Home CHEMISTRY TOPIC 5: QUALITATIVE ANALYSIS | CHEMISTRY FORM 4

TOPIC 5: QUALITATIVE ANALYSIS | CHEMISTRY FORM 4

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TOPIC 5: QUALITATIVE ANALYSIS | CHEMISTRY FORM 4

The Meaning of Qualitative Analysis

Qualitative analysis involves determining metals and non metals (or metallic and non-metallic elements) present in a given sample. It is a process used to determine what elements (or radicals) are present in the sample.

Whereas quantitative analysis involves determining how much (quantity) of a substance is present in a sample, qualitative analysis involves
identifying what (quality) substances are present in a sample.

Qualitative analysis may be divided into examination of:

acidic or non-metallic radicals or negative ions;
basic or metallic radicals, including ammonium ion.

The Importance of Qualitative Analysis in Real Life

Qualitative analysis has numerous applications. The following are some applications (importance) of qualitative analysis in real life.

Detection of poisonous substances in the environment Sometimes it may be necessary to find out the chemical composition of

contaminants in the environment. This may require the application of qualitative analysis procedures to identify the chemical composition of a given contaminant. Qualitative analysis methods are highly employed by environmental scientists to detect and identify different contaminants in the environment.

Determination of ions present in a chemical substance

This is achieved through dissolution of a substance in distilled water. Then
the characteristics of the solution formed serve as a clue to establish
the type of elements present in a tested sample. The mixture formed
following dissolution of a solid sample may be a clear solution, an
emulsion or a precipitate. The solution or emulsion is further analysed
to detect the ions present in it. The precipitate is then separated from
the filtrate and both are subjected to further tests to identify the
kind of elements present.

Determination of the type of gases produced in a chemical reaction

Many chemical reactions are accompanied with evolution of gases, as one of
the products of the reaction. In some cases, the smell of the gas may
not suffice to detect the gas, especially if the gas is colourless and
odourless. In such cases, the gas is subjected to various qualitative
analysis tests in order to establish its identify.

Finding the nature and identity of chemical substances

The nature of a chemical substance such as its solubility in water,
characteristic smell, flame colour, and the characteristics of its
reaction products can be used to identify the chemical substance under
test. In this way, the nature and identity of unknown substance can ultimately be known.

SOIL ANALYSIS

Determination of soil pH

Soils of given pH give specific colours when their solutions are added to
certain types of indicators. This procedure is purely qualitative
because it involves observation of the change in colour of indicators to
determine the pH of the soil. For further details on the measurement of
soil pH, read a topic on Soil Chemistry (Chapter Three) in this book.

Determination of soil composition

Qualitative tests are performed to determine the type of minerals contained in a
particular soil. Such tests include test for nitrate, sulphate, chloride
and phosphate ions. Determination of soil composition gives soil
scientists information necessary for conservation.

Application in medical and criminology fields

Qualitative analysis techniques are applied in medical field, for example in
carrying out various tests such as testing blood and urine samples,
determining the level of blood sugar, pregnancy diagnose and blood
grouping. Most of these analytical tests are done to diagnose a wide
range of diseases and medical conditions.

For example:

in detecting the causative agents for typhoid (salmonella typhi), the
blood is left to clot, or it is centrifuged in order to separate blood
corpuscles from plasma. The plasma is then subjected to various
qualitative tests to detect the presence of salmonella typhi.

in pregnancy diagnosis, a certain chemical is added to urine, where a
specific change in colour of the urine confirms whether one is pregnant
or not.

Qualitative analysis is also applied in blood grouping, whereby antibodies are
added to the blood to determine the blood group. Agglutination of the
blood corpuscles when antibodies are added help detect the group of the
blood.

Forensic scientists may use qualitative chemical analysis to identify substances
left at crime scenes, which can be vital in convicting criminals.

Application in industries

Many industries use qualitative analysis in their efforts to perform better
and make quality products.In chemical industries, the products often get
contaminated by unknown contaminants. Qualitative tests are done to
detect the contaminants. This may be followed by quantitative analysis
aiming at finding out the quantity (amount) of the contaminant present.

Qualitative analysis techniques

It is very important to be very keen when performing qualitative analysis
tests. Just a small error can cause misinterpretation of the contents of
a tested sample. The following are few but important measures that
should be observed when carrying out qualitative analysis experiments.

Adding the reagent

After adding the test reagent, make sure the solution is stirred thoroughly.
Before making any inference, wait until the solution has completely
settled down. Often, additional quantities of the reagent must then be
added so that an excess is present.

Avoid contamination

Contamination of the sample or reagent should strictly be avoided. For instance, if
the contaminant contains a cation, the test can give misleading positive
results. To avoid contamination of the sample and apparatus, the following precautions should be observed:

All the apparatus should be cleaned and dried thoroughly and must remain clean throughout the experiment.

Do not lay a glass rod on a dirt laboratory bench as it can get contaminated easily.

Avoid touching the side of a test-tube with the tip of a dropper. The contaminant can be picked up and transferred to another solution, a fact that would contaminate the solution, thus producing false results.

