Chapter 34

In the titration of a certain solution of a mixture of \(\mathrm{NaHCO}_{3}\) and \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) against \(\mathrm{HCl}, \mathrm{V}_{1} \mathrm{~mL}\) of \(\mathrm{HCl}\) is required with phenolphthalein as indicator and \(\mathrm{V}_{2} \mathrm{~mL}\) with methyl orange as indicator for the same volume of the titrated solution. Hence volume of \(\mathrm{HCl}\) for reaction of \(\mathrm{HCl}\) with \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) alone is (a) \(\mathrm{V}_{2} / 4 \mathrm{~mL}\) (b) \(2 \mathrm{~V}_{1} \mathrm{~mL}\) (c) \(\left(\hat{V}_{2}-\mathrm{V}_{1}\right) \mathrm{mL}\) (d) \(\left(\mathrm{V}_{1} / 3\right) \mathrm{mL}\)

Identify the products \(\mathrm{A}\) and \(\mathrm{B}\) here. (1) \(2 \mathrm{Ag}^{+}\)(excess) \(+\mathrm{S}_{2} \mathrm{O}_{3}^{2-} \longrightarrow \mathrm{Ag}_{2} \mathrm{~S}_{2} \mathrm{O}_{3}\) \(\stackrel{\mathrm{H}_{2} \mathrm{O}}{\longrightarrow} \mathrm{A}+\mathrm{H}_{2} \mathrm{SO}_{4}\) (2) \(2 \mathrm{NO}_{2}^{-}+2 \mathrm{I}^{-} \stackrel{\text { acid medium }}{\longrightarrow} \mathrm{B}+\mathrm{I}_{2}+2 \mathrm{H}_{2} \mathrm{O}\) (a) \(\mathrm{A}=\mathrm{Ag}_{2} \mathrm{O}, \mathrm{B}=\mathrm{N}_{2}\) (b) \(\mathrm{A}=\mathrm{Ag}_{2} \mathrm{~S}, \mathrm{~B}=\mathrm{N}_{2} \mathrm{O}\) (c) \(\mathrm{A}=\mathrm{Ag}_{2} \mathrm{O}, \mathrm{B}=2 \mathrm{NO}_{2}\) (d) \(\mathrm{A}=\mathrm{Ag}_{2} \mathrm{~S}, \mathrm{~B}=2 \mathrm{NO}\)

A white substance, \(X\) described as highly poisonous, dissolves in water. Its aqueous solution produces a scarlet precipitate with KI, soluble in excess KI solution giving a clear and colourless solution, Y. The aqueous solution of \(X\) gives a yellow precipitate with \(\mathrm{NaOH}\). What may be observed on adding \(\mathrm{NH}_{4} \mathrm{Cl}\) and \(\mathrm{NaOH}\) to \(\mathrm{Y} ?\) (a) Brown precipitate (b) Black precipitate (c) Grey precipitate (d) Bright red precipitate

\(20 \mathrm{~mL}\) of \(0.1 \mathrm{M} \mathrm{NaOH}\) and \(30 \mathrm{~mL}\) of \(0.12 \mathrm{M} \mathrm{NaHCO}_{3}\) solutions are mixed. \(25 \mathrm{ml}\) of the resulting solution are titrated against \(0.1 \mathrm{M} \mathrm{HCl}\) using phenolphthalein as the indicator. What would be the titre value? (a) \(100 \mathrm{~mL}\) (b) \(10 \mathrm{~mL}\) (c) \(25 \mathrm{~mL}\) (d) \(20 \mathrm{~mL}\)

