New Simplified Chemistry Class 10 ICSE Solutions – Practical Chemistry
Viraf J Dalal Chemistry Class 10 Solutions and Answers
These Solutions are part of New Simplified Middle School Chemistry Class 10 ICSE Solutions Here we have given New Simplified Chemistry Class 10 ICSE Solutions – Practical Chemistry
State the colour of the residue obtained on cooling when the following carbonates are heated :
- zinc carbonate
- lead carbonate
- copper carbonate.
- In case of zinc carbonate, residue is yellow when hot and White when cold
- In case of lead carbonate, residue is reddish-brown when hot and yellow when cold
- In case of Copper carbonate, residue is black when cold.
Sodium hydroxide solution is added first in a small quantity, then in excess to the aqueous salt solutions of copper (II) sulphate, zinc nitrate, lead nitrate, calciumchloride and iron (III) sulphate. For each of the aqueous salt solutions, state —
(a) the colour of the precipitate when NaOH is added in a small quantity ;
(b) the nature of precipitate (i.e. soluble or insoluble) when NaOH is added in excess.
The questions below refer to the following salt solutions listed A to F : A : Copper nitrate B : Iron (II) sulphate C : Iron (HI) chloride D : Lead nitrate E : Magnesium sulphate F : Zinc chloride.
- Which two solutions will give a white precipitate when treated with dilute hydrochloric acid followed by barium chloride solution, (i.e. white ppt. insoluble in dil. HCl)
- Which two solutions will give a white ppt. when treated with dil. HNO3 and AgNO3 soln.
- Which soln. will give a white ppt. when either dil. HCl or dil. H2SO4 is added to it.
- Which soin. becomes a deep/inky blue colour when excess of ammonium hydroxide is added to it.
- Which solution gives a white precipitate with excess ammonium hydroxide solution.
- B and E [Iron(II) Sulphate and Magnesium sulphate]
- C and F [Iron(II) chloride and Zinc chloride]
- D [Lead nitrate]
- A [Copper nitrate]
- D [Lead nitrate]
From the list of substances given—Ammonium sulphate, Lead carbonate, Chlorine, Copper nitrate, Ferrous sulphate — State : A substance that turns moist starch iodide paper blue.
State what is observed when excess of ammonia passed through an aqueous solution of lead nitrate.
When ammonia is passed through an aq. solution of lead nitrate, chalky white precipitate of lead hydroxide is formed which is insoluble in excess of ammonia.
Give one test each to distinguish between the following pairs of chemicals solutions
- Zn(NO3)2 and Ca(NO3)2
- NaNO3 and NaCI
- Iron [III] chloride and copper chloride.
- Add NaOH solution in excess to the two solutions. The one in which white ppt. initially formed dissolves in excess of NaOH solution is Zn(NO3)2 solution and the other is Ca(NO3)2 solution.
- Add freshly prepared ferrous sulphate solution to the two solutions. Then by the side of the test tube, pour cone, sulphuric acid (H2SO4) to each slowly. The one in which brown ring appears is sodium nitrate solution while the other is sodium chloride sol.
- Add NaOH solution to both the solutions. The one which give a reddish brown ppt. is Iron(II) chloride solution and the one which gives blue ppt. is copper chloride solution.
Give a reason why carbon dioxide and sulphur dioxide cannot be distinguished by using lime water.
Because both turns lime water milky.
Salts A, B, C, D and E undergo reaction (i) to (v) respectively. Identify the anion present in these salts on the basis of these reactions.
- When AgNO3 solution is added to a soln. of A, a white precipitate, insoluble in dilute nitric acid, is formed.
- Addition of dil. HCl to B produces a gas which turns lead acetate paper black.
- When a freshly prepared solution of FeSO4 is added to a soln. of C and cone. H2SO4 is gently poured from the side of the test-tube, a brown ring is formed.
- When dil. H2SO4 is added to D a gas is produced which turns acidified K2Cr2O7 soln. from orange to green.
- Addition of dil. HCI to E produced an effervescence. The gas produced turns limewater milky but does not effect acidified K2Cr2O7 soln.
- Chloride Cl1-
- Sulphide S2-
- Nitrate NO32-
- Sulphite SO32-
- Carbonate CO32-
How will the addition of barium chloride soln. help to distinguish between dil. HCl and dil. H2SO4.
Barium chloride does not react with dil HCl but with dil H2SO4 gives a white ppt. of barium sulphate.
