FRANK Solutions for Class 10 Chemistry Chapter 4 - Analytical Chemistry
Revise Chemistry concepts with our Frank Solutions for ICSE Class 10 Chemistry Chapter 4 Analytical Chemistry. Learn to identify the given cations with clear answers by TopperLearning’s Chemistry experts. Relearn the concept of amphoteric oxides. Find out how to write balanced equations to explain the reaction of amphoteric oxides with a caustic alkali.
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Chapter 4 - Analytical Chemistry Exercise 85
(a) Cuprous salts.
(b) Cupric salts.
(c) Aluminium salts.
(d) Ferrous salts.
(e) Ferric salts.
(f) Calcium salts.
(b) Cupric salts = Blue
(c) Aluminium salts = Colourless
(d) Ferrous salts= Light green
(e) Ferric salts = Yellow
(f) Calcium salts = Colourless
(a) Ferrous ion and Ferric ion.
(b) Zinc ion and Lead ion.
(a) FeCl3
(b) ZnSO4
(c) Pb(NO3)2
(d) CuSO4
(a) Zn(OH)2 from Pb(OH)2
(b) CaO from PbO
(c) CuO from ZnO
(a) Name the powdered metal added to sodium hydroxide solution.
(b) Name the gas evolved.
(c) Name the salt present in the colorless solution.
(a) A metallic hydroxide soluble in excess of NH4OH
(a) A metallic oxide soluble in excess of caustic soda solution.
(b) A strong alkali
(c) A weak alkali.
(d) Two coloured ions
(e) Two bases which are not alkalis but dissolve in strong alkalis.
(f) A coloured metallic oxide which dissolves in alkalis to yield colourless solutions.
Chapter 4 - Analytical Chemistry Exercise 86
(a) Dropwise and then
(b) In excess to the following solutions:
(i) CuSO4
(ii) ZnSO4
(iii) FeCl3
(c) Write balanced reactions.
(a) Which metal salt solution was used?
(b) What is the formula of white gelatinous precipitate obtained?
(a) A yellow monoxide that dissolves in hot and concentrated caustic alkali.
(b) A white, insoluble oxide that dissolves when fused with caustic soda or potash.
(c) A compound containing zinc in the anion.
(b) Al2O3
(c) Na2ZnO2
Fill in the blanks:
(a) Salts of ______ [normal / transition] elements are generally coloured. From the ions K1+, Cr3+, Fe2+, Ca2+, the ions generally coloured are ______.
(b) The hydroxide which is soluble in excess of NaOH is ______ [Zn(OH)2 / Fe(OH)3 / Fe(OH)2].
(c) The salt which will not react with NH4OH solution ______[ZnCl2, CuCl2 / NH4Cl/ FeCl2]
(d) The substance/s which react with hot conc. NaOH solution and undergoes a neutralization reaction ______ [Al2O3 / Al / Al(OH)3]
(e) To distinguish soluble salts of zinc and lead ______ [NaOH / NH4OH]can be used.
(a) transition, Cr3+, Fe2+, MnO44-.
(b) Zn(OH)2
(c) NH4Cl
(d) Al2O3, Al
(e) NH4OH
Choose the correct answer from the options given below :
(i) Color of ferrous ion is
(a) Blue
(b) Green
(c) Pink
(d) Light green
(ii) Which one is colourless anion?
(iii) Sodium zincate (Na2ZnO2) is
(a) Pale blue ppt
(b) Reddish brown ppt
(c) Colourless
(d) Dirty green ppt
(iv) Metal + alkali → salt + _________
(a) N2
(b) H2
(c) H2O
(d) OH
(v) Which salt solution is soluble in excess of NH4OH
(a) Iron (II) salts
(b) Iron (III) salts
(c) Lead salts
(d) Copper (II) salts
(i) Green
(ii)
(iii) Colourless
(iv) H2
(v) Copper(II) salts
Chapter 4 - Analytical Chemistry Exercise 87
You are given a mixture of precipitated copper hydroxide and zinc hydroxide. Name a solvent which will dissolve:
(a) Only copper hydroxide
(b) Only zinc hydroxide
(c) Both copper hydroxide and zinc hydroxide
(a) Addition of KCN
(b) Addition of excess of NaOH.
(c) Addition of excess of NH4OH.
(a) Zinc nitrate solution from calcium nitrate solution
(b) Iron (II) chloride from iron (III) chloride
(c) Lead hydroxide from magnesium hydroxide.