A solution, when diluted with \(\mathrm{H}_{2} \mathrm{O}\) and boiled, gives a white precipitate. On addition of excess \(\mathrm{NH}_{4} \mathrm{Cl} /\) \(\mathrm{NH}_{4} \mathrm{OH}\), the volume of precipitate decreases leaving behind a white gelatinous precipitate. Identify the precipitate which dissolves in \(\mathrm{NH}_{4} \mathrm{OH} / \mathrm{NH}_{4} \mathrm{Cl}\) (a) \(\mathrm{Zn}(\mathrm{OH})_{2}\) (b) \(\mathrm{Al}(\mathrm{OH})_{3}\) (c) \(\mathrm{Mg}(\mathrm{OH})_{2}\) (d) \(\mathrm{Ca}(\mathrm{OH})_{2}\)

When a solid substance is a mixture of \(\mathrm{KBr}\) and \(\mathrm{KNO}_{3} .\) Which of the following does not give a distinguishing test? (a) Adding \(\mathrm{AgNO}_{3}\) solution in presence of dilute \(\mathrm{HNO}_{3}\) to a solution of the mixture in water (b) Warming the mixture with concentrated \(\mathrm{H}_{2} \mathrm{SO}_{4}\) (c) Adding dilute \(\mathrm{H}_{2} \mathrm{SO}_{4}\) followed by drops of \(\mathrm{KMnO}_{4}\), to an aqueous solution of the substance, then adding \(\mathrm{CCl}_{4}\) and shaking (d) Adding chlorine water to an aqueous solution of the substance, followed by adding \(\mathrm{CCl}_{4}\) and shaking.

In the separation of \(\mathrm{Cu}^{2+}\) and \(\mathrm{Cd}^{2+}\) in 2 nd group qualitative analysis of cations, tetrammine copper (II) sulphate and tetrammine cadmium(II) sulphate react with \(\mathrm{KCN}\) to form the corresponding cyano complexes. Which one of the following pairs of the complexes and their relative stability enables the separation of \(\mathrm{Cu}^{2+}\) and \(\mathrm{Cd}^{2+} ?\) (a) \(\mathrm{K}_{2}\left[\mathrm{Cu}(\mathrm{CN})_{4}\right]\) less stable and \(\mathrm{K}_{2}\left[\mathrm{Cd}(\mathrm{CN})_{4}\right]\) more stable (b) \(\mathrm{K}_{3}\left[\mathrm{Cu}(\mathrm{CN})_{4}\right]\) more stable and \(\mathrm{K}_{2}\left[\mathrm{Cd}(\mathrm{CN})_{4}\right]\) less stable (c) \(\mathrm{K}_{3}\left[\mathrm{Cu}(\mathrm{CN})_{4}\right]\) less stable and \(\mathrm{K}_{2}\left[\mathrm{Cd}(\mathrm{CN})_{4}\right]\) more stable (d) \(\mathrm{K}_{2}\left[\mathrm{Cu}(\mathrm{CN})_{4}\right]\) more stable and \(\mathrm{K}_{2}\left[\mathrm{Cd}(\mathrm{CN})_{4}\right]\) less stable

A white substance, 'X' evolves on warming with ethanol and conc. \(\mathrm{H}_{2} \mathrm{SO}_{4}\), a vapour which burns with a green-edged flame. \(X\), when mixed with solid \(\mathrm{Na}_{2} \mathrm{CO}_{3}\) and heated on a cavity on charcoal gives a white luminous mass which, when moistened with a drop of \(\mathrm{Co}\left(\mathrm{NO}_{3}\right)_{2}\) solution and heated further yields a green mass. The substance, \(X\) is expected to be (a) \(\mathrm{ZnSO}_{4}\) (b) \(\mathrm{HgCl}_{2}\) (c) \(\mathrm{AlPO}_{4}\) (d) \(\mathrm{Zn}\left(\mathrm{BO}_{2}\right)_{2}\)

Pick out the correct statement(s) here: (1) Golden yellow \(\mathrm{PbI}_{2}\) dissolves in hot water to give a colourless solution. (2) \(\mathrm{Ba}^{2+}\) and \(\mathrm{Ca}^{2+}\) ions can be separated by adding \(\mathrm{CrO}_{4}^{2-}\) ion in acetic acid medium (3) Salts of calcium, copper and nickel give a green flame colour. (4) The sulphide ion gives with alkaline sodium nitroprusside a violet colour. (a) 1 and 3 (b) 2 and 4 (c) 1,2 and 4 (d) 2,3 and 4

