Tuesday, July 10, 2018



The Meaning of Qualitative Analysis
Explain 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
State 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:
  1. All the apparatus should be cleaned and dried thoroughly and must remain clean throughout the experiment.
  2. Do not lay a glass rod on a dirt laboratory bench as it can get contaminated easily.
  3. 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.
  4. 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.
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

Preliminary Test on an Unknown Sample
Carry out 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
GasColourSmellAction on litmusTest
CH3COOHColourlessVinegar-likeAcidicLiberated as dense white fumes
N2ColourlessOdourlessNeutralNo chemical test
Water vapourColourlessOdourlessNeutralTurns white CuSO4 blue
NO2Reddish-brownPungentAcidicNot as red as Br2 vapour and does not condense on the sides of the test tube
NH3ColourlessPungentAlkalineForms thick white fumes when in contact with HCl gas
HClWhite fumesIrritatingAcidicForms thick white fumes when in contact with NH3 gas
HBr & Br2White fumes & reddish- brown gasChokingAcidic & bleachesHBr resembles HCl, & Br2, condenses to a red liquid on the sides of the test tube
Cl2Pale greenBleachesChokingGives white fumes with NH4OH
I2VioletChokingBleachesTurns starch iodide paper blue-black
CO2ColourlessOdourlessSlightly acidicTurns lime water milky
COColourlessOdourlessNeutralBurns with pale blue flame
H2ColourlessOdourlessNeutralBurns with a „pop‟ sound
H2SColourlessRotten eggsAcidicBurns with blue flame to SO2, blackens lead acetate paper.
O2ColourlessOdourlessNeutralRe-ignites a glowing splint
SO2ColourlessIrritating smell of burning sulphurAcidicDecolourizes KMnO4 solution, turns K2Cr2O7 from orange to green
SO3ColourlessPungentAcidicFumes 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
Prepare 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 1 cm3 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
  • 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.
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
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.
  1. Potassium hexacyanoferrate (II) solution
  2. Potassium hexacyanoferrate (III) solution
  3. 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