Only distilled water from the wash bottle should be used to dissolve the solids. Spring, rain or tap water contains chemicals that can lead to wrong results and conclusions.

Warming up the solution

The solution is warmed by dipping the test-tube containing the solution in a
beaker of warm or boiling water (water bath). The test-tube is kept in a
water bath for some time, with constant stirring. Then, the solution is
tested for the presence of anions or cations contained in it.

Testing the pH of a solution

This is conducted by placing a litmus paper on a clean, dry surface and then
pouring a drop of the solution to be tested on it. The colour of the
paper is observed and noted while the paper is wet. Once dry, the colour
may change or disappear, resulting in wrong interpretation.

Qualitative Analysis Procedures

The procedures of qualitative analysis involve carrying out analytical
tests in the appropriate sequence of steps. The common procedures for
testing an unknown sample is to make its solution and then test this
solution for different ions present. The steps involved in the systemic
analysis of a given sample are as follows:

Preliminary tests

Colour and smell
Flame test
Solubility in water
Dry heating
Action on litmus (for gases evolved)

Tests for acid radicals (anions)

Dilute acid test (dilute H2SO4)
Concentrated acid test (concentrated H2SO4)
Wet test for acid radicals

Wet tests for basic radicals (cations)

Use special apparatus for qualitative analysis

Activity 1. Use special apparatus for qualitative analysis

Preliminary Test on an Unknown Sample

Preliminary tests include noting the appearance (colour, texture, feel, etc) of the
sample, detecting the smell of the gas liberated, observing the action
of a substance on litmus, and even the taste of the substance under
investigation. The preliminary tests give a clue about the type of the elements present in a sample.)

Table 5.2 Identification of gases

Gas	Colour	Smell	Action on litmus	Test
CH3COOH	Colourless	Vinegar-like	Acidic	Liberated as dense white fumes
N2	Colourless	Odourless	Neutral	No chemical test
Water vapour	Colourless	Odourless	Neutral	Turns white CuSO4 blue
NO2	Reddish-brown	Pungent	Acidic	Not as red as Br2 vapour and does not condense on the sides of the test tube
NH3	Colourless	Pungent	Alkaline	Forms thick white fumes when in contact with HCl gas
HCl	White fumes	Irritating	Acidic	Forms thick white fumes when in contact with NH3 gas
HBr & Br2	White fumes & reddish- brown gas	Choking	Acidic & bleaches	HBr resembles HCl, & Br2, condenses to a red liquid on the sides of the test tube
Cl2	Pale green	Bleaches	Choking	Gives white fumes with NH4OH
I2	Violet	Choking	Bleaches	Turns starch iodide paper blue-black
CO2	Colourless	Odourless	Slightly acidic	Turns lime water milky
CO	Colourless	Odourless	Neutral	Burns with pale blue flame
H2	Colourless	Odourless	Neutral	Burns with a „pop‟ sound
H2S	Colourless	Rotten eggs	Acidic	Burns with blue flame to SO2, blackens lead acetate paper.
O2	Colourless	Odourless	Neutral	Re-ignites a glowing splint
SO2	Colourless	Irritating smell of burning sulphur	Acidic	Decolourizes KMnO4 solution, turns K2Cr2O7 from orange to green
SO3	Colourless	Pungent	Acidic	Fumes in moist air forming dense white fumes

Colours of some ions in solution

The appearance of a substance in solid or solution form can help in its identification:

If a compound and its solution in water are colourless, it is probable that a transition metal is absent.

If its colour is black, it is probably an oxide or a sulphide.

If the solid and its solution in water are coloured, probably a transition metal is present.

The following are the colours of some transition element ions

Preparation of Stock Solutions from Soluble and Insoluble Salts

The solubilities of different compounds in water can be used in their identification. It is therefore important to know the solubilities of
different compounds

To test the solubility of a compound, put one spatula of the compound in 1cm3 of distilled water and stir. If the compound is soluble, this
amount will dissolve. If the compound is moderately soluble, some of this amount will dissolve. If the compound is insoluble, not even a
small amount will dissolve.

The following are some general rules on the solubility of different compounds in water:

All common nitrates of metals are soluble.

All common sodium, potassium and ammonium salts are soluble.

All common chlorides are soluble except those of silver, mercury (I) and lead (II).

All common sulphates are soluble except those of lead and barium. The sulphates of calcium and silver are sparingly soluble.

All carbonates, sulphites and phosphates of sodium, potassium, and ammonium are soluble but other common carbonates are insoluble.

Sodium, potassium and ammonium hydroxides [(ammonia solution, NH3(aq)]* are soluble but other common hydroxides are insoluble.

All sulphides are insoluble except those of the alkali metals, the alkaline earth metals and ammonium.

It is important to note that ammonium hydroxide does not exist. The
solution of ammonia in water (ammonia solution) is always wrongly termed
as ammonium hydroxide. Although the name ammonium hydroxide suggests an
alkali with the formula [NH4+][OH–], it is actually impossible to
isolate samples of NH4+ and OH– ions from a solution of ammonia in water
since the ions are negligibly very few in solution except in extremely
dilute solutions.

