Viva Questions with Answers on Qualitative Analysis.

Chemistry Lab ManualNCERT Solutions Class 11 Chemistry Sample Papers

1. What is qualitative analysis ?
Ans. The type of analysis that deals with the methods which are used to determine the constituents of a compound.
2. What is a radical ?
Ans. A radical may be defined as an atom or group of atoms which carries charge and behaves as a single unit in chemical reactions.
3. What are acidic and basic radicals ?
Ans. Radicals carrying positive charge are called basic radicals and those carrying negative charge are called acidic radicals.
4. What type of bond is present in an inorganic salt ?
Ans. Electrovalent bond.
5. Why do inorganic salts ionise when dissolved in water ?
Ans. Due to the high dielectric constant of water, the force of attraction holding the two ions in a salt decreases. Thus, the two ions separate. The ions are further stabilized by solvation.
6. Give examples of some coloured basic radicals.
Ans.Cu²⁺,Fe²⁺,  Fe³⁺, Cr³⁺, Ni²⁺, Co²⁺ and Mn²⁺.
7. What is the colour of iron salts ?
Ans. Ferrous salts are usually light green while ferric salts are generally brown.
8. Name any iron salt which is light green.
Ans. Ferrous sulphate.
9. What is the colour of nickel salts ?
Ans. Bluish green or green.
10. What is the colour of manganese salts ?
Ans. Light pink or flesh colour.
11. Name the basic radicals which are absent, if the given salt is white.
Ans. Cu²⁺,Fe²⁺,  Fe³⁺, Cr³⁺, Ni²⁺, Co²⁺ and Mn²⁺. 
12.Why a salt containing lead turn black in colour, when placed for a long time in labora-tory?
Ans. Due to the formation of black lead sulphide by the action of H₂S in atmosphere.
13. Name the salts which produce crackling sound when heated.
Ans. Lead nitrate, barium nitrate, potassium bromide, sodium chloride.
14. What is sublimation ?
Ans. It is the process by which a salt directly changes into gaseous phase without melting, when heated. On cooling vapours condense back to the solid state.
15. Tell the importance of preliminary tests in qualitative analysis.
Ans. Sometimes, preliminary tests give authentic information about an ion in the salt. For example, golden yellow colour in flame test shows the presence of sodium. In a charcoal cavity test, brown residue shows the presence of cadmium in a salt and so on.
16. How is dry heating test performed and what information you get if the residue changes to yellow when hot ?
Ans. In dry heating test, the salt is heated in a dry test tube. Yellow residue when hot shows the presence of Zn²⁺ ion.
17. What is the expected observation when copper sulphate is heated in a dry test tube ? Ans. A white residue is formed and water condenses on the colder walls of the test tube.
18. Name the radical which produces CO₂ on heating.
Ans. Carbonate.
19. What is the colour of residue when zinc salt is heated ?
Ans. A residue yellow when hot and white when cold is formed.
20. What is the colour of residue when cadmium salt is heated ?
Ans. A residue brown when hot, brown when cold.
21. If the residue in dry heating test is white, name the radicals which are absent.
Ans. Cu²⁺, Mn²⁺, Co²⁺, Cr³⁺, Zn²⁺ and Pb²⁺.
22. How is charcoal cavity test performed ? Describe the chemistry for the formation of incrustation as well as metallic bead.
Ans. The salt is mixed with the double the quantity of sodium carbonate and the mixture is heated in the charcoal cavity in luminous flame (reducing flame).

23. Which flame is used in charcoal cavity test ? How is it obtained ?
Ans. A reducing flame is used in charcoal cavity test. It is obtained by closing the air holes of the burner.
24. Why should we avoid excess of cobalt nitrate in cobalt nitrate test ?
Ans. Excess of cobalt nitrate is avoided because it forms black cobalt oxide in the oxidising flame. This colour masks the other colours which might be produced during the test.
25. In the flame test, sodium imparts yellow colour to the flame while magnesium does not impart any colour. Why ?
Ans. In case of magnesium, when the excited electron jumps back to the ground state, the frequency of radiation emitted does not fall in the visible region.
26. Write the chemistry of flame test.
Ans. In flame test, the valence electron of the atom gets excited and jumps to the higher level. When the electron jumps back to the ground state, the radiation is emitted whose frequency falls in the visible region.
