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# Plan To Determine The Concentration Of A Limewater Solution

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Introduction

Plan To Determine The Concentration Of A Limewater Solution In order to determine the concentration of this limewater solution I must perform a titration (also known as volumetric analysis) between the alkali and acid given to me. In order to carry this out I must know the concentration of one of the solutions (in this case the acid, which has been given to me at 2.00 mol dm-3) and the balanced equation between my two reactants; which is: Ca(OH)2 (aq) + 2HCl (aq) � CaCl2 (s) + 2H2O (l) For which the ionic equation would be (as with all neutralisation reactions): OH- (aq) + H+(aq) � H2O (l) Dilution Calculations As the concentration of my acid is 2.00 mol dm-3 I believe this will be too strong, so little will be used and my results will be more unreliable. If I did the experiment with the 2 mol dm-3 HCl: I will be using 25cm3 of sodium hydroxide so there would be: 1 74.1 = 0.0135 moles in 1dm3 of Ca(OH)2 as there is 1g dm-3 so the concentration is 0.0135 mol dm-3 this means there will be 25 � 0.0135 = 0.0003375 moles in the 25cm3 Ca(OH)2 I will use 1000 so the approximate amount of HCl needed to neutralise this will be 0.000746 moles Ca(OH)2 : HCl 1 ...read more.

Middle

from vibrant pink to clear in acid, whereas bromothymol blue is blue in alkaki and yellow in acid but has a halfway point of green so it would be more difficult to determine an exact point). Titration Equipment List And Diagram - 50cm3 burette - burette stand - 25cm3 pipette - pipette filler - funnel - 250cm3 conical flask - white tile - 0.02 mol dm-3 hydrochloric acid - 1g dm-3 calcium hydroxide solution - phenol phthaline I am using volumetric equipment (pipette and burette) so that the measurement errors are lower and my end result is more accurate. The white tile is used so that the colour of the alkali and indicator mixture is more visible and I will be able to determine the end point more easily. Titration Method Set up the equipment as shown in the diagram: attach the burette to the 50cm3 burette stand at a height that allows the burette to be read easily and leaves enough room for the conical flask to be placed underneath Using a plastic funnel, fill the burette up to the 0cm3 mark with the 0.02 mol dm-3 hydrochloric acid made during the dilution process. Remove the funnel so excess drips of acid do not affect the initial volume. ...read more.

Conclusion

(http://www.jtbaker.com/msds/englishhtml/h3883.htm) Calcium Hydroxide - Again the concentration I am using is very low but I will still follow most of the recommended safety practices. Avoid lost term exposure by inhalation by performing experiment in a well ventilated area. If ingested drink two glasses of water then induce vomiting. Has mild irritant properties, so long term contact with skin and eyes should be avoided; I will wear goggles and a lab coat to reduce the chance of any contact being made; but if some is spilt on my skin I will wash the area thoroughly with soap and water; if any gets into my eyes I will rinse with clean water immediately for at least 15 minutes lifting the lids occasionally. Not flammable or reactive. (http://www.sciencestuff.com/msds/C1989.html) I will immediately clean up any spillages using water and a paper towel, and to try and reduce the likelihood of spills I will immediately replace lids onto any bottles of solution once I have finished using them I will also be handing a lot of glass equipment, so I must ensure the burette is firmly held in place by its stand, and I will not leave the burette or pipette anywhere may they roll off and smash. If a breakage does occur I will clear it up immediately using a dustpan and brush and put the shards inside some newspaper before I place them in the bin. ...read more.

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