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Chemistry : Principles related to Practical chemistry ®
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PRINCIPLES RELATED TO PRACTICAL CHEMISTRY
S.No. Contents Page
Physical chemistry
01. Volumetric analysis 1
02. Enthalpy of solution of CuSO4 8
03. Enthalpy of neutralization of strong acid and strong base 10
04. Preparation of lyophilic and lyophobic sols 12
Kinetic study of the reaction of iodide ions with hydrogen peroxide at room
05. 16
temperature
06. EXERCISE : Multiple choice questions 17
Inorganic chemistry
01. Salt analysis 21
02. Preparation of inorganic compound 37
03. EXERCISE : Multiple choice questions 39
Organic chemistry
01. Determination of extra elements 45
02. Detection of functional groups 48
03. preparation of organic compounds 56
04. EXERCISE : Multiple choice questions 60
NEET SYLLABUS
PHYSICAL CHEMISTRY : The chemistry involved in the titrimetric exercises – Acids, bases and use of indicators,
oxalic acid vs KMnO4, Mohr's salt vs KMnO4.
Chemistry principles involved in the following experiments :
1. Enthalpy of solution of CuSO4
2. Enthalpy of neutralization of strong acid and strong base
3. Preparation of lyophilic and lyophobic sols
4. Kinetic study of the reaction of iodide ions with hydrogen peroxide at room temperature
INORGANIC CHEMISTRY :
Chemical principles involved in the qualitative salt analysis :
Cations : NH4+ , Pb , Cu , Al , Fe , Zn , Ni , Ca , Ba , Mg
2+ 2+ 3+ 3+ 2+ 2+ 2+ 2+ 2+
2– − –
Anions : CO2- 2-
3 , S , NO2 , Cl¯, Br¯, I , NO3¯, SO 4 (Insoluble salts excluded)
The chemistry involved in the preparation of the following
Inorganic compounds : Mohr's salt, potash alum
ORGANIC CHEMISTRY :
Determination of extra elements (Nitrogen, sulphur, halogens) in organic compounds; Detection of the following
functional groups; hydroxyl (alcoholic and phenolic), carbonyl (aldehyde and ketones) carboxyl and amino groups
in organic compounds.
The chemistry involved in the preparation of the following
Organic compounds : Acetanilide, p-nitro acetanilide, aniline yellow, iodoform.
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PHYSICAL CHEMISTRY
QUANTITATIVE ANALYSIS (VOLUMETRIC ANALYSIS)
• Volumetric analysis is the process by which the quantity of a substance present in the given solution is
determined by reacting it with a solution of other substances of known concentration. A given volume of the
solution of unknown concentration is treated with the solution of the other substances of known
concentration then by comparing the equivalence of the two solution, concentration of the unknown solution
can be determined. The process is known as Titration.
• In short titration may be defined as the process by which concentration of unknown solution is determined
with the help of a solution of known concentration.
Some Other Terms used in Volumetric Analysis :
1. Standard Solution : A solution of known concentration is called a standard solution, concentration of a
solution is generally expressed in terms of normality (N) or molarity (M).
2. Primary standard : The substances whose standard solution can be prepared directly by weighing is called
primary standard e,g. oxalic acid, ferrous ammonium sulphate etc.
A primary standard is a compound of sufficient purity in which total amount of impurities does not exceed
0.01-0.02%.
The substance to be used as a primary standard should also satisfy the following requirements:
1. It must be easily available in pure and dry form.
2. It should not undergo change in air i.e. it should not be hygroscopic, oxidised by air or affected by
gases such as carbon dioxide present in the atmosphere or lose water of crystallization, so that it can
be stored safely.
3. It should be easy to detect the impurities present in it.
4. It should have high relative molecular mass so that weighing errors are negligible.
5. Its reaction with another substance should be instantaneous and stoichiometric.
6. The substance should be readily soluble in water.
• Unstable hydrated salts, as a rule, should not to be used as primary standards. However, sodium
carbonate, sodium tetraborate, potassium hydrogenphthalate, oxalic acid, ferrous ammonium sulphate
etc. can be used as primary standards because of their sufficient stabilities.
Preparation of 0.1 M standard solution of sodium carbonate.
Sodium carbonate has characteristics nearer to the primary standards therefore its standard solution can be
made by direct weighing.
To prepare 0.1 M Na2CO3 solution, 10.6000g of sodium carbonate should be dissolved per litre of
–1
the solution (Molar mass of sodium carbonate is 106 g mol ).
Therefore, to prepare 100 mL of 0.1M Na2CO3 solution 1.0600 g of sodium carbonate is dissolved in
minimum quantity of water and the solution is diluted to exactly 100 mL by adding water to it.
3. Secondary standard : The substances whose standard solution can not be prepared by direct weighing.
A solution of secondary standard is the one which may be used for standardization after finding out its exact
concentration by titration against a standard solution of primary standard.
Sodium hydroxide and potassium permanganate are examples of secondary standards.
• Before starting titrimetric analysis, you should be familiar with some techniques such as, weighing by
using chemical balance, preparing standard solution, measuring volume by using burette and pipette.
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4. Normality (N) Normality of a solution is defined as the number of gram-equivalents of solute present per
litre of solution.
Number of gram − equivalents of solute
Normality =
Volume of solution (in litres)
Mass of solute in grams per litre of solution
N=
Equivalent mass of the solute
W 1
=
N ×
E V(sol ) (litre)
W = Mass of solute in gram, E = Gram-equivalent mass of solute
V(sol) = Volume of solution in litre.
5. Titrant : The solution which is generally taken in burette is called titrant.
6. Titer : The solution which is generally taken in conical flask with the help of pipette is called titer.
7. Equivalence Point: The point at which the titrant and titer react completely is called the equivalence
point.
8. End Point : The point at which the solution used in titration react completely and is indicated by the
indicator by changing its colour, is called the end point.
There is a difference of 1 drop in equivalence point and the end point.
9. Indicator : The chemical substances which when added to titer during titration indicate the completion of
the reaction by changing its colour at the end point are called indicators.
Types of Indicators : Depending upon the nature of the solution used in titration, indicators are divided
into four types.
(a) Internal Indicator : The indicators which are added to the titer during titration are called internal
indicators e.g. Methyl orange, phenolphthalein etc.
Methyl orange : Methyl orange is a weak base and is yellow in colour in the unionised form.
The anion formed from the indicator is an active species, which on accepting a proton (i.e acting as
Bronsted Lowry base) changes from the benzenoid form to the quinonoid form. The quinonoid form
is deeper in colour and thus is responsible for the colour change at the end point.
Benzenoid form of the anion Quinonoid form of the anion
(Yellow in colour) (Pinkish red in colour)
Phenolphthalein : Phenolphthalein is a weak acid, therefore it does not dissociate in the acidic
medium and remains in the unionised form, which is colourless.
→ H + Ph¯
+
HPh
Unionised Ionised
Colourless Pink
In the acidic medium, equilibrium lies to the left. In the alkaline medium, the ionisation of
+
phenolphthalein increases considerably due to the constant removal of H ions released from HPh by
the OH¯ ions from the alkali. So the concentration of Ph¯ ion increases in the solution, which imparts
pink colour to the solution.
→
+
HPh H + Ph¯
→
+
NaOH Na + OH¯
→
+
H + OH¯ H2O
For a weak acid vs strong alkali titration, phenolphthalein is the most suitable indicator. This is so
because the last drop of added alkali brings the pH of the solution in the range in which
phenolphthalein shows sharp colour change
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