Q. No.The reagents, \(NH_4Cl\) and aqueous \(NH_3\), will precipitate:
1. \(Ca^{2+}\)
2. \(Al^{3+}\)
3. \(B i^{3+}\)
4. \(Mg^{2+} \)
Subtopic: Detection of Cations |
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Which of the following reagents can be used to distinguish between sulphite and sulphate ions present in a solution?
1. \(FeSO_4\)
2. \(Na_2[FeI(CN)_5NO] \)
3. \(BaCl_2 \)
4. \(Na_3[Co(NO_2)6] \)
1. \(FeSO_4\)
2. \(Na_2[FeI(CN)_5NO] \)
3. \(BaCl_2 \)
4. \(Na_3[Co(NO_2)6] \)
Subtopic: Detection of Anions |
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\(Na_2CO_3 \) cannot be used in place of \((NH_4)_2CO_3 \) for the precipitation of fifth group radicals.
This is because:
1. Magnesium will precipitate
2. The concentration of carbonate ions is very low
3. Sodium ions will react with acidic radicals
4. \(Na^{+} \) ions interfere with the detection of the fifth group
This is because:
1. Magnesium will precipitate
2. The concentration of carbonate ions is very low
3. Sodium ions will react with acidic radicals
4. \(Na^{+} \) ions interfere with the detection of the fifth group
Subtopic: Detection of Cations |
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A metal sulphate (A) on heating evolves two gases (B) and (C) and an oxide (D).
Gas (B) turns \(K_2Cr_2O_7\) paper green while gas (C) forms a trimer in which there
is no \(S-S\) bond. Oxide (D) with conc. \(HCl\) forms a Lewis acid (E) which exists
in a dimer. Compounds (A), (B), (C), (D) and (E), respectively, are:
1. \(FeSO_4, SO_2,Fe_2O_3,FeCl_3\)
2. \(Al_2(SO_4)_3,SO_2,SO_3,Al_2O_3,FeCl_3\)
3. \(FeS,SO_2,SO_3,FeSO_4,FeCl_3\)
4. \(FeS,SO_2,SO_3,Fe_2(PO_4)_3,FeCl_2\)
Gas (B) turns \(K_2Cr_2O_7\) paper green while gas (C) forms a trimer in which there
is no \(S-S\) bond. Oxide (D) with conc. \(HCl\) forms a Lewis acid (E) which exists
in a dimer. Compounds (A), (B), (C), (D) and (E), respectively, are:
1. \(FeSO_4, SO_2,Fe_2O_3,FeCl_3\)
2. \(Al_2(SO_4)_3,SO_2,SO_3,Al_2O_3,FeCl_3\)
3. \(FeS,SO_2,SO_3,FeSO_4,FeCl_3\)
4. \(FeS,SO_2,SO_3,Fe_2(PO_4)_3,FeCl_2\)
Subtopic: Detection of Cations |
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In this sequence, X, Y, Z are, respectively,:
1. Acidified \(H_2O_2;\) Alkaline \(H_2O_2;\) Acidified \(H_2O_2\)
2. Alkaline \(H_2O_2;\) Acidified \(H_2O_2;~Zn/HCl.\)
3. Acidified \(H_2O_2;\) Heat; Alkaline \(H_2O_2\)
4. Alkaline \(H_2O_2;\) Acidified \(H_2O_2;\) on standing
1. Acidified \(H_2O_2;\) Alkaline \(H_2O_2;\) Acidified \(H_2O_2\)
2. Alkaline \(H_2O_2;\) Acidified \(H_2O_2;~Zn/HCl.\)
3. Acidified \(H_2O_2;\) Heat; Alkaline \(H_2O_2\)
4. Alkaline \(H_2O_2;\) Acidified \(H_2O_2;\) on standing
Subtopic: Detection of Cations |
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Aqueous solution of a salt when treated with \(AgNO_3\) solution gives a white precipitate, which dissolves in \(NH_4OH.\)
The ion present in the salt is:
1. \(Cl^-\)
2. \(NO_3^-\)
3. \(I^-\)
4. All the av
The ion present in the salt is:
1. \(Cl^-\)
2. \(NO_3^-\)
3. \(I^-\)
4. All the av
Subtopic: Detection of Anions |
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Ammonium dichromate is used in some fireworks. The green-coloured powder blown in the air is due to:
1. \(CrO_3 \)
2. \(Cr_2O_3 \)
3. \(Cr\)
4. \(CrO(O_2) \)
1. \(CrO_3 \)
2. \(Cr_2O_3 \)
3. \(Cr\)
4. \(CrO(O_2) \)
Subtopic: Detection of Cations |
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A white precipitate obtained in the analysis of a mixture becomes black on treatment with \(\mathrm{NH_4OH}.\) It may be:
1. \(\mathrm{PbCl_2}\)
2. \(\mathrm{AgCl}\)
3. \(\mathrm{HgCl_2}\)
4. \(\mathrm{Hg_2Cl_2}\)
1. \(\mathrm{PbCl_2}\)
2. \(\mathrm{AgCl}\)
3. \(\mathrm{HgCl_2}\)
4. \(\mathrm{Hg_2Cl_2}\)
Subtopic: Detection of Cations |
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On adding \(KI\) solution in excess to a solution of \(CuSO_4\) we get a precipitate 'P and another liquor M. Select the correct pairs:
1. P is \(Cu_2I_2 \) and M is \(I_2\) solution
2. P is \(CuI_2 \) and M is \(I_2\) solution
3. P is \(Cu_2I_2 \) and M is \(KI_3\) solution
4. P is \(CuI_2 \) and M is \(KI_3\) solution
1. P is \(Cu_2I_2 \) and M is \(I_2\) solution
2. P is \(CuI_2 \) and M is \(I_2\) solution
3. P is \(Cu_2I_2 \) and M is \(KI_3\) solution
4. P is \(CuI_2 \) and M is \(KI_3\) solution
Subtopic: Detection of Anions |
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Consider the following sequence of tests:
\(M^{n+} ~+ HCl \rightarrow \) White precipitate \(\xrightarrow \Delta \) water soluble
The metal ion \((M^{n+})\)) can be:
1. \(Hg^{2+}\)
2. \(Ag^{+}\)
3. \(Pb^{2+}\)
4. \(Sn^{2+}\)
\(M^{n+} ~+ HCl \rightarrow \) White precipitate \(\xrightarrow \Delta \) water soluble
The metal ion \((M^{n+})\)) can be:
1. \(Hg^{2+}\)
2. \(Ag^{+}\)
3. \(Pb^{2+}\)
4. \(Sn^{2+}\)
Subtopic: Detection of Cations |
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