JEE Chemistry Qualitative Salt Analysis MCQs Set 03

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Multiple Choice Questions

Question 1: On mixing two colourless gases, a deep brown colour is observed. The gases are
(a) \( \ce{N2O} \) and \( \ce{O2} \)
(b) \( \ce{NO} \) and \( \ce{O2} \)
(c) \( \ce{N2O3} \) and \( \ce{O2} \)
(d) none of these
Show Answer & Explanation

Answer: (b) \( \ce{NO} \) and \( \ce{O2} \)

Explanation:
1. \( \ce{2NO + O2 -> 2NO2} \).
2. Nitrogen dioxide is brown.

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 2: Which of the following metals will give a blue ash when its salt is heated with solid \( \ce{Na2CO3} \) and \( \ce{Co(NO3)2} \) on a charcoal piece?
(a) Zn
(b) Cu
(c) Mg
(d) Al
Show Answer & Explanation

Answer: (d) Al

Explanation:
1. Aluminium oxide forms Thenard's blue (\( \ce{CoAl2O4} \)) on heating with cobalt nitrate.
2. Zinc gives a green ash and Mg gives pink.

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 3: Which one among the following pairs of ions cannot be separated by \( \ce{H2S} \) in dilute hydrochloric acid?
(a) \( \ce{Ni^{2+}, Cu^{2+}} \)
(b) \( \ce{Bi^{3+}, Sn^{4+}} \)
(c) \( \ce{Zn^{2+}, Cu^{2+}} \)
(d) \( \ce{Al^{3+}, Hg^{2+}} \)
Show Answer & Explanation

Answer: (b) \( \ce{Bi^{3+}, Sn^{4+}} \)

Explanation:
1. Both Bi(III) and Sn(IV) precipitate as sulphides in group II, so they cannot be separated.
2. In the other pairs one ion precipitates and the other stays in solution.

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 4: Nessler's reagent is used to detect
(a) \( \ce{NH4^+} \)
(b) \( \ce{CrO4^{2-}} \)
(c) \( \ce{MnO4^-} \)
(d) \( \ce{PO4^{3-}} \)
Show Answer & Explanation

Answer: (a) \( \ce{NH4^+} \)

Explanation:
1. Nessler's reagent gives a brown precipitate or colour with ammonium ions.

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 5: The metal that does not give the borax-bead test is
(a) manganese
(b) lead
(c) chromium
(d) nickel
Show Answer & Explanation

Answer: (b) lead

Explanation:
1. Cr, Ni and Mn form coloured metaborate beads.
2. Lead gives no characteristic coloured bead.

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 6: A substance [X] on treatment with dil. \( \ce{H2SO4} \) gives a colourless gas [Y] with an irritating smell. [Y] + \( \ce{K2Cr2O7} \) + \( \ce{H2SO4} \) gives a green solution. [X] and [Y] are
(a) \( \ce{CO3^{2-}} \), \( \ce{CO2} \)
(b) \( \ce{Cl^-} \), HCl,
(c) \( \ce{SO3^{2-}} \), \( \ce{SO2} \)
(d) \( \ce{S^{2-}} \), \( \ce{H2S} \)
Show Answer & Explanation

Answer: (c) \( \ce{SO3^{2-}} \), \( \ce{SO2} \)

Explanation:
1. Sulphite gives pungent \( \ce{SO2} \), which reduces orange dichromate to green \( \ce{Cr^{3+}} \).

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 7: To an inorganic mixture dil. \( \ce{H2SO4} \) is added in the cold; a colourless, odourless gas is evolved. The mixture contains
(a) nitrite
(b) sulphite
(c) carbonate
(d) acetate
Show Answer & Explanation

Answer: (c) carbonate

Explanation:
1. Carbonate gives colourless odourless \( \ce{CO2} \).
2. Sulphite gives pungent \( \ce{SO2} \), acetate gives vinegar smell, nitrite gives brown fumes.

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 8: \( \ce{Pb^{2+}} \), \( \ce{Cu^{2+}} \), \( \ce{Zn^{2+}} \) and \( \ce{Ni^{2+}} \) ions are present in a given acidic solution. On passing hydrogen sulphide gas through this solution, the available precipitate will contain
(a) \( \ce{PbS} \) and \( \ce{CuS} \)
(b) \( \ce{CuS} \) and \( \ce{NiS} \)
(c) \( \ce{PbS} \) and \( \ce{NiS} \)
(d) \( \ce{CuS} \) and \( \ce{ZnS} \)
Show Answer & Explanation

Answer: (a) \( \ce{PbS} \) and \( \ce{CuS} \)

Explanation:
1. In acid, only group II sulphides (PbS and CuS) are precipitated; ZnS and NiS need a basic medium.