(b) When ammonium hydroxide is added to solution B, a pale blue precipitate is formed. This pale blue precipitate dissolves in excess ammonium hydroxide to give an inky blue solution. Name the cation present in solution B. What is the probable colour of solution B?
(b) The cation present in solution B is Cu2+. The probable colour of solution B is blue.
(i) Solution of Calcium carbonate:
Calcium carbonate is CaCO3 and contains Ca2+ ions. Sodium hydroxide solution NaOH can be used to identify Ca2+ since its addition to calcium carbonate solution will give white precipitates of Ca(OH)2 which are sparingly soluble in excess of NaOH.
(ii) Solution of Lead carbonate:
Lead carbonate is PbCO3 and contains Pb2+ ions. Ammonium hydroxide solution NH4OH can be used to identify Pb2+ since its addition to lead carbonate solution will give white precipitates of Pb(OH)2 which are insoluble in excess of NH4OH.
(iii) Solution of Zinc carbonate:
Zinc carbonate is ZnCO3 and contains Zn2+ ions. Sodium hydroxide solution NaOH can be used to identify Zn2+ since its addition to zinc carbonate solution will give white gelatinous precipitates of Zn(OH)2 which are soluble in excess of NaOH.
(i) Adding sodium hydroxide solution to each portion in turn till it is in excess.
(ii) Adding ammonium hydroxide to each portion in turn till it is in excess.
(b) What will you observe when barium chloride solution is added to iron(II) sulphate solution.
(c) How will the action of dilute hydrochloric acid on sodium carbonate and sodium sulphite enables you to distinguish between these two compounds?
Chapter 4 - Analytical Chemistry Exercise 88
(i) Sodium chloride solution and sodium nitrate solution.
(ii) Sodium sulphate solution and sodium chloride solution.
(iii) Calcium nitrate solution and zinc nitrate solution.
Write balanced equations for the following reactions:
(i) Iron(II) chloride solution with sodium hydroxide solution.
(ii) Chlorine and cold dilute sodium hydroxide solution.
(iii) Zinc and sodium hydroxide solution
(iv) Sulphur dioxide and sodium hydroxide solution
(Give the equation for the formation of the normal salt)
(i) Neutral litmus solution is added to alkaline solution
(ii) Ammonium hydroxide is added to iron (III) sulphate solution.
(iii) Lead nitrate and sodium chloride are mixed.
(iv) Ethane is bubbled through a solution of bromine in tetrachloromethane (carbon tetra chloride).
(v) Sulphur burns.
(i) Sodium hydroxide is added dropwise to a solution of zinc sulphate, till it is in excess.
(ii) Ammonium hydroxide is added first in a small quantity, and then in excess, to a solution of copper sulphate.
(iii) Excess of ammonium hydroxide is added to a substance, obtained by adding hydrochloric acid to silver nitrate solution.
(iv) Moist starch iodide paper is placed at the mouth of a test tube containing chlorine gas.
(v) A paper dipped in potassium permanganate solution is placed at the mouth of a test tube, containing sulphur dioxide gas.
Chapter 4 - Analytical Chemistry Exercise 89
A. Copper nitrate
B. Iron (II) sulphate
C. Iron (III) chloride
D. Lead nitrate
E. Magnesium sulphate
F. Zinc chloride
(i) Which two solutions will give a white precipitate when treated with dilute hydrochloric acid followed by barium chloride solution/
(ii) Which two solutions will give a white precipitate when treated with dilute nitric acid followed by silver nitrate solution?
(iii) Which solution will give a white precipitate when either dilute hydrochloric acid or dilute sulphuric acid is added to it?
(iv) Which solution becomes a deep/inky blue colour when excess of ammonium hydroxide is added to it?
(v) Which solution gives a white precipitate with excess ammonium hydroxide?
(ii) C and F (Iron (III) chloride and Zinc chloride)
(iii) D (Lead nitrate)
(iv) A (Copper nitrate)
(v) F (Zinc chloride)
Chapter 4 - Analytical Chemistry Exercise 90
The metal oxide which can react with acid as well as alkali is:
(a) Silver oxide.
(b) Copper (II) oxide.
(c) Aluminium oxide
(d) Calcium oxide
Identify the substances P, Q and R in each case based on the information given below:
(i) The deliquescent salt P, turns yellow on dissolving in water, and gives a reddish brown precipitate with sodium hydroxide solution.
(ii) The white crystalline solid Q is soluble in water. It liberates a pungent smelling gas when heated with sodium hydroxide solution.
(iii) The pale green solid R turns reddish brown on heating. Its aqueous solution gives a white precipitate with barium chloride solution. The precipitate is insoluble in mineral acids.
