Volumetric Analysis to Find Concentration of Acid

Volumetric Analysis to Find Concentration of supermanA. Dilshan JayawickramaIntroductionVolumetric Analysis is a quantitative method and which deals with the the great unwashed of a particular substance used in the analysis. However in volumetrical analysis most important portion is the volume. Here the volumetric analysis is proceed with known amount of etymons. But, concentrations of both the solution has non been mentioned since it is done to find unwrap the concentration of known harsh or a nucleotide. When adding known concentration solution to mystic concentration solution drop wise will result a show veer at a pourboire and this procedure called Titration. In volumetric analysis there are 5 main types as acrimonious base titration, oxidation-reduction titration, precipitation titration, complexometric titration and iodometric titration (Datta and Johar, 2014).Titration is the process of observing the color wobble of mixed solution when known concentration soluti on is added to unknown concentration solution.Titrant is the solution in volumetric analysis whose concentration is known.Titrand is the solution in volumetric analysis whose concentration is to be found. (Solution with unknown concentration).Indicator is the substance used to observe the color change of the resulting solution.Equivalence point is the point which will show the color change of the resulting solution for the first time when adding solutions from buret drop wise.End point is the point at which the color change will not be disappeared and stay permanently.Phenolphthalein is used because it is slightly acidic and it can detect the pH range of 8.3 to 10.0 resulting color change colorless to pink. Phenolphthalein is insoluble in water where it is soluble is alcohols. (Matthews, 2003).Color change of Indicators (Phenolphthalein)(Pradeep and Dave, 2013)Preparation of 0.1moldm-3 of NaOHTook 10.0ml of NaOH (1moldm-3) to the graduated pipette using pipette filler and introdu ced it into the volumetric flask whose volume is 100ml. thence diluted the solution up to 100ml by adding dis mangered water until the lower meniscus of the diluted NaOH solution to tally with the ring object present on the volumetric flask.Acid Base Titration is carried out to find the concentration of an acid or a base by neutralizing the acid or the base of which the concentration is unknown.The burette should be fill with the Base (known concentration solution) and the titration flask should contain the acid which the concentration is to be determined. Then three drops of indicator, phenolphthalein should be added to the titration flask, because the phenolphthalein will leads towards the color change in the resulting solution.In the titration above, the acid which has the unknown concentration is HCl and the base which has the known concentration is NaOH. When NaOH added with HCl, it results NaCl with H2O. atomic number 11 hydroxide + Hydrochloric acid Sodium Chloride + Water N aOH + HCl NaCl + H2OAfter setting up the equipment, the titration is carried out by allowing base from burette to fall into the acid drop wise and should observed the resulting solution actually carefully until it occurs the color change. At some point, when the NaOH drops falls into the HCl solution will result pink color due to phenolphthalein and that pink color is not permanent since it disappears. When observing the pink color for the first time, it will be the equivalence point.Then the test should be carried out so on until watch pink color will hold on without disappearing and it is called the endpoint of the titration. Once endpoint is reached, smasher of the burette should close soon and start up stop the titration. Then tabulate the reading by repeating the experiment at least three times to get three readings. Finally calculate the concentration of the unknown solution by putting the reading into the basic comparisons of chemistry.ObjectivesThe objective of this pr actical is to find out the unknown concentration of an acid or a base by Volumetric Analysis which is a quantitative analytical method.MaterialsVolumetric FlaskBuretteFunnelGraduated PipetteTransfer pipetteBeakersHydrochloric AcidSodium HydroxidePhenolphthaleinBurette HolderTitration FlaskPipette filerDistilled WaterMethodologyFirst the graduated pipette was washed with a trivial amount of Sodium Hydroxide (NaOH). Then the filled sodium hydroxide was discarded and 10.0 ml of NaOH was filled to the graduated pipette using pipette filler and transferred to a volumetric flask. A little amount of distilled water was poured into the volumetric flask and swirled. Then more distilled water was added up