A certain pale-green substance, \(X\) becomes dark brown on adding \(\mathrm{NaNO}_{2}\) in presence of dil. \(\mathrm{H}_{2} \mathrm{SO}_{4}\). its aqueous solution gives precipitates with (i) \(\mathrm{BaCl}_{2}\) and (ii) \(\mathrm{NaOH}\) in separate tests. The latter \(\mathrm{NaOH}\) in separate tests. The latter precipitate, Y, gradually changes colour from green to brown, on exposure to air. Identify X here? (a) \(\mathrm{NiSO}_{4}\) (b) \(\mathrm{FeSO}_{4}\) (c) \(\mathrm{ZnSO}_{4}\) (d) \(\mathrm{Cr}_{2}\left(\mathrm{SO}_{4}\right)_{3}\)

Which represents the correct set of reactions and test here? List I 1 . Oc1c(Br)cc(Br)cc1Br CC Oc1ccccc1 Phenol \(\quad 2,4,6\)-tribromophenol 2\. \(3 \mathrm{C}_{6} \mathrm{H}_{3} \mathrm{OH}+\mathrm{FeCl}_{3} \longrightarrow\) CC(C)(C)C \(\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{O}\right)_{3} \mathrm{Fe}^{3}+3 \mathrm{HCl}\) Ferric phenoxide 3\. \(\left(\mathrm{NH}_{4}\right)_{2}\left[\mathrm{Ce}\left(\mathrm{NO}_{3}\right)_{6}\right]+2 \mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH}\) Phenol \(\left[\mathrm{Ce}\left(\mathrm{NO}_{3}\right)_{4}\left(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH}\right)_{2}\right]+2 \mathrm{NH}_{4} \mathrm{NO}_{3}\) Green or brown ppt. 4\. \(\mathrm{R}-\mathrm{CO}-\mathrm{CH}_{3}+3 \mathrm{I}_{2}+4 \mathrm{NaOH}\) \(\mathrm{CHI}_{3}+3 \mathrm{NaI}+3 \mathrm{H}_{2} \mathrm{O}+\mathrm{RCOONa}\) List II (i) Ceric ammonium nitrate test (ii) Bromine water test (iii) Ferric chloride test (iv) Iodoform test The correct matching is \(\begin{array}{llll}1 & 2 & 3 & 4\end{array}\) \(\begin{array}{llll}\text { (a) (ii) } & \text { (i) (iv) (iii) }\end{array}\) (b) (i) (ii) (iv) (iii) (c) (ii) (iii) (i) (iv) (d) (i) (iv) (ii) (iii)

Which of the following salts will form colourless beads in borax bead test? (a) \(\mathrm{CoCl}_{2}\) (b) \(\mathrm{Ba}\left(\mathrm{NO}_{3}\right)_{2}\) (c) \(\mathrm{K}_{2} \mathrm{C}_{2} \mathrm{O}_{4}\) (d) \(\mathrm{CoC}_{2} \mathrm{O}_{4}\)

Which of the following sulphates are soluble in water? (a) \(\mathrm{PbSO}_{4}\) (b) \(\mathrm{CuSO}_{4}\) (c) \(\mathrm{BaSO}_{4}\) (D) \(\mathrm{Ag}_{2} \mathrm{SO}_{4}\)

An aqueous solution containing \(\mathrm{S}^{2-}\) ions will not give (a) White precipitate with \(\mathrm{CaCO}_{3}\) suspension (b) Purple colour with sodium thiosulphate solution (c) A yellow precipitate with the suspension of \(\mathrm{CdCO}_{3}\) in water (d) Black precipitate with lead acetate solution

