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Solved Examples on Principles Related to Practical Chemistry.

Question 1: The gas liberated on heating a mixture of two salts with NaOH gives a reddish brown precipitate with an alkaline solution of K2HgI4. The aqueous solution of the mixture on treatment with BaCl2 gives a white precipitate which is sparingly soluble in conc. HCl. On heating the mixture with K2Cr2O7 and conc. H2SO4 red vapours  of A are produced. The aqueous solution of the mixture gives a deep blue colouration B with potassium ferricyanide solution. Identify the radicals in the given mixture and write the balanced equations for the formation of A and B.

Solution: Let us summarise the given facts of the question.




The given reactions lead to following conclusions.

i) Heating of mixture with NaOH to give NH3 gas (indicated by reddish brown ppt. with alkaline solution of K2HgI4) indicates the presence of   ion in the mixture

ii) Heating of mixture with K2Cr2O7 and conc. H2SO4 to give red vapours (of chromyl chloride) indicates the presence of Cl ion in the mixture.

iii)  Reaction of aqueous solution of the mixture with barium chloride solution to give white ppt. (of BaSO4) sparingly soluble in conc. HCl indicates the presence of  ions in the mixture.

iv)  Reaction of aqueous solution of the mixture with potassium ferricyanide solution to give deep blue colour indicates the presence of Fe2+ ions in the mixture.

 Hence the mixture contains the following four ions. NH4+, Fe2,  SO42-and Cl.
Equations for the formation of A and B


Question2. : When an orange coloured crystalline compound (A) was heated with common salt and concentrated sulphuric acid an orange - yellow coloured gas (B) was evolved. The gas (B) when passed through caustic soda solution gave a yellow solution (C) which in turn gave the following reactions.

  1. Addition of silver nitrate solution to (C) gave first a white precipitate which then turns red. Quantitatively, 0.155 g of the gas (B) required 2.0 m moles of AgNO3 to produce the first trace of red colour.
  2. Acidification of the solution (C) with dil. H2SO4 gave an orange solution which contained chromium in +6 oxidation state. The solution liberated iodine from aqueous potassium iodide, leaving a green solution containing chromium in +3 oxidation state. Quantitatively 0.155 g of the gas (B) liberated 1.5 mmole of iodine.

Deduce the formula of A, B and C and explain the reactions.

Solution: Let us summaries the given reactions.



The above set of reactions indicates that compound A is K2Cr2O7, B is chromyl chloride gas and C is sodium chromate which explains all the given reactions as below.


The quantitative data is explained in the following manner. From the above reactions we observe that


155 g of CrO2Cl2  require 2 mole of AgNO3

This also coincides with the given data.

Question: 3, A white amorphous powder (A) when heated, gives a colourless gas (B), which turns lime water milky (which dissolves on passing excess of gas (B) and the  residue (C) which is yellow while hot but white when cold. The residue (C) dissolves in dilute HCl and the resulting solution gives a white precipitate on addition of potassium ferrocyanide solution. (A) dissolves in dil. HCl with the evolution of a gas which is identical in all respects to gas (B).  The solution of (A) in dil. HCl gives a white ppt. (D) on addition of  NH4Cl  excess of NH4OH and on passing H2S gas. Another portion of this solution gives initially a white ppt. (E) on addition of NaOH  solution which dissolves in excess of NaOH. The solution on passing again H2S gives back the white ppt. of (E), the white ppt. on heating with dil H2SO4 give a gas used in II and IV group analysis. What are (A) to (E)? Give balanced chemical equations of the reactions.

Solution:



From observations for section (a), one may conclude that the colourless gas is CO2 because it turns lime water milky, due to formation of insoluble CaCO3.


CaCO3  is...

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