27. What is the function of blue glass in flame test ?
Ans. The blue glass can absorb a part or whole of the coloured light in certain cases. Therefore, the flame appears to be of different colour when viewed through blue glass. This helps in identification of some basic radicals.
28. Why do we use cone. HCl in preparing a paste of the salt for flame test ?
Ans. In order to convert metal salts into metal chlorides which are more volatile than other salts.
29. Why can’t we use glass rod instead of platinum wire for performing flame test ?
Ans. This is because glass contains sodium silicate which imparts its own golden yellow colour to the flame.
30. Why is platinum metal preferred to other metals for flame test ?
Ans. Because platinum does not react with acids and does not itself impart any characteristic colour to the flame.
31. Why do barium salts not impart colour to the flame immediately ?
Ans. Because barium chloride is less volatile, it imparts colour to the flame after some time.
32. Why should we avoid the use of platinum wire for testing lead salts ?
Ans. Because lead combines with platinum and the wire gets corroded.
33. Why should only a particle or two of the given salt should be touched with the bead in borax bead test ?
Ans. If salt is used in excess an opaque bead is formed.
34. Why borax bead test is not applicable in case of white salts ?
Ans. White salts do not form coloured meta-borates.
35. What is Nessler’s Reagent ?
Ans. It is a solution of mercuric iodide in potassium iodide. Its formula is K₂[HgI₄].
36. Name the acid radicals detected with dil. H₂SO₄.
Ans. CO₃^2-, S^2-, SO₃^2-, NO₂^–.
37. Why dil. H₂SO₄ is preferred while testing acid radicals over dil. HCl ?
Ans. When the salt is treated with HCl, during reaction HCl gas is also given out along with the gas evolved by the salt. So the actual gas cannot be identified whereas with H₂SO₄, no such problem arises.
38. Name the acid radicals detected by cone. H₂SO₄.
Ans. Cl^–, Br^–, I^–, NO₃^–, CH₃COO^–.
39. Name the radicals which are tested with the help of water extract.
Ans. NO₃^–, NO₂^– and CH₃COO^–.
40. Name the radicals which are confirmed with the help of sodium carbonate extract.
Ans. S^2-, Cl^–, Br^–, I^–, PO₄^3-, SO₃^2-, SO₄^2-.
41. How is sodium carbonate extract prepared ?
Ans. The salt is mixed with double the amount of solid Na₂CO3 and about 20 ml of distilled water. It is then boiled till it is reduced to one-third, and then filtered. The filtrate is sodium carbonate extract or (S.E.).
42. What is water extract ?
Ans. The given salt or mixture is shaken well with distilled water and the solution is filtered. The filtrate is water extract or (W.E.).
43. CO₂ and SO₂ both turn lime water milky. How will you distinguish between them ?
Ans. By passing through acidified K₂Cr₂O₇ solution. SO₂ turns K₂Cr₂O₇ green while CO₂ has no effect.
44. CO₂ and Br₂ both are brown in colour. How will you distinguish between them ?
Ans. By passing through FeSO₄ solution. NO₂ turns FeSO₄ soln. black while Br₂ has no effect.
45. How will you test the presence of carbonate ?
Ans. Treat a small quantity of the mixture with dil. H₂SO₄. CO₂ gas is evolved. When the gas is passed through lime water, it is turned milky.

46. What is lime water ?
Ans. A solution of Ca(OH)₂ in water is called lime water.
47. What will happen if excess of CO₂ is passed through lime water ?
Ans. The white ppt. of CaCO₃ changes into soluble calcium bicarbonate and the milkiness, therefore, disappears.

48. How do you test for sulphide ?
Ans. Warm the salt with dil. H₂SO₄. H₂S gas is evolved. It turns a paper dipped in lead acetate black.
49. Is there any gas other than CO₂ which turns lime water milky ?
Ans. Yes, it is SO₂ gas.
50. All nitrates on heating with cone. H₂SO₄ in presence of paper pallet evolve NO₂ gas. What is the function of paper pallet ?