Which of the following radicals are decomposed by conc. \(\mathrm{H}_{2} \mathrm{SO}_{4}\) only? (a) \(\mathrm{C}_{2} \mathrm{O}_{4}^{2-}\) (b) \(\mathrm{HCO}_{3}^{-}\) (c) \(\mathrm{SO}_{3}^{2-}\) (d) \(\mathrm{CH}_{3} \mathrm{COO}^{-}\)

To the aqueous solution of the salt acidified potassium permanganate is added and its colour is discharged. It indicates the absence of (a) \(\mathrm{Sn}^{2+}\) (b) \(\mathrm{Be}^{2+}\) (c) \(\mathrm{Fe}^{2+}\) (d) \(\mathrm{NO}_{3}^{-}\)

Which among the species will be soluble in excess of \(\mathrm{NaOH} ?\) (a) \(\mathrm{ZnCl}_{2}\) (b) \(\mathrm{Sr}_{2} \mathrm{~S}_{3}\) (c) \(\mathrm{CuS}\) (d) \(\mathrm{AlCl}_{3}\)

Which of the following compounds are water soluble? (a) \(\mathrm{ZnSO}_{4}\) (b) \(\left[\mathrm{Zn}\left(\mathrm{NH}_{3}\right)_{4}\right](\mathrm{OH})_{2}\) (c) \(\mathrm{ZnS}\) (d) \(\mathrm{Na}_{2} \mathrm{ZnO}_{2}\)

Brown vapours can be of (a) \(\mathrm{Br}_{2}\) (b) \(\mathrm{NO}_{2}\) (c) \(\mathrm{HCl}\) (d) \(\mathrm{HBr}\)

Which of the following sulphides are yellow? (a) \(\mathrm{As}_{2} \mathrm{~S}_{3}\) (b) \(\mathrm{ZnS}\) (c) \(\mathrm{CdS}\) (d) \(\mathrm{SnS}_{2}\)

Which ion can show different colours in different compounds? (a) \(\mathrm{Sr}^{2+}\) (b) \(\mathrm{Ni}^{2+}\) (c) \(\mathrm{Pb}^{2+}\) (d) \(\mathrm{Cd}^{2+}\)

If \(\mathrm{Pb}\left[\mathrm{CH}_{3} \mathrm{COO}\right]_{2}\) and \(\mathrm{Na}_{2} \mathrm{~S}\) are mixed and dissolved in water and the solution is filtered then the filtrate will give test of (a) \(\mathrm{CH}_{3} \mathrm{COO}^{-}\) (b) \(\mathrm{Pb}^{2+}\) (c) \(\mathrm{Na}^{+}\) (d) \(\mathrm{S}^{2-}\)

\(\mathrm{FeCl}_{3}\) is acidic towards litmus. On treatment with excess of \(\mathrm{NH}_{4} \mathrm{SCN}\) it gives red coloured compound (A) and on treatment with excess of \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) in the presence of conc. \(\mathrm{H}_{2} \mathrm{SO}_{4}\), it evolves deep red vapours of on passing the vapours of (B) into \(\mathrm{NaOH}\), then adding a solution of acetic acid and lead acetate it gives yellow precipitate of compound of chromium (C). The compound (B) is (a) \(\mathrm{CrO}_{2} \mathrm{Cl}_{2}\) (b) \(\mathrm{Br}_{2}\) (c) \(\mathrm{NO}_{2}\) (d) \(\mathrm{CrOCl}_{4}\)