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 9: Which of the following sulphates is insoluble in water?
(a) \( \ce{CuSO4} \)
(b) \( \ce{Bi2(SO4)3} \)
(c) \( \ce{CdSO4} \)
(d) \( \ce{PbSO4} \)
Show Answer & Explanation

Answer: (d) \( \ce{PbSO4} \)

Explanation:
1. Lead sulphate is a white insoluble salt.

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 10: When concentrated \( \ce{H2SO4} \) is added to dry \( \ce{KNO3} \), brown fumes evolve. These fumes are
(a) \( \ce{SO2} \)
(b) \( \ce{NO} \)
(c) \( \ce{NO2} \)
(d) \( \ce{SO3} \)
Show Answer & Explanation

Answer: (c) \( \ce{NO2} \)

Explanation:
1. Nitric acid formed decomposes (and is partly reduced), producing brown \( \ce{NO2} \).

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 11: Sodium nitroprusside, when added to an alkaline solution of sulphide ions, produces a purple colour ion due to the formation of
(a) \( \ce{Na[Fe(H2O)5NOS]} \)
(b) \( \ce{Na3[Fe(CN)5NOS]} \)
(c) \( \ce{Na4[Fe(CN)5NOS]} \)
(d) \( \ce{Na2[Fe(H2O)5NOS]} \)
Show Answer & Explanation

Answer: (c) \( \ce{Na4[Fe(CN)5NOS]} \)

Explanation:
1. Sulphide attacks the nitrosyl group of nitroprusside to give the purple complex \( \ce{Na4[Fe(CN)5NOS]} \).

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 12: An aqueous solution of a salt when treated with \( \ce{AgNO3} \) solution gives a white precipitate, which dissolves in \( \ce{NH4OH} \). The radical present in the salt is
(a) \( \ce{Cl^-} \)
(b) \( \ce{NO3^-} \)
(c) \( \ce{Br^-} \)
(d) \( \ce{I^-} \)
Show Answer & Explanation

Answer: (a) \( \ce{Cl^-} \)

Explanation:
1. White AgCl is soluble in ammonia; AgBr is pale yellow and AgI yellow.

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 13: When \( \ce{H2S} \) gas is passed through HCl containing aqueous solutions of \( \ce{CuCl2} \), \( \ce{HgCl2} \), \( \ce{BiCl3} \) and \( \ce{CoCl2} \), which does not precipitate out?
(a) \( \ce{CoS} \)
(b) \( \ce{Bi2S3} \)
(c) \( \ce{HgS} \)
(d) \( \ce{CuS} \)
Show Answer & Explanation

Answer: (a) \( \ce{CoS} \)

Explanation:
1. CoS has a high solubility product and needs a basic medium; it does not precipitate in acid.

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 14: When a dilute aqueous solution of \( \ce{AgNO3} \) (excess) is added to KI solution, positively charged sol particles of AgI are formed due to adsorption of the ion
(a) \( \ce{O2^-} \)
(b) \( \ce{NO3^-} \)
(c) \( \ce{Ag^+} \)
(d) \( \ce{K^+} \)
Show Answer & Explanation

Answer: (c) \( \ce{Ag^+} \)

Explanation:
1. A colloid preferentially adsorbs the ion common to it, here \( \ce{Ag^+} \) from the excess reagent.

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 15: In the chromyl chloride test, the reagent used is
(a) \( \ce{K2CrO4} \)
(b) \( \ce{CrO3} \)
(c) \( \ce{K2Cr2O7} \)
(d) \( \ce{(NH4)2Cr2O7} \)
Show Answer & Explanation

Answer: (c) \( \ce{K2Cr2O7} \)

Explanation:
1. Solid chloride is heated with \( \ce{K2Cr2O7} \) and conc. \( \ce{H2SO4} \) to give red vapours of chromyl chloride.

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 16: A white sodium salt dissolves readily in water to give a solution which is neutral to litmus. When silver nitrate solution is added to the solution, a white precipitate is formed which does not dissolve in dilute nitric acid. The anion could be
(a) \( \ce{S^{2-}} \)
(b) \( \ce{SO4^{2-}} \)
(c) \( \ce{Cl^-} \)
(d) \( \ce{CO3^{2-}} \)
Show Answer & Explanation

Answer: (c) \( \ce{Cl^-} \)

Explanation:
1. A neutral sodium salt rules out carbonate and sulphide (basic).
2. White AgCl is insoluble in dilute nitric acid; silver sulphate would not give such a precipitate.