The salt which, in solution gives a pale green ppt. with sodium hydroxide solution and a white precipitate with barium chloride solution is :
A : Iron (III) sulphate
B : Iron (II) sulphate
C : Iron (II) chloride
D : Iron (III) chloride
B : Iron (II) sulphate
Carbon dioxide and sulphur dioxide gas can be distinguished by using :
(A) Moist blue litmus paper
(B) Lime water
(C) Acidified potassium dichromate paper
(D) None of the above.
(C) Acidified potassium dichromate paper
Identity the substances ‘R’ based on the information given below :
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.
Ferrous sulphate (Fe2SO4).
Give one chemical test to distinguish between the following pairs of compounds.
- ZnSO4 and ZnCl2
- FeCl2 and FeCl3
- Calcium nitrate soln. and Calcium chloride soln.
Select the correct answer from A, B, C, D and E –
(A) Nitroso Iron (II) sulphate
(B) Iron (III) chloride
(C) Chromium sulphate
(D) Lead (II) chloride
(E) Sodium chloride.
The compound which is responsible for the green colour formed when SO2 is bubbled through acidified potassium dichromate solution.
(C) Chromium sulphate
State your observation –
- A piece of moist blue litmus paper
- Paper soaked in potassium permanganate solution- is introduced into a gas jar of sulphur dioxide.
- Moist blue litmus turns red and finally colourless as SO2 act as an acidic gas and then a bleaching agent.
- The pink colour of potassium permanganate paper turns colourless because of bleaching property of sulphur dioxide.
Write the equation for the reaction of magnesium sulphate solution with barium chloride solution.
MgSO4 + BaCl2 → BaSO4 + MgCl2
Choose from the list of substances – Acetylence gas, aqua fortis, coke, brass, barium chloride, bronze, platinum.
An aqueous salt solution used for testing sulphate radical.
Name the gas which turns acidified potassium dichromate clear green.
Sulphur dioxide gas (SOs)
Identify the anion present in the following compounds :
- Compound X on heating with copper turnings and concentrated sulphuric acid liberates a reddish brown gas.
- When a solution of compound Y is treated with silver nitrate solution a white precipitate is obtained which is soluble in excess of ammonium hydroxide solution.
- Compound Z which on reacting with dilute sulphuric acid liberates a gas which turns lime waer milky, but the gas has no effect on acidified potassium dichromate solution.
- Compound L on reacting with Barium chloride solution gives a white precipitate insoluble in dilute hydrochloric acid or dilute nitric acid.
- Nitrate ion, NO3–
- Chloride ion, Cl–
- Carbonate ion, CO32-
- Sulphate ion, SO42-
State one chemical test between each of the following pairs :
- Sodium carbonate and Sodium sulphite
- Ferrous nitrate and Lead nitrate
- Manganese dioxide and Copper(II) oxide
- Treat each of the compound with dilute sulphuric acid. In case of sodium carbonate a colourless and odourless gas is evolved. In case of sodium sulphite a colourless gas evolved which has a choking smell and causes coughing.
- To each of the aqueous solutions of compounds add aqueous sodium hydroxide solution. A dirty green precipitate is formed in case of ferrous nitrate, whereas a white chalky precipitate is formed in case of lead nitrate.
- Heat each of the compound with cone, hydrochloric acid. In case of manganese dioxide a greenish yellow gas (chlorine) is evolved. In case of copper(II) oxide, no gas evolved and a bluish green solution is formed.
State one observation : A zinc granule is added to copper sulphate solution.
The blue colour of copper sulphate solution fades to form a colourless solution.
Give balanced equation for the reaction :
Silver nitrate solution and Sodium chloride solution.
Give a chemical test to distinguish between :
- NaCl soln. and NaNO3 soln.
- HCl gas and H2S gas.
- Calcium nitrate soln. and zinc nitrate soln.
- Carbon dioxide gas and sulphur dioxide gas.
- Add silver nitrate solution to sodium chloride solution and sodium nitrate solution. In case of sodium chloride, a curdy white ppt. is formed. In case of sodium nitrate solution the reaction mixture remains colourless.
- Moist lead acetate paper turns black in case of hydrogen sulphide gas, but does not change its colour in case of hydrogen chloride gas.
- To each of the solution add first sodium hydroxide solution in small amount and then in excess. In case of calcium y nitrate a fine white precipitate is formed, which does not dissolve in excess of sodium hydroxide. In case of zinc nitrate a gelatin like white precipitate is formed which dissolves in excess of sodium hydroxide.
