Hey there! We receieved your request
Stay Tuned as we are going to contact you within 1 Hour
One of our academic counsellors will contact you within 1 working day.
Click to Chat
1800-5470-145
+91 7353221155
Use Coupon: CART20 and get 20% off on all online Study Material
Complete Your Registration (Step 2 of 2 )
Sit and relax as our customer representative will contact you within 1 business day
OTP to be sent to Change
Ferrous sulphate (Green vitriol), FeSO4.7H2O
Ferric oxide, Fe2O3
Ferric Chloride, FeCl3
Copper(II) Sulphate Pentahydrate or Blue Vitriol, CuSO4.5H2O
Silver Nitrate, AgNO3
Halides of Silver
Mercury (I) Chloride / Mercurous Chloride /Calomel, (Hg2Cl2)
Mercury (II) Chloride HgCl2
Mercury-II Iodide
Potassium Dichromate, K2Cr2O7
Potassium Permanganate, KMnO4
Related Resources
It occurs in nature as copperas and commonly known as hara Kasis.
By dissolving scrap Fe in dil. H2SO4 From Kipp’s waste which contains ferrous sulphate with some free H2SO4; the latter is neutralised with scrap iron forming FeSO4 and hydrogen. By the action of air and water on iron pyrites. The solution is treated with scrap iron to remove H2SO4 and to reduce Fe2(SO4)3 to FeSO4.
By dissolving scrap Fe in dil. H2SO4
From Kipp’s waste which contains ferrous sulphate with some free H2SO4; the latter is neutralised with scrap iron forming FeSO4 and hydrogen.
By the action of air and water on iron pyrites. The solution is treated with scrap iron to remove H2SO4 and to reduce Fe2(SO4)3 to FeSO4.
Hydrated and anhydrous FeSO4 are green and white in colour respectively. It is isomorphous with epsom salt, MgSO4.7H2O and ZnSO4.7H2O. It effervesces on exposure to air. Light green crystals of FeSO4 lose water and turn brown on exposure to air, due to oxidation. On heating at 300°C it gives anhydrous FeSO4 which on further heating gives Fe2O3 and SO2. Like other ferrous salts, it takes up HNO3 forming brown coloured double compound, Fe(NO)SO4, nitroso ferrous sulphate (Ring test for nitrates). It decolourises acidified potassium permanganate and turns acidified dichromate green (reducing character). It forms double salts with sulphates of alkali metals with general formula R2SO4.FeSO4.6H2O. With ammonium sulphate, it forms a double salt known as ferrous ammonium sulphate or Mohr’s salt, FeSO4.(NH4)2SO4.6H2O. It does not effervesce. It ionises in solution to gives Fe2+, NH4+ and SO42– ions.
Hydrated and anhydrous FeSO4 are green and white in colour respectively. It is isomorphous with epsom salt, MgSO4.7H2O and ZnSO4.7H2O. It effervesces on exposure to air.
Light green crystals of FeSO4 lose water and turn brown on exposure to air, due to oxidation.
On heating at 300°C it gives anhydrous FeSO4 which on further heating gives Fe2O3 and SO2.
Like other ferrous salts, it takes up HNO3 forming brown coloured double compound, Fe(NO)SO4, nitroso ferrous sulphate (Ring test for nitrates).
It decolourises acidified potassium permanganate and turns acidified dichromate green (reducing character).
It forms double salts with sulphates of alkali metals with general formula R2SO4.FeSO4.6H2O. With ammonium sulphate, it forms a double salt known as ferrous ammonium sulphate or Mohr’s salt, FeSO4.(NH4)2SO4.6H2O. It does not effervesce. It ionises in solution to gives Fe2+, NH4+ and SO42– ions.
It occurs in nature as haematite. Fe2O3 is a red powder, insoluble in H2O and not acted upon by air or H2O It is amphoteric in nature and reacts with acids and alkalies. It is reduced to iron by H2,C and CO. It is used as a catalyst in the oxidation of CO to CO2 in the Bosch process.
It occurs in nature as haematite.
Fe2O3 is a red powder, insoluble in H2O and not acted upon by air or H2O
It is amphoteric in nature and reacts with acids and alkalies.
It is reduced to iron by H2,C and CO.
It is used as a catalyst in the oxidation of CO to CO2 in the Bosch process.
Hydrated ferric chloride (FeCl3.6H2O) can be prepared by dissolving iron, Fe(OH)3 or ferric oxide in dil. HCl. Reaction of Fe with dry Cl2 gives anhydrous FeCl3,
Hydrated ferric chloride (FeCl3.6H2O) can be prepared by dissolving iron, Fe(OH)3 or ferric oxide in dil. HCl.