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 17: Which of the following pairs of ions, when mixed in dilute solutions, may give a precipitate?
(a) \( \ce{Na^+, SO4^{2-}} \)
(b) \( \ce{Fe^{3+}, PO4^{3-}} \)
(c) \( \ce{Na^+, S^{2-}} \)
(d) \( \ce{NH4^+, CO3^{2-}} \)
Show Answer & Explanation

Answer: (b) \( \ce{Fe^{3+}, PO4^{3-}} \)

Explanation:
1. \( \ce{FePO4} \) is insoluble.
2. Sodium salts and ammonium carbonate are soluble.

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 18: \( \ce{H2S} \) gas passed through a solution containing HCl precipitates the cations of group II but not those of the fourth group. It is because
(a) presence of HCl decreases the sulphide ion concentration
(b) sulphides of group IV cations are soluble in HCl
(c) presence of HCl increases the sulphide ion concentration
(d) solubility product of group II sulphides is more than that of group IV sulphides
Show Answer & Explanation

Answer: (a) presence of HCl decreases the sulphide ion concentration

Explanation:
1. The acid lowers \( \ce{[S^{2-}]} \) enough for the very insoluble group II sulphides to precipitate, but not the more soluble group IV sulphides.

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 19: Which of the following anions would decolourise acidified \( \ce{KMnO4} \) solution?
(a) \( \ce{SO4^{2-}} \)
(b) \( \ce{S^{2-}} \)
(c) \( \ce{CH3COO^-} \)
(d) \( \ce{NO3^-} \)
Show Answer & Explanation

Answer: (b) \( \ce{S^{2-}} \)

Explanation:
1. Sulphide is a reducing agent and reduces purple permanganate to colourless \( \ce{Mn^{2+}} \).

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 20: The gas which is absorbed by ferrous sulphate solution giving a blackish brown colour is
(a) N2
(b) CO
(c) NO
(d) NH3
Show Answer & Explanation

Answer: (c) NO

Explanation:
1. NO forms the dark brown nitrosyl complex with ferrous ions.

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 21: In qualitative analysis, in order to detect the second group basic radical, \( \ce{H2S} \) gas is passed in the presence of dilute HCl to
(a) increase the dissociation of the salt solution
(b) increase the dissociation of \( \ce{H2S} \)
(c) decrease the dissociation of \( \ce{H2S} \)
(d) decrease the dissociation of the salt solution
Show Answer & Explanation

Answer: (c) decrease the dissociation of \( \ce{H2S} \)

Explanation:
1. HCl supplies the common ion \( \ce{H^+} \), suppressing ionisation of \( \ce{H2S} \) so that only the least soluble sulphides of group II precipitate.

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 22: Neutral ferric chloride is added to the aqueous solution of acetate. The blood red colour obtained is due to the compound
(a) \( \ce{Fe(OH)2} \)
(b) \( \ce{Fe(OH)2(CH3COO)} \)
(c) \( \ce{Fe(CH3COO)3} \)
(d) \( \ce{Fe(OH)3} \)
Show Answer & Explanation

Answer: (c) \( \ce{Fe(CH3COO)3} \)

Explanation:
1. Ferric ions form the blood-red complex ferric acetate with acetate ions (the basis of the acetate test).

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 23: On addition of aqueous NaOH to a salt solution, a white gelatinous precipitate is formed which dissolves in excess alkali. The salt solution contains
(a) barium ions
(b) iron ions
(c) chromium ions
(d) aluminium ions
Show Answer & Explanation

Answer: (d) aluminium ions

Explanation:
1. Al(OH)3 is white and gelatinous and dissolves in excess NaOH as aluminate.
2. Chromium hydroxide is green, Ba(OH)2 is soluble and Fe hydroxides are brown or green.

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 24: An aqueous solution of a colourless metal sulphate M gives a white precipitate with NaOH. This was soluble in excess NaOH. On passing \( \ce{H2S} \) through this solution a white precipitate is formed. The metal M in the salt is
(a) Al
(b) Ca
(c) Ba
(d) Zn
Show Answer & Explanation

Answer: (d) Zn

Explanation:
1. Zn(OH)2 dissolves in excess NaOH as zincate, and \( \ce{H2S} \) then gives white ZnS.
2. Al would give white Al(OH)3 rather than a sulphide.

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

Question 25: Haemoglobin is a complex of
(a) \( \ce{Fe^{2+}} \)
(b) \( \ce{Fe^{4+}} \)
(c) \( \ce{Fe^{3+}} \)
(d) \( \ce{Cu^{2+}} \)
Show Answer & Explanation

Answer: (a) \( \ce{Fe^{2+}} \)

Explanation:
1. Haemoglobin contains Fe(II) in a porphyrin ring.

Teacher's Note:
1. Link each observation to its reagent: colour, gas evolved and precipitate are the usual clues in salt analysis.
2. Memorise the confirmatory test for each ion; they are asked repeatedly.

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