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

Find the concentration of limewater solution Titration

Extracts from this document...


Finding the Concentration of Limewater Solution The aim of the experiment is to find the concentration of a limewater solution (calcium hydroxide) as accurately as possible. The limewater solution is approximately 1gdm-3 but to get a more accurate concentration I will use an acid based titration. A neutralisation reaction will take place between the acid (hydrochloric acid) and the base (calcium hydroxide) during the titration. I will use the base to neutralise the acid and make a salt (calcium chloride) and water. This reaction can be written as: 2HCl + Ca(OH)2 � CaCl2 + 2H2O However I need to find the exact concentration of the reagent, Calcium Hydroxide solution. To overcome this problem I will need to perform an acid based titration. The other problem is that the acid reagent is too concentrated as it is 2mol/dm�. This means the reaction will occur faster because there is a greater chance of a successful collision, which means it would be harder for me to acquire an accurate result, as the end point will occur too quickly. I will need to reduce the concentration of the hydrochloric acid, thus prolonging the time taken for the reaction to take place so I can get a more accurate result*. So I can make accurate calculations with my results I will need to convert the concentration of the limewater solution, which is in g/dm�, to mol/dm�. ...read more.


Slowly let the water drain out whilst twisting the burette so that it is washed from all sides. Then turn it back the right way and open the burette tap, releasing all the water from the burette. Next repeat the process using HCl to get rid of the deionised water. We now need to wash out the pipette. To do this you need the pipette filler. Place the pipette filler on top of the pipette and squeeze out the air in the filler by pressing the valve at the top of the filler, then to suck the limewater into the pipette you need to press the valve at the bottom of the filler. Fill it to approxamatly half way and repeat the process of cleaning used with the burette. Use deionised water first and then the substance going to be used, which is limewater solution. Finally the conical flask in which you will put 25cm� of Ca(OH)2 needs to be washed, but with deionised water only. You now need to set up the burette. Fix it to the clamp so that the 0 mark is roughly at eye-level. If it is too high, then you need to place it on a stool to fill the burette. You now need to fill the burette with HCl, using a funnel, to about twice the amount you need. ...read more.


Therefore the titre end point has an error analysis of 0.1cm�. To work out the percentage error you must divide the error analysis by the the reading taken, for example if the titre end volume is 25cm�: Percentage error = (0.05/25) x 100 = 0.4% % Error of the 5cm� pipette The pipette has an error of 0.1cm�. Therefore the percentage error is: Percentage error = (0.05/5) x 100 = 1% % Error of 25cm� pipette The pipette has an error of 0.05cm� so the percentage error is: Percentage error = (0.05/25) x 100 = 0.2% % Error of 500cm� volumetric flask The volumetric flask has an error of 0.2cm� so the percentage error is: Percentage error = (0.2/500) x 100 = 0.04% This is the reason for the equipment stated for experiment, as it has a lower % Error than a simple measuring cylinder. Also this is the reason for diluting the acid instead of using 2mol/dm�. The original acid would have given a much higher percentage error because the The total error of the equipment used in the experiment is experiment is �1.64%. From the error calculations we can determine why it is better to use diluted HCl rather than the 2mol/dm� HCl. If the full concentration is used and the titre used is 20cm� then the amount of HCl required is: 20/100 = 0.2cm� therefore the percentage error is: Percentage error = (0.1/0. ...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

    Enthalpy of Neutralisation.

    3 star(s)

    and Sodium Hydroxide (200cm3 of 1 molar). The equation for the reaction is as follows: CH3COOH + NaoH ? CH3COONa + H2O ?H = -56.1 kJ mol-1 In this reaction, exothermic reaction is taking place. Data result table. Initial temperature: 26oC. 1 ml of CH3COOH Temperature in degrees centigrade 0 22 0 22 0 22 0 22

  2. How much Iron (II) in 100 grams of Spinach Oleracea?

    present in 100 grams of Spinach. Although this is not the expected answer of 4 mg's, it is closer to the expected result than Experiment A. This could be due to the smaller volume of spinach extract solution that I used in Experiment B's titrations.

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

    (Note: Burette and pipette must be rinsed 2-3 times with 5 cm� of solution to be used. Every time filling up burette using a funnel, the funnel is held to avoid the breakage to the burette and spill of fluid due to the displacement of air.

  2. The Concentration of Limewater Solution.

    This ensures that the solution is thoroughly mixed and that the methyl orange indicates the overall pH of the solution. 10. Record the volume of hydrochloric acid used, reading the burette scale from the bottom of the liquid meniscus. 11.

  1. Determine the solubility of calcium Hydroxide solution with the aid of the titration process

    It is used to securely maintain the contents (in this case hydrochloric acid) until the time of use; it avoids the acid interacting with any other element. Safety spectacles Will be placed in front of the subject's eyes and will have to be worn throughout the course of the experiment.

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

    Things to do during my titration so that I obtain accurate and reliable results: * Make sure that the burette is washed out with distilled water so that no contamination occurs and all impurities gone. If possible rinse out the burette with the solution that it will be filled up with e.g.

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

    is typically a water-soluble, sour-tasting chemical compound. In common usage an acid is any substance that, when dissolved in water, gives a solution with a pH of less than 7. In general scientific usage an acid is a molecule or ion that is able to give up a proton (H+ ion)

  2. I have to plan an experiment to find the solubility of calcium hydroxide, Ca(OH)2, ...

    The spotting tile is there to help establish when the neutralisation between the acid (hydrochloric acid) and alkali (calcium hydroxide) has fully occurred. The equipment will be set up as below: Before beginning any one of the titrations, always record the initial volume from the burette.

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