• 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 determine the concentration of a limewater solution by method of titration.

Extracts from this document...

Introduction

Assessed Practical To determine the concentration of a limewater solution. Aim: The aim of this experiment is to determine the concentration of a limewater solution by method of titration. Ca(OH)2 (aq) + 2HCl (aq) CaCl2 (aq) + 2H2O (l) The calculation below is to determine the dilution factor and the volume of HCl needed for this titration. Moles of Ca(OH)2 = Mass / Mr 1 / 40.1 + (16 x 2) + (1 x 2) 1 / 74 0.013513513 moles Concentration of Ca(OH)2 = N / V 0.01 / 1 0.01 moldm -3 Moles = C x V 0.013513513 x (25/1000) 0.0003378moles Ratio: HCl : Ca(OH)2 2 : 1 0.000676 : 0.0003378 Moles of HCl = moles of Ca(OH)2 x 2 V = N / C 0.00674 / 2 ...read more.

Middle

* 250cm3 conical flask * distilled water * 25cm3 pipette To dilute the Hydrochloric acid- 1. Pour 2.5cm3 of HCl into a volumetric flask using a 5cm3 graduated pipette. 2. .Fill up to the marked like on the 250cm3 volumetric flask with distilled water. 3. This has diluted the 2mol dm -3 HCl to 0.02mol dm -3 . Titration: 1. Firstly the burette should be placed securely in the stand, 10 cm above the surface of the table. 2. Fill the burette with 50cm� of HCl, using a funnel to prevent spillage of the acid. Record the initial volume in a results table. 3. Pipette 25cm� of limewater into a 250cm� conical flask. ...read more.

Conclusion

Record the final volume of HCl in the results table. Then calculate the titres by minusing the final volume from the initial volume. 7. Dispose of the contents in the conical flask; rinse the conical flask with distilled water. Add 25cm� of limewater and five drops of methyl orange. Place the conical flask underneath the burette. 8. Repeat steps 5, 6 and 7 until you have three titres that are all within 0.1cm� of each other. This means that the results obtained are concordant to each other. Safety, Hazards and Preventions: Chemical Name Hazard Precaution Hydrochloric acid (2mol dm -3) Irritant Wear safety goggles and a Lab coat. Calcium Hydroxide (1g dm -3) Minimal Hazard Wear safety goggles Indicator: Methyl orange Skin Contaminant Use a pipette to avoid skin contact. ...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

or


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. Plan. In this experiment I intend to discover the exact concentration of an unknown ...

    This is because the limewater contains roughly 1g dm-3, the concentration of which can be worked out thus: Moles = Mass Mr = 1 74.1 = 0.0134952766531713 = 0.01 mol dm-3 (to 3 significant figures) As a result, the hydrochloric acid at 2 mol dm-3 would make the experiment unreliable

  2. Find the concentration of limewater solution Titration

    2/ 0.02 = 100, this means the dilution factor by which I have diluted the acid is 100. I will need to make 250 cm� of 0.02mol/dm� hydrochloric acid. The amount of 2mol/dm� I will need to add is 250/100 = 2.5cm�.

  1. determining the concentration of a limewater solution

    an average of my 4 results to give a better figure that will be more reliable and therefore, will give me a more accurate calculation. I will not be including the pilot in this because it was merely a test run and I do not feel that I did it to the same accuracy as the others.

  2. The aim of this experiment is to determine as accurately as possible the concentration ...

    There isn't a graduate colour change making the end point hard to notice. Hazards Hydrochloric Acid The solution of HCl we start with, is of 2.00mol dm-3, the hazards associated with HCl of this high concentration include: * Is an Irritant After diluting the HCl it will be of 0.02mol

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

    If only 2 drops were used it would be too difficult to notice the exact colour change. 12. Take the initial burette reading, from the base of the meniscus (white tile behind) 13. Place the conical flask beneath the burette on a white tile, so the colour change will be easily noticeable when it occurs.

  2. To determine the concentration of a limewater solution

    distilled water, including the12.5 cm3 of 2M HCl, the concentration of the acid will be 0.1 moles dm-3, as the following calculation illustrates: Concentration (moles dm-3) = number of moles volume (dm3) = 0.025 = 0.100 moles dm-3 (to 3.s.f)

  1. The Concentration of Limewater Solution.

    No of moles of HCl in 10.00cm3 = volume x concentration = 0.010 x 2 = 0.020 moles Concentration of diluted HCl = no of moles = 0.020 = 0.020mol dm3 Volume 1dm3 Therefore, I will dilute 10.00cm3 of the 2.00mol dm-3 hydrochloric acid, which will have a concentration of 0.020mol dm3.

  2. To determine the concentration of Limewater solution

    You can then add very precise amount of the HCl to the substance in order to find the end point using an indicator. By titrating the two substances you can find out how many moles they both need to react with each other.

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