Ans. Paper pallet (carbon) reduces HNO₃ to NO₂ 
51. How will you test whether the given solution in a bottle is lime water ?
Ans. Take 2 ml of the solution in a test tube and blow into it by means of a glass tubing. Milkiness indicates that the solution is lime water.
52. How is ring test performed for nitrates ?
Ans. To the salt solution, freshly prepared ferrous sulphate solution is added and then sulphuric acid (cone.) is added along the walls of the tube. A dark brown ring is formed at the junction of the two solutions.
53. Why the hot reaction mixture in case of cone. H₂SO₄ test is not thrown into the sink ? Ans. In order to avoid spurting, due to which H₂SO₄ may fly and spoil clothes and may result into serious injuries.
54. What is Tollen’s reagent ?
Ans. Ammonical AgNO₃ solution is called Tollen’s reagent.
55. Give formula of Diphenylamine reagent.
Ans. (C₆H₅)₂ NH.
56. Why a dark brown ring is formed at the junction of two layers in ring test for nitrates ?
Ans. H2S04 being heavier forms the lower layer and reacts only with a small amount of nitrate and FeS04 at its surface, therefore, a brown ring appears only at the junction of the two layers.
57. Why acetic acid is added before adding lead acetate solution ?
Ans. In order to prevent the hydrolysis of lead acetate which would yield white precipitate of lead hydroxide.
58. What is the formula of Sodium nitroprusside ?
Ans. Na₂[Fe(CN)₅ NO].
59. What is chromyl chloride test ?
Ans. Heat a small amount of the mixture with cone. H₂SO₄ and solid K₂Cr₂O₇ in a dry test tube. Deep brownish red vapours of chromyl chloride are formed. Pass these vapours in water. A yellow sol. of H₂CrO₄ is formed. Add to this solution NaOH, acetic acid and lead acetate, a yellow ppt. confirms chloride in the mixture.

60. What is the chemistry of carbon disulphide test for a bromide or iodide ?
Ans. To a part of the soda extract add dil. HCl. Now to this add small amount of CS₂ and excess of chlorine water and shake the solution well. Chlorine displaces bromine or iodine from the bromide or iodide, which dissolves in carbon disulphide to produce orange or violet colouration.
61. Why do bromides and iodides not respond to chromyl chloride test ?
Ans. Because chromyl bromide (CrO₂Br₂) and chromyl iodide (CrO₂I₂) compounds are not formed, instead of these bromine and iodine are evolved.
62. Describe the chemistry of match stick test.
Ans. In match stick test, the sulphate is reduced to sulphide by carbon of match stick which then gives violet colour with sodium nitroprusside solution.
63. Why does iodine give a blue colour with starch solution ?
Ans. The blue colour is due to the physical adsorption of iodine upon starch.
64. What is Nessler’s Reagent ?
Ans. Nessler’s reagent is K₂[HgI₄], Potassium tetraiodomercurate (II). It is used for detecting ammonia and ammonium ions.
65. Name a cation which is not obtained from a metal.
Ans. Ammonium ion (NH₄⁺).
66. What is aqua regia ?
Ans. Aqua regia is a mixture of concentrated HCl and concentrated HNO₃ in the ratio 3:1 by volume.
67. What is the name of the product obtained when NH₄⁺ ions are reacted with Nessler’s Reagent ?
Ans. Basic mercure (II) amido-iodine, HgO . Hg(NH₂)I. Its common name is iodide of Millon’s base.
68. Why O.S. is not prepared in cone. HNO₃ ?
Ans. HNO₃ is an oxidising agent which on decomposition gives oxygen. A yellow ppt. of sulphur is obtained in presence of HNO₃ when H₂S is passed.
69. Why is original solution for cations not prepared in concentrated H₂SO₄ ?
Ans. H₂SO₄ would lead to precipitation of cations of group V as sulphates.
70. Name group reagents for different groups.
Ans. Group I—Dil. HCl.
Group II—H₂S in the presence of dil. HCl.
Group III—NH4OH in presence of NH4Cl.
Group IV—H2S in presence of NH4OH.
Group V—(NH₄)₂ CO₃ in presence of NH4Cl and NH4OH.
Group VI—No specific group reagent.