Action of heat on the original substance

Different substances decompose on heating to give different products. Many
compounds decompose on heating and leave solid residues. In performing
this test, the compound is heated in an ignition tube or dry test tube.
Heating is continued until no further change occurs. The gas evolved,
residue left or sublimate formed on heating may help to identify the
acid radical present in a compound.

Table 5.5 Action of heat on the test substance

Action of dilute sulphuric acid or dilute hydrochloric acid

Treat the solid with cold dilute sulphuric or hydrochloric acid. Identify the
gas evolved. If there is no reaction with the cold acid, heat the
mixture gently. Heat carefully and ensure the mixture does not boil. The
gas evolved can be identified as follows:

Table 5.6 Detection of acidic radicals

Action of concentrated sulphuric acid

As in the above test, the acid is added to the solid substance and if no
reaction occurs, the mixture is warmed gently, but the mixture should
not be boiled. Then, the gas given off is identified. In addition,
observe any product, other than the gas, which results from the reaction.

Table 5.7 Action of conc. H2SO4

Note:

Oxalates give CO2 with concentrated H2SO4 but not with. HCl.

Nitrates do not give NO2 when treated with HCl but nitrites give NO2 gas.

If no result is obtained in the above tests, the salt is probably a sulphate, chromate or phosphate.

Precipitation of Insoluble Salts from their Solutions

Precipitate insoluble salts from their solutions

Activity 2

Precipitate insoluble salts from their solutions

Cations and Anions Identifie

Confirm cations and anions identified

The detection of acidic radicals is important in that, in addition to other
information, it enables a clear-cut identification of the substance
being analysed. The substances are first dissolved in distilled water to make solutions. Then, the resulting solutions are tested for radicals.

Table 5.8 shows a list of test/experiments, each of which confirms the presence of a given ion. Depending on the availability of reagents, students can do any of the listed tests to confirm the ions present in test solutions.

Table 5.8 confirmatory tests for anions

TESTS FOR METALLIC RADICALS

Flame test

Some metal ions can be identified by the colour of their flame during a
flame test. Flame test involves mixing solutions of ions with conc. HCl
and then heating them on a platinum or nichrome wire over a non luminous
flame. Alternatively, a dry solid can be used instead of the
solution.To perform this experiment, dip a platinum or nichrome wire
into concentrated hydrochloric acid and hold it just above the blue part
of the flame. Repeat the process until the wire is clean. After that
dip the clean wire into the acid and the dip it into the solution of the
test substance (or its solid particles). Heat the substance strongly
and observe the colour of the flame formed.

The flame changes to a colour characteristics of the element. The following are characteristic flame colours of some metal ions.

Action of hydrochloric acid

Add dilute hydrochloric acid dropwise to the test solution until the
solution tests acidic to litmus paper. Observe for any reaction. A
precipitate will form with any cation that forms an insoluble chloride.
For example:

This can then be subjected to further tests to confirm the specific cation present in the solution.

Action of sulphuric acid

Add dilute sulphuric acid dropwise to the test solution until the solution is acidic. Observe for any reaction. A precipitate will form with any
cation that forms an insoluble sulphate. For example:

Action of sodium hydroxide

Add sodium hydroxide solution, a little at a time, to the test solution
until there is an excess of it. Stir or shake the mixture and observe
for any reaction. If no precipitate is formed, warm the mixture gently
and test for ammonia. If a precipitate forms, continue adding the sodium
hydroxide solution.

Table 5.9 Reaction of cations with dilute NaOH

Reaction equations:

The oxides of zinc, aluminium and lead are soluble in excess sodium
hydroxide. This is due to the amphoteric nature of the hydroxides of
these metals.

Action of aqueous ammonia

Add dilute aqueous ammonia to the test solution, drop by drop. Stir or
shake the mixture and observe for any reaction. If a ppt forms, continue adding aqueous ammonia.

Table 5.10 Reaction of cations with aqueous ammonia

An excess of aqueous ammonia dissolves the hydroxides of copper and zinc forming complex compounds of the metals:

Confirmatory tests for cations

After the preliminary tests have been performed, there is always a need to
carry out confirmatory tests to confirm the presence of cations in substances.

Table 5.11 Confirmatory tests for cations

Confirmatory tests for iron salts

The original test solution has to be divided into three portions. Then the solutions should be treated with the following reagents and the results recorded as shown in table 5.12.

Potassium hexacyanoferrate (II) solution

Potassium hexacyanoferrate (III) solution

Potassium thiocyanate solution

Table 5.12 Tests for iron salts

Table 5.13 Tests for bromides and iodides

Write-up of analytical data

All the observations made and any experimental data obtained during the
experiment (or test) must be presented in a tabular form a shown below.
Results presented in a table are concise, easy to read and understand.
The last column of the table gives the conclusions based on the
observations made.

Table 5.14 Table of results