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

Determining the Concentration of a Limewater Solution

Extracts from this document...

Introduction

Determining the Concentration of a Limewater Solution Introduction Previous to conducting my experiment, research was carried out and the results of it adapted to aid me in solving the problem set. In the Advanced Chemistry Student's Book by Nuffield, on page 86, I found a similar experiment to mine with a description of implementation, which aided me in the fact that I discovered the temperature of my solution did not need to be taken. This was because the solution of calcium hydroxide they used was saturated, and therefore they measured the temperature of the saturated solution along with its solubility, due to the fact that the solubility of saturated substances varies with temperature. This procedure will not be necessary in my particular experiment as the solution I will use will be far from saturated. Safety measures were observed and taken into account by looking at the hazard card for calcium hydroxide. I found the substance to have minimal hazards, especially when diluted in a non-saturated solution, and thus concluded the only precaution needed to be taken was to wear eye protection during handling of the solution. ...read more.

Middle

+ (2 x 1.0) = 74.1 Therefore number of moles present = 1/74.1 = 0.013495 mol To dilute the 2.0mol dm-3 solution to 0.01mol dm-3 deionised water will be used to eliminate the possibility of impurities being present within the solution, the probability of this increasing would have been increased if tap water had been used. An entire decimetre of solution was not required for this investigation, therefore only 500cm3 was made up. The dilution was carried out accordingly; 10.00cm3: 1000.00cm3 = 0.02mol dm-3. Therefore 5.00cm3: 1000.00cm3 = 0.01mol dm-3. Therefore 2.50cm3: 500.00cm3 = 0.01mol dm-3. For this dilution a graduated pipette will be used to accurately measure 2.50cm3 of acid, following this the deionised water will be added until the bottom of the meniscus rests on the 500cm3 mark. The lid will then be firmly placed on the volumetric flask and the solution will be shaken well, at least 20 shakes to ensure that the concentration of acid is equally distributed throughout the solution. Prior to pouring the acid into the burette a small funnel will be placed into the top to aid accurate pouring, ensuring none of the solution is wasted. ...read more.

Conclusion

24.20 48.50 24.25 Initial burette reading (cm3) 0.00 24.20 0.00 Titre (cm3) 24.20 24.30 24.25 Average titre = 24.25cm3 ((24.20 + 24.20 + 24.25) / 3) Analysis The balanced equation: 2HCl (aq) + Ca (OH) 2(aq) --> CaCl2 (aq) + 2H2O (l) Therefore to find the concentration of the limewater I obtained the average titre, and then worked out the number of moles of hydrochloric acid that were used using the equation: No. of moles (mol) = Concentration (mol dm-3) x Volume (dm3 Therefore 0.01 x 0.02425 = 0.0002425mol. To work out the number of moles of limewater used, the ratio of limewater to hydrochloric acid is 1:2, therefore 0.0002425/2 = 0.00012125. To work out the concentration of the limewater this figure is divided by the volume of limewater used using the equation: Concentration (mol dm-3) = No. of moles (mol) / Volume (dm3). Therefore 0.00012125/0.025 = 0.00485. To work out the concentration in g dm-3 we must first obtain the molar mass of calcium hydroxide which is 74.1. Using the equation: Mass (g) = Number of moles (mol) x Molar mass Therefore 0.00485 x 74.1 = 0.359385gdm-3. This being only accurate to approximately 0.36gdm3 due to the limited precision of the apparatus 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. How much Iron (II) in 100 grams of Spinach Oleracea?

    (aq) react with 5 moles of Iron (II), and by using the equation below it is possible to work out how much Iron (II) is present in the spinach extract solution and then use this to work out how much Iron (II)

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

    Do not try to fill the burette to zero mark. Burette readings must be accurate up to two decimal places and the flow rate of the liquid should not exceed 30cm� per minute. 6. Pipette 20.0cm� (or 25cm) acid solution into three clean Erlenmeyer flasks.

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

    3 11.87 = | -5.89| = 5.89cm� (c) Concentration of base (diluted solution) M1V1 = M2V2 M1(11.87) = (0.01)(25) M1 = 0.25 ------- 11.87 = 0.0211M (d) Concentration of base (original solution) M1V1 = M2V2 M1(50) = (0.0211)(250) M1 = (0.0211)(250) ----------------- 50 = 0.1055M Discussions: Acid An acid (often represented by the generic formula AH)

  2. Determining the concentration of a limewater solution by volumetric analysis

    Start releasing the acid in single drops when the purple solution in the flask begins to turn colourless and when the solution is completely colourless stop adding hydrochloric acid as the endpoint has been reached. Using this first attempt as a test run to get used to the procedure and

  1. determining the concentration of a limewater solution

    Ca(OH)2 (aq) + 2HCl (aq) � CaCl2 (s) + 2H2O(l) The above equation shows that to neutralise the limewater, the ratio of Ca(OH)2 : HCl must be 1:2. This means that to have an equal amount of the limewater solution and dilute hydrochloric acid neutralising each other I will need to dilute

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

    This would now result in the HCl having a concentration of 0.02M, which is 100 x more dilute than the original 2M HCl that was provided. Now the HCl is ready for use in the titration. Begin by preparing the burette.

  1. An investigation to find the concentration, in g/dm, of a limewater solution.

    -Conical flask - this will contain the limewater solution and indicator -Clean white tile - to observe colour change of the indicator, when it turns colourless then the solution will have neutralised -Pipette - this will be used to measure out an accurate volume of limewater -HCl, distilled water, limewater,

  2. Determining theConcentration of Limewater Solution

    Hazardcoeb ebr seebebw oreb ebk ineb foeb eb: Precautionscofe fer sefefew orfe fek infe fofe fe; Hydrochloric Acidcoeg egr seegegw oreg egk ineg foeg eg. The HCL we are using is very dilute and therefore is not corrosive but is an irritant.

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