\(\mathrm{FeCl}_{3}\) is acidic towards litmus. On treatment with excess of \(\mathrm{NH}_{4} \mathrm{SCN}\) it gives red coloured compound (A) and on treatment with excess of \(\mathrm{K}_{2} \mathrm{Cr}_{2} \mathrm{O}_{7}\) in the presence of conc. \(\mathrm{H}_{2} \mathrm{SO}_{4}\), it evolves deep red vapours of on passing the vapours of (B) into \(\mathrm{NaOH}\), then adding a solution of acetic acid and lead acetate it gives yellow precipitate of compound of chromium (C). The compound (A) is (a) \(\mathrm{NH}_{4}\left[\mathrm{Fe}(\mathrm{CN})_{4}\right]\) (b) \(\mathrm{Fe}(\mathrm{SCN})_{2}\) (c) \(\mathrm{FeCl}_{3}\) (d) \(\mathrm{Fe}(\mathrm{SCN})_{3}\)

Borax \(\left[\mathrm{Na}_{2} \mathrm{~B}_{4} \mathrm{O}_{7} .10 \mathrm{H}_{2} \mathrm{O}\right]\) when heated on platinum loop it gives a dark transparent glass like bead. The hot bead is dipped in the salt till it reacts with transition metal oxide. It produces characteristic bead of meta borate. $$ \begin{array}{ll} \text { Colour of the bead } & \text { Ion } \\ \text { Blue green or light blue } & \mathrm{Cu}^{2+} \\ \text { Yellow } & \mathrm{Fe}^{2+} \text { or } \mathrm{Fe}^{3+} \\ \text { Green } & \mathrm{Cr}^{3+} \\ \text { Violet } & \mathrm{Mn}^{2+} \\ \text { Dark blue } & \mathrm{Co}^{2+} \\ \text { Brown } & \mathrm{Ni}^{2+} \end{array} $$ The hybridisation of \(\mathrm{B}\) in borax is (a) sp (b) \(\mathrm{sp}^{2}\) (c) \(\mathrm{sp}^{3}\) (d) Both (B) and (C)

Borax \(\left[\mathrm{Na}_{2} \mathrm{~B}_{4} \mathrm{O}_{7} .10 \mathrm{H}_{2} \mathrm{O}\right]\) when heated on platinum loop it gives a dark transparent glass like bead. The hot bead is dipped in the salt till it reacts with transition metal oxide. It produces characteristic bead of meta borate. $$ \begin{array}{ll} \text { Colour of the bead } & \text { Ion } \\ \text { Blue green or light blue } & \mathrm{Cu}^{2+} \\ \text { Yellow } & \mathrm{Fe}^{2+} \text { or } \mathrm{Fe}^{3+} \\ \text { Green } & \mathrm{Cr}^{3+} \\ \text { Violet } & \mathrm{Mn}^{2+} \\ \text { Dark blue } & \mathrm{Co}^{2+} \\ \text { Brown } & \mathrm{Ni}^{2+} \end{array} $$ Glassy bead is of (a) \(\mathrm{Na}_{3} \mathrm{BO}_{3}\) (b) \(\mathrm{B}_{2} \mathrm{O}_{3}+\mathrm{NaBO}_{2}\) (c) \(\mathrm{SiO}_{2}\) (d) \(\mathrm{Na}_{2} \mathrm{~B}_{4} \mathrm{O}_{7}\)

Borax \(\left[\mathrm{Na}_{2} \mathrm{~B}_{4} \mathrm{O}_{7} .10 \mathrm{H}_{2} \mathrm{O}\right]\) when heated on platinum loop it gives a dark transparent glass like bead. The hot bead is dipped in the salt till it reacts with transition metal oxide. It produces characteristic bead of meta borate. $$ \begin{array}{ll} \text { Colour of the bead } & \text { Ion } \\ \text { Blue green or light blue } & \mathrm{Cu}^{2+} \\ \text { Yellow } & \mathrm{Fe}^{2+} \text { or } \mathrm{Fe}^{3+} \\ \text { Green } & \mathrm{Cr}^{3+} \\ \text { Violet } & \mathrm{Mn}^{2+} \\ \text { Dark blue } & \mathrm{Co}^{2+} \\ \text { Brown } & \mathrm{Ni}^{2+} \end{array} $$ The colour of bead \(\mathrm{Ni}\left(\mathrm{BO}_{2}\right)_{2}\) is of (a) Brown (b) Blue (c) Green (d) Violet