- To each of the gas add few drops of acidified potassium dichromate solution. In case of carbon dioxide no change takes place. In case of sulphur dioxide, potassium dichromate solution turns blue.
From A : CO ; B : CO2 ; C : NO2 ; D : SO3 – State which will not produce an acid on reaction with water.
A : CO
Distinguish between : Sodium nitrate and sodium sulphite (using dilute sulphuric acid)
Sodium nitrate will not react with dilute sulphuric acid.
Sodium sulphite reacts with dil. sulphuric acid to liberate foul smelling hydrogen sulphide gas.
State your observation : When moist starch iodide paper is introduced into chlorine gas.
The starch iodide paper turns blue due to the liberation of free iodine.
The flame test with a salt P gave a brick red flame. What is the cation in P?
Cation in P is Ca2+ (calcium ion).
Gas Q turns moist lead acetate paper silvery black. Identify the gas Q.
pH of liquid R is 10. What kind of substance is R?
The gas Q is H2S (Hydrogen sulphide).
The substance R is a alkaline.
Select the gas that has a charateristic rotten egg smell. [ammonia, ethane, hydrogen chloride, hydrogen sulphide, ethyne]
State one relevant observation : When hydrogen sulphide gas is passed through lead acetate solution.
When hydrogen sulphide gas is passed through lead acetate solution, it forms a black precipitate of lead sulphide.
Identify the anion present in each of the following compounds: A, B, C :
- Salt ‘A’ reacts with cone. H2SO4 producing gas which fumes in moist air and gives dense fumes with ammonia.
- Salt ‘B’ reacts with dil. H2SO4 producing a gas which turns lime water milky but has no effect on acidified potassium dichromate solution.
- When barium chloride solution is added to salt solution. ‘C’ a white precipitate insoluble in dilute hydrochloric acid is obtained.
- Chloride ion (Cl–)
- Carbonate ion (CO32) or bicarbonate ion (HCO3-1)
- Sulphate ion (SO42-)
Identify the cation present in each of the following compounds — W, X, Y, Z :
- To solution ‘W’, ammonium hydroxide is added in minimum quantity first and then in excess. A dirty white precipitate is formed which dissolves in excess to form a clear solution.
- To solution ‘X’ ammonium hydroxide is added in minimum quantity first and then in excess. A pale blue precipitate is formed which dissolves in excess to form a clear inky blue solution.
- To solution ‘Y’ a small amount of sodium hydroxide is added slowly and then in excess. A white insoluble precipitate is formed.
- To a salt ‘Z’ calcium hydroxide solution is added and then the mixture is heated. A pungent smelling gas turning moist red litmus paper blue is obtained.
- Zn2+ (Zinc Ion)
- Cu2+ (Copper (II) Ion)
- Ca2+ (Calcium Ion)
- NH4+ (Ammonium Ion)
Identify the cations in each of the following cases :
- NaOH solution when added to the solution ‘A’ gives a reddish brown precipitate.
- NH4OH solution when added to the solution ‘B’ gives white ppt which does not dissolve in excess.
- NaOH solution when added to the solution ‘C’ gives white ppt which is insoluble in excess.
- Ferric (Fe3+) ion
- Plumbous (Pb2+) ion
- Calcium (Ca2+) ion
Choose the correct answer from the options – 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.
D. Copper chloride.
Identify the substance underlined – Cation that does not form a precipitate with ammonium hydroxide but forms one with sodium hydroxide.
Identify the salts P and Q from the observations given below :
- On performing the flame test salt P produces a lilac coloured flame and its solution gives a white precipitate with silver nitrate solution, which is soluble in ammonium hydroxide solution.
- When dilute HCl is added to a salt Q, a brisk effervescence is produced and the gas turns lime water milky. When NH4OH solution is added to the above mixture [after adding dilute HCl], it produces a white precipitate which is soluble in excess NH4OH solution.
(i) The salt P is potassium chloride.
- Reason : K+ ions give lilac colour to flame and Cl– ions react with silver nitrate to form silver chloride precipitate which is soluble in excess of ammonium hydroxide.
(ii) The salt Q is zinc carbonate.
- Reason : CO3-2 ions are responsible for the liberation of carbon dioxide with HCl. The salt formed is zinc chloride which forms white precipitate with ammonium hydroxide. This precipitate is soluble in excess of ammonium hydroxide.