Reaction of Fe with dry Cl2 gives anhydrous FeCl3,
Properties of Ferric Chloride
Anhydrous salt is yellow, deliquescent compound and highly soluble in H2O. Its aqueous solution is acidic due to hydrolysis. On heating it gives FeCl2 and Cl2. It oxidizes H2S to S, SO2 to H2SO4, SnCl2 to SnCl4 and Na2S2O3 to Na2S4O6
Anhydrous salt is yellow, deliquescent compound and highly soluble in H2O.
Its aqueous solution is acidic due to hydrolysis.
On heating it gives FeCl2 and Cl2.
It oxidizes H2S to S, SO2 to H2SO4, SnCl2 to SnCl4 and Na2S2O3 to Na2S4O6
In the laboratory, it is prepared by dissolving cupric oxide, cupric hydroxide or carbonate in dilute H2SO4.
CuO + H2SO4 → CuSO4 + H2O
Cu(OH)2 + H2SO4 → CuSO4 + 2H2O
CuCO3 + H2SO4 → CuSO4 + H2O + CO2
The solution of CuSO4 thus obtained is concentrated and cooled when crystals of blue vitriol, CuSO4.5H2O separates out.
Commercially it is prepared by the action of hot dilute sulphuric acid on scrap copper in the presence of air.
2Cu + 2H2SO4 + O2 → 2CuSO4 + 2H2O
(1) Action of Heat
It has 5 molecules of water of crystallisation; all of which can be removed on heating, to form colourless CuSO4 (again coloured with H2O). CuSO4.5H2O CuSO4.H2O CuSO4 (white ppt) CuO + SO3 At high temperature it forms cupric oxide. It forms double salts with alkali sulphates, e.g. K2SO4.CuSO4.6H2O When treated with NH4OH, it first forms precipitate of cupric hydroxide copper (II) sulphate (Schweitzer’s reagent), used for dissolving cellulose in the manufacture of artificial silk. It reacts with KCN forming a complex compound K3[Cu(CN)4]. It liberates iodine from soluble iodides.
It has 5 molecules of water of crystallisation; all of which can be removed on heating, to form colourless CuSO4 (again coloured with H2O). CuSO4.5H2O CuSO4.H2O CuSO4 (white ppt) CuO + SO3
At high temperature it forms cupric oxide.
It forms double salts with alkali sulphates, e.g. K2SO4.CuSO4.6H2O
When treated with NH4OH, it first forms precipitate of cupric hydroxide copper (II) sulphate (Schweitzer’s reagent), used for dissolving cellulose in the manufacture of artificial silk.
It reacts with KCN forming a complex compound K3[Cu(CN)4].
It liberates iodine from soluble iodides.
(2) Action of Alkalis
CuSO4 + 2NaOH → Cu(OH)2 + Na2SO4
With NH4OH it forms tetraamminecopper (II) sulphate
CuSO4 + 4NH4OH → [Cu(NH3)4]SO4 + 4H2O
(3) Reaction with KI
CuSO4 + 2KI → CuI2 + K2SO4
2Cul2 → 2Cul + l2
The liberation of iodine in this reaction is quantitative. Therefore, this reaction is used to estimate copper volumetrically.
It is used as an electrolyte in electroplating, electrotyping and refining of copper. It is used in reservoirs and swimming pools to prevent the growth of weeds. It is used as a fungicide under the name Bordeaux mixture, which is a mixture of CuSO4 and slaked lime Ca(OH)2. Anhydrous CuSO4 is used for detection of moisture in organic liquids such as alcohol, ether etc.
It is used as an electrolyte in electroplating, electrotyping and refining of copper.
It is used in reservoirs and swimming pools to prevent the growth of weeds.
It is used as a fungicide under the name Bordeaux mixture, which is a mixture of CuSO4 and slaked lime Ca(OH)2.
Anhydrous CuSO4 is used for detection of moisture in organic liquids such as alcohol, ether etc.
Silver nitrate is prepared by the action of dilute nitric acid on silver and then evaporating the solution to crystallization.
3Ag + 4HNO3 → 3AgNO3 + NO ↑ + 2H2O
It decomposes on heating.
2AgNO3 2AgNO2 2Ag + 2NO2
On coming into contact with organic matter like skin or clothes, it is reduced to finely – divided silver, giving a black stain.
(2) Precipitation Reactions
Silver nitrat forms precipitates with some salt solutions which help in the detection of acid radicals.