Borax \(\left[\mathrm{Na}_{2} \mathrm{~B}_{4} \mathrm{O}_{7} .10 \mathrm{H}_{2} \mathrm{O}\right]\) when heated on platinum loop it gives a dark transparent glass like bead. The hot bead is dipped in the salt till it reacts with transition metal oxide. It produces characteristic bead of meta borate. $$ \begin{array}{ll} \text { Colour of the bead } & \text { Ion } \\ \text { Blue green or light blue } & \mathrm{Cu}^{2+} \\ \text { Yellow } & \mathrm{Fe}^{2+} \text { or } \mathrm{Fe}^{3+} \\ \text { Green } & \mathrm{Cr}^{3+} \\ \text { Violet } & \mathrm{Mn}^{2+} \\ \text { Dark blue } & \mathrm{Co}^{2+} \\ \text { Brown } & \mathrm{Ni}^{2+} \end{array} $$ The flame used in borax bead test is (a) Oxidising (b) Reducing (c) Both (A) and (B) (d) Neither (A) nor (B)

Match the following $$ \begin{array}{ll} \hline \text { List-I } & \text { List-II } \\ \hline \text { a. } \mathrm{AgNO}_{3}+\mathrm{NaCNS} & \text { (p) White } \\ \text { b. } \mathrm{AgNO}_{3}+\mathrm{Na}_{3} \mathrm{PO}_{4} & \text { (q) Black } \\ \text { c. } \mathrm{AgNO}_{3}+\mathrm{K}_{2} \mathrm{CrO}_{4} & \text { (r) Brick red } \\ \text { d. } \mathrm{AgNO}_{3}+\mathrm{Na}_{2} \mathrm{~S} & \text { (s) Yellow } \\ \hline \end{array} $$

Match the following $$ \begin{array}{ll} \text { List-I } & \text { List-II } \\ \hline \text { a. } \operatorname{Borax} \stackrel{\Delta}{\longrightarrow} & \text { (p) } \mathrm{BN} \\ \text { b. } \text { Borax }+\mathrm{NH}_{4} \mathrm{Cl} \stackrel{\Delta}{\longrightarrow} & \text { (q) } \mathrm{H}_{2} \mathrm{~B}_{4} \mathrm{O}_{7} \end{array} $$ c. Borax \(\stackrel{\Delta}{\longrightarrow}\) (r) \(\mathrm{H}_{3} \mathrm{BO}_{3}\) d. Borax \(+\mathrm{H}_{2} \mathrm{O} \longrightarrow\) (s) \(\mathrm{NaBO}_{2}+\mathrm{B}_{2} \mathrm{O}_{3}\)

Match the following $$ \begin{array}{ll} \hline \text { List-I } & \text { List-II } \\ \hline \text { a. Chromyl chloride test } & \text { (p) } \mathrm{CH}_{3} \mathrm{COO}^{-} \\ \text {b. Ring test } & \text { (q) } \mathrm{S}^{2-} \\ \text { c. Smell of vinegar } & \text { (r) } \mathrm{Cl}^{-} \\ \text {d. Smell of rotten eggs } & \text { (s) } \mathrm{NO}_{3}^{-} \end{array} $$

\(0.2063 \mathrm{~g}\) of an organic compound (molar mass 168 ) was heated with sufficient amount of HI and the resulting solution was treated with alcoholic \(\mathrm{AgNO}_{3}\) solution. This led to precipitation of \(0.8658 \mathrm{~g}\) of \(\mathrm{AgI}\). The number of methoxy groups in one molecule of the organic compound is /are (Given : Atomic mass of \(\mathrm{Ag}=108, \mathrm{I}=127)\) (a) 2 (b) 3 (c) 1 (d) 4