The following materials are provided – solutions of cobalt chloride, ammonia, potassium permanganate, lime water, starch-iodide, sodium hydroxide, lead acetate, potassium iodide. Also provided are litmus and filter papers, glowing splinters and glass rods. Using the above how would you distinguish between :
(a) a neutral, acidic and a basic gas
(b) oxygen and hydrogen gas
(c) carbon dioxide and sulphur dioxide gas
(d) chlorine and hydrogen chloride gas
(e) hydrogen sulphide and nitrogen dioxide gas
(f) ammonia and carbon dioxide gas
(g) zinc carbonate and potassium nitrate
(h) hydrated copper sulphate and anhydrous copper sulphate
(i) ammonium sulphate and sodium sulphate.
(a) Neutral gas does not effect litmus paper. Acidic gas turns blue litmus paper red and basic gas turns red litmus blue.
(b) Oxygen is obtained by heating KMNO4 whereas hydrogen gas is obtained with the action of Zn and dil H2SO4.
(c) No effect of CO2 on KMnO4 or K2Cr2O7 whereas SO2 turns K2Cr2O7 from orange to green.
(d) Chlorine decolourises the colouring matter whereas HCl does not.
(e) H2S gas turns KMnO4 from pink to colourless and NO2 liberates violet vapours with KI.
(f) NH3 turns red litmus blue and S02 turns blue litmus red.
(g) Lime water turns zinc carbonate milky and no effect on potassium nitrate.
(h) Hydrated copper sulphate anhydrous copper sulphate. Take some dry CuSO4 on filter paper. It will be white in colour.
anhydrous copper sulphate white in colour. CuSO4 (white powder)
Now keep it in air for some time, it will absorb water vapous from atmosphers, its colour will change to blue.
(i) Ammonium sulphate and sodium sulphate : When ammonium sulphate is heated with NaOH, gas ammonia is producedwhich turns red litmus blue. But sodium sulphate has no reaction with NaOH.
Give a chemical test to distinguish between the following:
- Sodium carbonate and sodium sulphate
- Potassium chloride and potassium nitrate
- Copper carbonate and copper sulphite
- Lead chloride and lead sulphide
- Iron (II) sulphate and iron (III) sulphate
- Calcium sulphate and zinc sulphate
- Lead nitrate and zinc nitrate
- Copper sulphate and calcium sulphate
- Manganese dioxide and copper (II) oxide
- dil. HCl, dil. HNO3, dil. H2SO4.
[explain the procedure for the preparation of the solutions for the above tests wherever required]
(i) Sodium carbonate and sodium sulphate : Add BaCl2 solution to Na2CO3,a white precipitates produced which are soluble in dil. HCl.
(ii) Add cone. H2SO4 to potassium chloride and heat.
colourless gas produced which gives dense-white fumes when a glass rod dipped in ammonia is brought near it.
To the salt solution potassium nitrate, add cone. H2SO4 and copper turnings and heat.
Reddish brown fumes evolved which gives violvet vapours and turns potassium iodide paper brown.
(iii) On adding dilute H2SO4 to copper carbonate acid heating, a colorless odour less gas is evolved which turns lime water milky and has no effect on KMnO4 or K2Cr2O7 solution.
CO2 gas turns lime water milky.
Now add dil. H2SO4 to copper sulphite and heat.
A colourless gas with suffocating odour evolved which turns lime water milky and changes then pink colour of acidified KMnO4 to colourless and orange colour of acidified K2Cr2O7 to clear green.
(iv) Added MnO2 and cone. H2SO4 to the salt Lead Chloride and heat it.
A greenish coloured yellow coloured gas with punget odour is evolved which turns moist starch iodide paper blue black.
Now add dil. H2SO4 to Lead sulphide and heat.
Colourless gas with rotten egg smell is evolved. The gas evolved turns moist lead acetate paper silvery black.
(v) Iron (II) sulphate is when reacted with small amount of NaOH solution, dirty green precipitates of Iron (II) hydroxide are produced which are insoluble in excess of NaOH.
Iron (III) sulphate is when reacted with small amount of NaOH solution, reddish brown precipitates of Fe(OH)3 are formed which are insoluble in excess of NaOH.
(vi) Add sol. of NaOH to calcium sulphate solution, milky white ppts. of calcium hydroxide are formed which are soluble in excess of NaOH.
Now add NaOH to zinc sulphate a white ppts of Zn(OH)2 are produced which are soluble in excess of NaOH.
Also when sol. of NH4OH is add to CaSO4, no ppts. are formed i. e., no reaction whereas when a sol. of NH4OH is add to ZnSO4, gelatinous white ppts. are formed which are soluble is excess of NH4OH.
