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

The aim of this experiment is to find the concentration of a sample of limewater solution in g dm3.

Extracts from this document...


Chemistry Plan The aim of this experiment is to find the concentration of a sample of limewater solution in g dm3. I am required to design my own experiment and choose a range of appropriate equipment and apparatus. I am provided with 250 cm3 of limewater, which has been made such that it contains approximately 1g/dm3 of calcium hydroxide. Also available is hydrochloric acid which has a concentration of 2.00 mol dm3, this concentration is too much though so it is necessary to dilute it. The apparatus, equipment and chemicals that I will use are as follows: - 1) Pipette 25cm3 2) Volumetric flask 500cm3 3) Conical flask 250cm3 4) Burette 5) White tile 6) Clamp and stand 7) Indicator (methyl orange) 8) Limewater (250cm3 with approximately 1g/dm3 of calcium hydroxide) 9) Hydrochloric acid- standard solution (conc. 2.00 mol/dm3) 10) Distilled water Slaked lime dissolved in water is called limewater. ...read more.


That is why I have chosen the pipette, volumetric flask and burette. All of these instruments have an accuracy of �0.05cm3, which is suitable for my experiment and should produce accurate and reliable results. In making my choice of indicator I also had to be very careful. The Limewater used will be a relatively weak base so it will be appropriate to use methyl orange as it has an end point on the ph scale between 8-5. Whereas phenolphthalein indicator has an end point much higher up in the ph scale. So if I were to use the phenolphthalein indicator then the end point (colour change) would be reached before the equivalence point (when the chemicals, acid-base break up). Implementing Safety is very important and it is necessary to follow safety procedures. It is important to wear eye protection when working with any acid. Also long hair should be tied back. ...read more.


When the indicator is added the colour of the solution is light, clear, orange and this should turn to pink by the end of the titration. In order to obtain consistent and reliable results it is necessary to repeat the experiment 3 times at a minimum and if the results were not in 0.1 of each other then further experiments would be needed. 0.1 is the figure that I have used as it is the accuracy of the burette. After this it the results must be noted in a table complete with the correct units. Using these results we first apply this formula Number of moles= concentration*volume(dm3) to the Hcl as we know its amount and concentration so can work out its number of moles. We then look back at the balanced equation and see the reaction ratio. In this case it is 2 moles of Hcl to 1mole of Ca(OH)2. So we times this number by 2 and we have the number of moles of limewater. ...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. Aim/Objective: To find out the dissolved oxygen content (in mg dm-3) in a water ...

    So, a smaller amount of sodium thiosulphate solution would be required in titration, which would lead to a smaller amount of dissolved oxygen content in the sample. In the experiment, it was assumed that the water sample did not contain any solutes which will oxidize or reduce iodine.

  2. Antacid Experiment.

    When we reached the final result (for the Superdrug indigestion tablet it was somewhere near 9.5cm-cubed of 1m-hydrochloric acid) the solution would stay yellow, acidic, and would not be able to turn back to an alkali, no matter how long you would stir it for.

  1. Find out the accurate concentration of an aid solution thought to have a concentration ...

    slowly until the base of the meniscus is on the 25cm3 mark. Fill a burette with 0.1 mol dm3 sodium carbonate solution. Make sure that the burette jet is also full of solution. 5. Record the volume reading in the burette before starting the titration.

  2. Determine the concentration of lime water.

    In titration it is impossible for one to judge the solution during the end point of the indicator to be the exact same colour all three times with just the naked eye. This is another limitation in the procedure. During titration the colour change can be rapid to counter this

  1. determining the concentration of a limewater solution

    Hydrochloric acid also reacts very strongly with certain metals such as calcium and must not be kept or stored any where near them. Due to these factors, goggles must be worn at all times. It is also advisable to wear a lab coat and latex gloves.

  2. The aim of my experiment is to find the exact concentration of limewater. In ...

    all stools should be out of the way under the desks as well as bags so they do not cause any accidents during the experiment. Some of the chemicals being used do have hazards and therefore it is necessary that extra care is taken.

  1. The aim of this experiment is to find out the concentration of a solution ...

    Calculate the mass of sodium carbonate to make 250cm� of a 0.1 M solution. Na2CO3 (aq) + H2SO4 (aq) --> Na2SO4 (aq) + CO2 (g) + H2O(l) Na2CO3 (aq) (2x23)+(12)+(3x16)= 106g in 1000cm� of H2O(l) = 1 molar solution Therefore there is 10.6g in 1000cm� of H2O(l)

  2. Calibrating a PH meter and preparing a 1mol dm-3 solution of sodium hydroxide

    Gloves were worn to prevent contact with the solution. It is very corrosive and can cause burns in all tissues that come in contact with it. The pain sustain can be severe and last for several hours.

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