When \(\mathrm{H}_{2} \mathrm{~S}\) is passed through \(\mathrm{Hg}_{2}{\underline{\phantom{xx}}}^{2+}\), we get (a) \(\mathrm{Hg}_{2} \mathrm{~S}\) (b) \(\mathrm{HgS}\) (c) \(\mathrm{HgS}+\mathrm{Hg}_{2} \mathrm{~S}\) (d) \(\mathrm{HgS}+\mathrm{Hg}\)

How do we differentiate between \(\mathrm{Fe}^{3+}\) and \(\mathrm{Cr}^{3+}\) in group III? (a) by increasing \(\mathrm{NH}_{4}{\underline{\phantom{xx}}}^{+}\)ion concentration (b) by decreasing \(\mathrm{OH}^{-}\)ion concentration (c) by adding excess of \(\mathrm{NH}_{4} \mathrm{OH}\) solution (d) both (a) and (b)

Which one of the following statement is correct? (a) Ferric ions give a deep green precipitate on adding potassium ferrocyanide solution (b) From a mixed precipitate of \(\mathrm{AgCl}\) and \(\mathrm{AgI}\), ammonia solution dissolves only \(\mathrm{AgCl}\) (c) Manganese salts give a violet borax bead test in the reducing flame (d) On boiling a solution having \(\mathrm{K}^{+}, \mathrm{Ca}^{2+}\) and \(\mathrm{HCO}_{3}^{-}\) ions we get a precipitate of \(\mathrm{K}_{2} \mathrm{Ca}\left(\mathrm{CO}_{3}\right)_{2}\)

Calomel \(\left(\mathrm{Hg}_{2} \mathrm{Cl}_{2}\right)\) on reaction with ammonium hydroxide gives (a) \(\mathrm{HgO}\) (b) \(\mathrm{Hg}_{2} \mathrm{O}\) (c) \(\mathrm{HgNH}_{2} \mathrm{Cl}\) (d) \(\mathrm{NH}_{2}-\mathrm{Hg}-\mathrm{Hg}-\mathrm{Cl}\)

In the chemical reactions, \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{NH}_{2}+\mathrm{CHCl}_{3}+3 \mathrm{KOH} \longrightarrow\) (a) \(+(\mathrm{b})+3 \mathrm{H}_{2} \mathrm{O}\) the compounds (a) and (b) are respectively: (a) \(\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{CONH}_{2}\) and \(3 \mathrm{KCl}\) (b) \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NC}\) and \(\mathrm{K}_{2} \mathrm{CO}_{3}\) (c) \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NC}\) and \(3 \mathrm{KCl}\) (d) \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{CN}\) and \(3 \mathrm{KCl}\)

Amount of oxalic acid present in a solution can be determined by its titration with \(\mathrm{KMnO}_{4}\) solution in the presence of \(\mathrm{H}_{2} \mathrm{SO}_{4} .\) The titration gives unsatisfactory result when carried out in the presence of \(\mathrm{HCl}\), because of (a) Gets oxidized by oxalic acid to chlorine (b) Furnishes \(\mathrm{H}^{+}\)ions in addition to those from oxalic acid (c) Reduces permanganate to \(\mathrm{Mn}^{2+}\) (d) Oxidises oxalic acid to carbon dioxide and water

Silver Mirror test is given by which one of the following compounds? (a) Acetone (b) Formaldehyde (c) Benzophenone (d) Acetaldehyde

Which of the following compounds is not colored yellow? (a) \(\mathrm{Zn}_{2}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\) (b) \(\mathrm{K}_{3}\left[\mathrm{Co}\left(\mathrm{NO}_{2}\right)_{6}\right]\) (c) \(\left(\mathrm{NH}_{4}\right)_{3}\left[\mathrm{AS}\left(\mathrm{Mo}_{3} \mathrm{O}_{10}\right)_{4}\right]\) (d) \(\mathrm{BaCrO}_{4}\)