required be v Because we know that: V1?C1=V2?C2 Where C1=the concentration of the concentrated solution V1=the volume of the concentrated solution C2=the concentration of the dilute solution V2=the volume of the dilute solution So, v�c=v�c V�1=250�0.032 V=8.00 cm3 The volume used for dilution is 7.00 cm3 to 9.00 cm3 Method: 1.Set up the apparatus, use a clamp to fix the burettes, one is on the left and one is on the right. 2. Put the funnel on the burette 1, and then pour the sodium hydroxide into the burette 1, and read the number carefully with ...read more.

Conclusion

7. Add 5 drops of phenolphthalein in the conical flask, now the colour of the solution is colourless. 8. Titrate with the diluted sodium hydroxide from the second burette. You must pour the solution very carefully, because you don't know when the solution will change colour. Firstly put the white tile under the conical flask to see the colour more clearly and then titrate it very slowly. Shake the conical flask very often and see if the solutions change the colour after some drops. When the colour has changed to pink, you've got the result. Record it. Repeat the titration as many times in order to get two results which agree to within 0.1 cm3.because it will make the results more accurate. Titration of ethandioic acid with diluted sodium hydroxide. Rough Accurate Final burette reading /cm3 Initial burette reading /cm3 Volume of diluted NAOH / cm3 Show that results you used to obtain this value of the volume of diluted sodium hydroxide by placing a tick under the readings used. ...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. The Use of Volumetric Flask, Burette and Pipette in Determining the Concentration of NaOH ...

    When carrying out an acid-base titration, we must able to recognize when to stop adding the standard solution. That is, we must be able to recognize when neutralisation has occurred. This is the purpose of the indicator. A sudden color change due to the indicator signals that neutralisation has occurred.

  2. The Use of Volumetric Flask, Burette and Pipette in Determining the Concentration of NaOH ...

    Most organic acids are weak acids. A few clarifications: The terms "hydrogen ion" and "proton" are used interchangebly; both refer to H+. In chemical equations H+ is often written, although in water it will actually be H3O+. The strength of an acid is measured by its Ka value.

  1. Finding out how much acid there is in a solution.

    * You should not eat or drink during an experiment, as it could get contaminated. * Be careful when using sulphuric acid, even though it is not that harmful as it has a low concentration, make sure that it does not come in contact with your skin, as it could cause burns and irritation to the eyes.

  2. Find out how much acid there is in a solution

    * Record the final reading of the burette. * Write down the titre. Accurate Titration * When proceeding with an accurate titration it is mostly based upon some of the similar procedures carried out from the rough titration. However, particular attention is involved when achieving the end point of a titration.

  1. Finding out how much acid there is in a solution.

    This indicator is very useful as the change in colour could be easily identified when the titrations are taking place. The following shows the equipment to be used in the actual titration: 1. Tripod stand 2. White Tile 3. 2 Clamps 4. Conical Flask 5. Burette 6. Distilled Water 7.

  2. To determine the concentration of a solution of ethandioic acid.

    Remember to remove the funnel before doing this! 4. Remove the volumetric flask from under the tap and make up the contents of the flask to the mark with distilled water. [To avoid errors, on reaching a point quite close to the mark, stop pouring the distilled water and use

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