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Preparation and analysis of inorganic and organic compounds Essay

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Task 1 titration of sodium hydroxide with hydrochloric acid

In this experiment the sodium hydroxide is neutralized with Hydrochloric acid to produce sodium chloride (the soluble salt) it is then crystallized in a dish.

The equation for the above reaction is →NaOH(aq) + HCl(aq) → NaCl(aq) + H20(l)


Add 25cm3 of sodium hydroxide into a conical flask then add couple of drops of methyl orange indicator
Next fill the burette with HCL using a funnel to the 0 mark
Add HCL to sodium hydroxide in small amounts swirling constantly keep adding until the solution changes to a red colour record your result
Using the same volume of HCL now add it to another 25 cm3 of sodium hydroxide to produce a neutral solution
Use a Bunsen burner and an evaporating dish to reduce the volume to half
Finally leave to evaporate in a crystallizing dish to produce a white crystalline solid

Average Volume = 26.

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Mass of Evaporating dish = 53.86 (Mass = 55.04 – 53.86 = 1.18g)

Mass = n x Mr = 0.025 x 58.5 = 1.4625

Calculating Percentage Yield 1.18 x 100 = 80.7 %


Test for ions present

Sodium Na+ — test carried out = flame test – result golden yellow

This happens as the electrons move to higher energy level and then fall back down when heated which gives out yellow light.

Chloride test → test carried out = add silver nitrate – result white precipitate of silver chloride was formed

Task (e)

Purity analysis of NaCl

In this task I will be showing the purity 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 indicator

The chemical formula for the following reaction is:NaCl(aq) + AgNO3(aq) → AgCl(s) + NaNo3(aq)


These are the results obtained for the following experiment:




Final burette reading




Initial Burette Reading








Average Volume = 20.55

Converted to dm3 /1000

1)calculate no of moles of silver nitrate

N= C x V =0.05 x 0.02055 = 0.010275 moles

2)answer = no of mole of NaCl (1 : 1 ratio)

3) Calculate the actual concentration of NaCl

C= n/V = 0.010275 = 0.10275moldm-3


4)percentage purity

ppurity = 0.1 x 100 = 97.3%)


Task 2


1)shake 2g of 2- hydroxybenzoic acid with 4 cm3 of ethanoic anhydride in a 100cm3 conical flask

2) add five drops of concentrated sulphuric acid agitating the flask for about 10 mins the whole wil form a crystalline mush

3) Dilute by stirring it in 4cm3 of cold glacial ethanoic acid and cool by placing in a water bath containing crushed ice

4) filter off the crystals using a Hirsch funnel and wash once with ice cold water

5) place the crude aspirin in a 100cm3 beaker add hot water not boiling water till it dissolves

6)cool and filter of crystals this process is known as recrystallisation

7) Take 4 test tubes add 2cm3 of distilled water in each and in 1 tube add one crystal of the product before recrystallisation and shake

8) Second tube add one crystal of the recrystallised product and shake

9) Third tube add one crystal of 2-hydroxybenzoic acid and shake

10) In last tube add one crystal of known pure aspirin and shake

11)To each tube add 2 drops in turn of neutral iron (III) chloride and shake

Following this method I got the following results

Mass at start was 2.04

Finishing mass was 2.08

Amount of yield:

138 →180

1 →180/138

1 →1.3

2.04 → 2.652

2.08 x 100 = 78.4%


Organic testing

To test for a phenol group


Add 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 impure

Melting point analysis

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Hi, I am Sara from Studymoose

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Hi, I am Sara from Studymoose

Hi there, would you like to get such a paper? How about receiving a customized one? Click to learn more https://goo.gl/CYf83b


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