Preparation and analysis of inorganic and organic compounds Essay

Task 1 titration of sodium hydrated oxide with hydrochloric acidIn this experiment the sodium hydroxide is neutralized with Hydrochloric acid to produce sodium chloride (the soluble salt) it is then(prenominal) lechatelieritelized in a dish.The equation for the above reaction is NaOH(aq) + HCl(aq) NaCl(aq) + H20(l) systemAdd 25cm3 of sodium hydroxide into a conical flask then number couple of drops of methyl orange indicatorNext fill the burette with HCL using a funnel to the 0 markAdd HCL to sodium hydroxide in small amounts swirling constantly keep adding until the solution changes to a red colour shew your resultUsing the same volume of HCL now add it to another 25 cm3 of sodium hydroxide to produce a neutral solution implement a Bunsen burner and an evaporating dish to reduce the volume to halfFinally leave to evaporate in a quartz glasslizing dish to produce a white crystalline solidAverage Volume = 26.35Mass of Evaporating dish = 53.86 (Mass = 55.04 53.86 = 1.18g)Mass = n x Mr = 0.025 x 58.5 = 1.4625Calculating Percentage Yield 1.18 x 100 = 80.7 %1.4625Test for ions presentSodium Na+ test carried out = flame test result golden yellowThis happens as the electrons move to high energy level and then fall back down when heated which gives out yellow light.Chloride test test carried out = add silver bear upon result white precipitate of silver chloride was formedTask (e)Purity analysis of NaClIn this task I willing be showing the goodness analysis of NaCl the same procedure will be carried out as before but this time 0.1 moldm-3 of sodium chloride is titrated with 0.05 moldm-3 silver nitrate the indicator will be the chromate indicatorThe chemical formula for the following reaction isNaCl(aq) + AgNO3(aq) AgCl(s) + NaNo3(aq)RESULTSThese are the results obtained for the following experimentRough12Final burette schooling19.920.520.6Initial Burette Reading0.000.000.00Titre19.920.520.6Average Volume = 20.55Converted to dm3 /10001)calculate no of moles of silver nitrateN= C x V =0.05 x 0.02055 = 0.010275 moles2)answer = no of mole of NaCl (1 1 ratio)3) Calculate the actual concentration of NaClC= n/V = 0.010275 = 0.10275moldm-30.014)percentage purityppurity = 0.1 x 100 = 97.3%)0.010275Task 2Method1)shake 2g of 2- hydroxybenzoic acid with 4 cm3 of ethanoic anhydride in a 100cm3 conical flask2) add five drops of concentrated sulphuric acid agitating the flask for well-nigh 10 mins the whole wil form a crystalline mush3) Dilute by stirring it in 4cm3 of coldness glacial ethanoic acid and cool by placing in a water bath containing crushed ice4) filter off the crystals using a Hirsch funnel and wash once with ice cold water5) place the crude aspirin in a 100cm3 beaker add hot water not boiling water till it dissolves6)cool and filter of crystals this process is known as recrystallisation7) Take 4 test tubes add 2cm3 of distilled water in each and in 1 tube add one crystal of the product before recrystallisation and shake8) Seco nd tube add one crystal of the recrystallised product and shake9) Third tube add one crystal of 2-hydroxybenzoic acid and shake10) In last tube add one crystal of known pure aspirin and shake11)To each tube add 2 drops in turn of neutral iron (III) chloride and shakeFollowing this method I got the following resultsMass at start was 2.04Finishing chain reactor was 2.08Amount of yield138 1801 180/1381 1.32.04 2.6522.08 x 100 = 78.4%2.652Organic testingTo test for a phenol groupMethodAdd neutral iron III chloride(if a phenol group is present it will change into purple complex and if theres no purple then the aspirin is pure)Using the following method my result showed a purple complex showing that my aspirin was impureMelting point analysis