71. Why is it essential to add dil. HCl before proceeding to the test for the basic radicals of group II ?
Ans. In the precipitation of group II cations as their sulphides. H₂S is used in the presence of dil. HCl. H₂S is itself a weak acid and dissociates as follows :
Hydrochloric acid being a strong acid is largely ionised to H⁺. Thus, hydrogen ion concentration is increased and consequently the concentration of sulphide ions produced by the ionisation of H₂S is sufficiently decreased due to common ion effect. As a result of which the sulphide ion concentra¬tion is sufficient only to exceed the solubility product of the sulphides of group II cations.
Since the solubility products (Ksp) for the sulphides of groups III and IV cations are very high, those cations are not precipitated out under the above conditions.
72. Why is it essential to boil off H₂S gas before precipitation of radicals of group III ?
Ans. Before precipitation of group III cations, the solution is boiled with cone, nitric acid. If H₂S is not boiled off then it would react with HNO₃ and would be oxidized to colloidal sulphur, which would interfere with further analysis.
73. Why is the O.S. boiled with cone. HNO₃ in III group ?
Ans. In the presence of NH4Cl, Fe(OH)₂ is not completely precipitated because of its high solubility product. For this reason Fe⁺⁺ salts are oxidised to Fe⁺⁺⁺ salts by boiling with cone. HNO₃ before adding NH4Cl and NH4OH ; otherwise Fe⁺⁺ would not be completely precipitated in III group.
74. Why is NH4Cl added along with NH4OH in III group ?
Ans. It is done in order to decrease the concentration of OH^– ions by suppressing the ionisation of NH4OH by common ion effect. If NH4OH alone is used in that case, the concentration of OH^– is enough to ppt. the hydroxide of IV, V and VI groups.
75. What is blue lake ?
Ans. It is blue particles, blue litmus adsorbed on white ppt. of Al(OH)3, floating in colourless solution.
76. H₂S gas is passed in presence of NH4OH in group IV. Explain why ?
Ans. When H₂S gas is passed in alkaline medium or NH4OH, the H⁺ ions from the dissociation of H₂S gas combine with hydroxyl ions (OH^–) from the dissociation of NH4OH to form nearly unionised H₂O.
The removal of H⁺ ions from the solution causes more of H₂S to dissociate, thereby increasing the concentration of S^2- ions to such an extent that the ionic product of IV group metal sulphides exceeds their solubility product. Hence they are precipitated.
77. Presence of NH4Cl is quite essential before the addition of (NH4)2 COs in group V. Explain why ?
Ans. Ammonium chloride suppresses the ionisation of NH4OH and (NH₄)₂ CO₃ due to common ion effect which results in the decrease in the concentration of OH^– and CO₃^2- ions. So the ionic product does not exceed the solubility product of Mg(OH)₂ or MgCO₃ and thereby they are not precipitated in V group.
78. Why are the group V radicals tested in the order Ba²⁺,  Sr²⁺and Ca²⁺ ?
Ans. Tests of Sr²⁺ and Ca²⁺ are given by Ba²⁺ also. Similarly tests of Ca²⁺ are given by Sr²⁺ also. Therefore before confirming Sr²⁺ we have to show absence of Ba²⁺ and before confirming Ca²⁺ we have to show absence of Ba²⁺ and Sr²⁺.
79.  Na2CO₃ cannot be used in place of (NH₄)₂ CO₃ in the group V. Explain why ?
Ans. Na2CO₃ is highly ionised electrolyte, which produces very high cone, of CO₃^2- ions. As a result ionic product of MgCO₃ may increase its Ksp and it may get precipitated along with the radicals of V group.
80. How will your prepare chlorine water ?
Ans. Take cone. HCl in a test tube and add KMnO4 soln. dropwise till the pink colour starts persisting. Now add a few drops of cone. HCl so that pink colour disappears. The colourless solution thus obtained is chlorine water.
81. Can we use ammonium sulphate in place of ammonium chloride in group III precipitation ?
Ans. No, ammonium sulphate cannot be used because it would cause precipitation of group V radicals as their sulphates in group III.
82. Why does cone. HNO₃ kept in a bottle turn yellow in colour ?
Ans. This is due to formation of NO by decomposition of HNO₃ which is further oxidized to NO2. Yellow colour in due to dissolved to NO2.