(vii) When a sol. of NH4OH in small amount is added to lead nitrate sol. a chalky white precipitates of lead hydroxide are produced. The precipitats so formed are unsoluble in excess of NH4OH.
Now add NH4(OH) in small amount to zinc nitrate, a Gelatinous white precipitates of Zn(OH)2 are formed which are soluble in excess of NH4OH.
(viii) When a sol. of NaOH in small amount is added to copper sulphate, pale blue precipitates of copper (II) hydroxide are formed which are insoluble in excess of NaOH.
Now add sol. of NaOH to calcium sulphate sol. milky white ppts. of Ca(OH)2 are formed which are insoluble in excess of NaOH.
(ix) Test : (i) Add cone. HCl to the sol. and heat, (ii) Filter the sol. after reaction.
Manganese dioxide (Black) : Greenish coloured gas is evolved MnO2 + 4HCl → MnCl2 + 2H2O + Cl2 Filterate is brownish in colour.
Copper (II) oxide : There is no evolution of chlorine gas. CuO → 2HCl + CuCl2 + H2O Filterate is blueish colour.
(x) Dil. HCl is prepared by dissolving HCl gas in water. It ionises to H3O+ and CT ions. HCl gas is prepared by explosive mixture of equal volumes of hydrogen gas and chlorine gas.
Identify the cation (positive ion) and anion (negative ion) in the following substances, A, B and C. Also identify P, Q, R, S, T, U, V, W.
(a) Substance ‘A’is water soluble and gives a curdy white precipitate ‘P’ with silver nitrate solution. ‘P’ is soluble in ammonium hydroxide but insoluble in dil. HNO3. Substance ‘A’ reacts with ammonium hydroxide solution to give a white precipitate ‘Q’ soluble in excess of NH4OH.
(b) A solution of substance ‘B’ is added to barium chloride solution. A white ppt. ‘R’ is formed, insoluble in dil. HCl or HNO3. A dirty green ppt. ‘S’ is formed on addition of ammonium hydroxide to a solution of ‘B’ and the precipitate is insoluble in excess of ammonium hydroxide.
(c) Substance ‘C’ is a coloured, crystalline salt which on heating decomposes leaving a black residue ‘T’. On addition of copper turnings and cone. H2SO2 to ‘C’ a coloured acidic gas ‘U’ is evolved on heating. A solution of ‘C’ is added to NaOH soln. until in excess. A pale blue ppt. ‘P’ is obtained insoluble in excess of NaOH. A solution of ‘C’ then added to NH4 soln. in excess to gives an inky blue solution ‘V’. A solution of ‘C’ is warmed and hydrogen sulphide gas is passed through it. A black ppt. ‘W’ appears.
Unit Test Paper — Chemistry Practicals
Q.1. Match the ‘cations’ A to F and the solubility of ppt. G or H with the correct colours from ‘X’ and ‘Y’.
Q.2. Select the correct ‘anion’ of a salt from the anions given, which matches with description 1 to 5.
- The salt soln. reacts with AgNO3 soln. to give a white ppt. insoluble in dil. HNO3.
- The salt soln. reacts with Ba(NO3)2 soln. to give a white ppt. insoluble in dil. HNO3.
- The salt soln. reacts with Ba(NO3)2 soln. to give a white ppt. soluble in dil. HNO3 but insoluble in dil. H2SO4.
- The salt reacts with dil. H2SO4 on heating evolving a gas which turns KMnO4 soln. pink to colourless.
- The salt reacts with cone. H2SO4 on heating evolving a coloured gas which turns potassium iodide paper brown.
- Cl– ion(D)
- SO42-– ion(C)
- C032- ion (A)
- S2- ion (E)
- NO31- ion(B)
Q.3. Give balanced equations for the conversions A and B.
Q.4. Complete the table given below :
Q.5. Select the correct word from the words in bracket.
- The solution which on heating with CaCO3 evolves CO2 gas. [cone. H2SO4 / dil.H2SO4 / dil. HCl]
- The solution which can be used to distinguish an ammonium salt from a sodium salt. [CuCl2 soln. / NH4OH / dil. H2SO4 / AgNO3 soln.]
- The pH of blood is around 7.4, of saliva is 6.5 and of acid rain is around 4.5. The solution which is slightly alkaline of the three, [saliva / acid rain / blood]
- Decomposition of [NaCl / NaHCO3 / NaNO3] by dil. H2SO4, forms an unstable acid.
- A metal which reacts with an alkali to liberate hydrogen, [iron / copper / aluminium]
- dil. HCl
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