to the volumetric flask till it rises up to the ring mark and lower meniscus balanced.Cleaned the burette with small amount of NaOH. After that the burette was fixed vertically to the burette holder and the burette was filled up to 0.00ml mark. Then the graduated pipette was washed with som e (Hydrochloric) HCl acid to clean up. After cleaning the graduated pipette by HCl acid, it was filled with HCl acid whose concentration is to be found, exactly up to 10.0 ml with the help of pipette filler.Then 10.0ml of HCl acid was introduced to the titration flask and three drops of phenolphthalein was directly put into HCl acid in the titration flask without let it touching the glass of the titration flask. After that, placed the titration flask under the burette which was fixed to the holder.The tap of the burette was slowly opened to freeing the NaOH drop wise into the titration flask, then at one place, the NaOH drops when fall into the HCl acid will show some pink color dot for the very first time, and that point will call as the equivalence point of the titration. Then the tap was adjusted slowly to reduce the rate at which it release NaOH drops.Few seconds later at a point the pale pink color can be seen which is permanent, and that point is called the end point. Then c losed the tap of the burette and the volume of NaOH which has been used to neutralize the acid is recorded. After recording the first reading continued the practical ii more times to get another two readings. Results were tabulated.ResultsThe experiment is carried out for three times to get three readings and reading taken at each test has been tabulated below.Average volume = 32.10cm3 + 34.00cm3 + 35.20cm3 3= 33.76 cm3DiscussionTitration is the process of determining the concentration of unknown solution when two solutions are put into to neutralize. A chemical reaction has been used for this take aim and the reaction should be fast and should be a complete reaction. The titration should have a determinable equivalence point and an endpoint.We used HCl and diluted NaOH (0.1moldm-3) in this titration process and the indicator used is phenolphthalein which can cover a range of 8.3 to 10.0 pH value. Here, the indicator is acting like a signal showing where to stop the titration at e ndpoint.When NaOH added with HCl, it results NaCl with H2O.Sodium hydroxide + Hydrochloric acid Sodium Chloride + Water NaOH + HCl NaCl + H2OActually the endpoint is the neutral point where acid and base get neutralized. For this reaction, Ionic equation is H+ + OH H2OHere at the endpoint in first titration, the whole resulting solution turned into pale pink color, still other two reading were too far apart due to some errors.The errors which may lead to deviate the readings may beImproper calibration of glass waresmisread the volume in graduated pipetteUsing of contaminated solutionsUsing of solutions with wrong concentrationsUsing indicators in wrong amountsUsing impure glass wares non transferring the proper volume and not taking the proper volumeNot filling up the burette properlyUsing wrong solutions since all looks akin (colorless)Sometimes it can be due to the usage of contaminated solutions because taking the pipette for the next test without washing. It can be due to the way which cleaned the pipette after using once.Sometimes the titration results can alter due to human errors such as difficulty with reading the burette value or sometimes hand glows can have some drops of some other solutions and get dropped to the test which is going on.As the first reading 32.10cm3 was a successful effort, but still the test 02 (34.00cm3) and test 03 (35.20cm3) was unsuccessful due to those errors. Sometimes the color change was so rapid change and unable to stop the tap of the burette on time.ConclusionThe concentration of the unknown was determined by using titration process and by the known value for the other solution. Calculation should be carried out in order to get the final answer to determine the unknown concentration of HCl.CalculationAverage volume = 32.10cm3 + 34.00cm3 + 35.20cm3 3= 33.76cm3Assumption Number of moles remain unchangedTherefore by using, C1V1 = C2V20.100moldm-3 x 0.100dm-3 = C2 x 0.033dm-3C2 = 0.100moldm-3 x 0.100dm-3 0.033dm-3C2 = 0.30 moldm-3THE UNKNOWN CONCENTRATION OF HCl IS 0.30moldm-3ReferencePradeep, D.J. and Dave, K. (2013) A Novel, Inexpensive and Less Hazardous Acid-Base Indicator, journal of Laboratory Chemical Education, 1(2), pp. 34-35. Online DOI 10.5923/j.jlce.20130102.04 (Accessed 30 October 2014).Matthews, P. (2003) Advanced Chemistry. New Delhi Cambridge University Press.Datta, S.C. and Johar, N.K. (2014) Undergraduate Chemistry. New Delhi Anne Books Pvt.Ltd.