(i) P is Ferric chloride
(ii) Q is an ammonium salt
(iii) R is ferrous sulphate
(i) Zinc sulphate solution and Zinc chloride solution.
(ii) Iron (II) chloride solution and iron (III) chloride solution.
(ii) When NaOH solution is added to the given solution, iron (II) chloride gives dirty green precipitate while reddish brown precipitate is obtained with iron(III) chloride.
From the list given below, select the word (s) required complete the blanks (i) to (v) in the following passage :
Note : words chosen from the list are to be used only once. Write only the answers. Do not copy the passage, [ reddish brown, ammonium, nitrogen dioxide, hydroxyl, dirty green, ammonia, acidic, alkaline]
Nitrogen and hydrogen combine in the presence of a catalyst to give (i) ________ gas. When the above mentioned gas is passed through water it forms a solution which will be (ii) ______ in nature and the solution contains (iii) ______ ions and (iv) _______ions. The above solution when added to iron (II) sulphate solution gives a (v) _________coloured precipitate of iron (II) hydroxide
(i) Ammonia
(ii) Alkaline
(iii) Ammonium
(iv) Hydroxyl
(v) Dirty green
Write the equation for the following reaction :
Zinc oxide is treated with sodium hydroxide solution.
Choose the correct answer from the options given below :
(i) Hydroxide of this metal is soluble is sodium hydroxide solution
(a) Magnesium
(b) Lead
(c) Silver
(d) Copper
(ii) When dilute sulphuric acid reacts with iron sulphide, the gas evolved is _______
(a) Hydrogen sulphide
(b) Sulphur dioxide
(c) Sulphur trioxide
(d) Vapour of sulphuric acid
(i) Lead
(ii) Hydrogen sulphide
Chapter 4 - Analytical Chemistry Exercise 91
State two relevant observations for each of the following:
(i) Ammonium hydroxide solution is added to copper (II) nitrate solution in small quantities and then in excess
(ii) Ammonium hydroxide solution is added to zinc nitrate solution in minimum quantities and then in excess
(i) (a) When NH4OH is added to copper (II) nitrate solution in small quantities, a pale blue precipitate is observed.
(b) When added in excess, NH4OH dissolves to give an inky blue solution forming a complex salt.
(ii) (a) When NH4OH is added to zinc nitrate solution in minimum quantity, it forms a gelatinous white precipitate.
(b) When added in excess, it dissolves to form a complex salt.
Distinguish between the following pairs of compound using the test given within brackets.
(i) Iron (II) Sulpate an and iron(III) using ammonium hydroxide)
(ii) A lead salt and a zinc salt (using excess ammonium hydroxide
(i) Iron (II):
Iron (III):
(ii) Pb(NO3)2+2 NH4OH → Pb(OH)2+2NH4NO3
On adding excess of NH4OH, chalky white ppt. of
insoluble Pb(OH)2 is formed.
ZnSO4 + 2NH4OH → Zn(OH)2 + (NH4)2SO4
With excess of NH4OH, white gelatinous ppt. of soluble Zn(OH)2 is formed.
State your observations when ammonium hydroxide solution is added drop by drop and then in excess to each of the following solutions :
(i) Copper sulphate solution
(ii) Zinc sulphate solution
i) When NH4OH is added to copper sulphate solution drop-wise, a pale blue ppt. is obtained.
CuSO4 + 2NH4OH → Cu(OH)2 + (NH4)2SO4 + 4H2O
With excess of NH4OH, the ppt. dissolves to give a deep blue solution of tetra amine copper (II) sulphate.
Cu(OH)2 + (NH4)2SO4 + NH4OH → [Cu(NH3)4]SO4 + H2O
ii) When NH4OH is added to zinc sulphate solution drop-wise, a white, gelatinous ppt. is obtained.
ZnSO4 + 2NH4OH → Zn(OH)2 + (NH4)2SO4
With an excess of NH4OH, the ppt. dissolves to give a colourless solution of tetra amine zinc (II) sulphate.
Zn(OH)2 + (NH4)2SO4 + 2NH4OH → [Zn(NH3)4]SO4 + 4H2O
Fill in the blank from the choices given in bracket.
Potassium sulphite on reacting with hydrochloric acid releases ________
Potassium sulphite on reacting with hydrochloric acid releases sulphur dioxide.
Choose the correct answer from the options given below :
A chloride which forms a precipitate that is soluble in excess of ammonium hydroxide is :
(a) Calcium chloride
(b) Ferrous chloride
(c) Ferric chloride
(d) Copper chloride
Copper chloride
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