Some of the precipitation reactions are:
NaCl + AgNO3 → AgCl ↓ + NaNO3 NaPO4 + 3AgNO3 → Ag3PO4 ↓ + 3NaNO3 K2CrO4 + 3AgNO3 → AgCrO ↓ + 2KNO3 Na2S + 2AgNO3 → Ag2S ↓ + 2NaNO3 Na2S2O3 + 2AgNO3 → Ag2S2O3 ↓ + 2NaNO3 Na2C2O4 + 2AgNO3 → Ag2C2O4 ↓ + 2NaNO3 Na3BO3 + 3AgNO3 → Ag3BO3 ↓ + 3NaNO3
NaCl + AgNO3 → AgCl ↓ + NaNO3
NaPO4 + 3AgNO3 → Ag3PO4 ↓ + 3NaNO3
K2CrO4 + 3AgNO3 → AgCrO ↓ + 2KNO3
Na2S + 2AgNO3 → Ag2S ↓ + 2NaNO3
Na2S2O3 + 2AgNO3 → Ag2S2O3 ↓ + 2NaNO3
Na2C2O4 + 2AgNO3 → Ag2C2O4 ↓ + 2NaNO3
Na3BO3 + 3AgNO3 → Ag3BO3 ↓ + 3NaNO3
Uses of Silver Nitrate
It is used for
Preparing silver halides which are used in photography. For making inks and hair dyes. In qualitative and quantitative analysis. For silvering of glass, i.e. preparation of mirrors.
Preparing silver halides which are used in photography.
For making inks and hair dyes.
In qualitative and quantitative analysis.
For silvering of glass, i.e. preparation of mirrors.
Silver halides are prepared by the action of sodium or potassium halide on silver nitrate solution (except for AgF)
AgNO3 + NaX → AgX(s) + NaNO3
Silver fluoride is prepared by the action of HF on silver (I) oxide.
2HF + 2Ag2O → 2AgF + H2O
Properties of Silver Halides
AgCl is white solid, AgBr is a pale yellow solid and AgI is a yellow solid. AgF is soluble in water whereas other halides are insoluble in water. AgCl dissolves in ammonia to form a complex. AgCl + 2NH4OH → [Ag(NH3)2]Cl + 2H2O AgBr is partially soluble and AgI is insoluble in NH4OH. All the silver halides dissolve in potassium cyanide and Na2S2O3 solution to form complexes. AgCl + 2KCN → K [Ag(CN)2] + KCl AgCl + 2Na2S2O3 → Na2[Ag(S2O3)2] + NaCl
AgCl is white solid, AgBr is a pale yellow solid and AgI is a yellow solid.
AgF is soluble in water whereas other halides are insoluble in water. AgCl dissolves in ammonia to form a complex.
AgCl + 2NH4OH → [Ag(NH3)2]Cl + 2H2O
AgBr is partially soluble and AgI is insoluble in NH4OH.
All the silver halides dissolve in potassium cyanide and Na2S2O3 solution to form complexes. AgCl + 2KCN → K [Ag(CN)2] + KCl AgCl + 2Na2S2O3 → Na2[Ag(S2O3)2] + NaCl
All silver halides (particularly AgBr) are photosensitive and hence are widely used in photography.
It can be prepared by mixing a chloride solution with a mercury (I) salt solution.
Hg2(NO3)2 + 2NaCl → Hg2Cl2 ↓ + 2NaNO3
It can also prepared by heating a mixture of mercuric chloride and mercury in an iron vessel.
Properties of Mercurous Chloride
It is a white power insoluble in water but soluble in chlorine water. Hg2Cl2 + Cl2 → 2HgCl2 It decomposes on heating to HgCl2 Hg2Cl2 → HgCl2 + Hg On treatment with ammonia, if turns black due to the formation of finely divided mercury. Hg2Cl2 + 2NH3→ Hg + Hg(NH2)Cl + NH4Cl
It is a white power insoluble in water but soluble in chlorine water. Hg2Cl2 + Cl2 → 2HgCl2
It decomposes on heating to HgCl2 Hg2Cl2 → HgCl2 + Hg
On treatment with ammonia, if turns black due to the formation of finely divided mercury. Hg2Cl2 + 2NH3→ Hg + Hg(NH2)Cl + NH4Cl
Uses of Mercurous Chloride
In making standard calomel electrode and As a purgative in medicine.
In making standard calomel electrode and
As a purgative in medicine.
It is prepared by passing dry chlorine over heated mercury. HgCl2 + Hg → Hg2Cl2 It is also obtained by treating HgO with HCl HgO + 2HCl → HgCl2 + H2O Commercially, it is prepared by heating a mixture of HgSO4 and NaCl in the presence of MnO2 HgSO4 + 2NaCl HgCl2 + Na2SO4
Properties of Mercury (II) Chloride
It is a white crystalline solid sparingly soluble in cold water but soluble in hot water. Its solubility can be increased by adding Cl-.
HgCl2 + 2Cl– → [HgCl4]2–
It is readily soluble in organic solvents suggesting its covalent nature.
When treated with SnCl2 it is reduced to mercury.
2HgCl2 + SnCl2 → SnCl4 + Hg2Cl2
Hg2Cl2 + SnCl2 → 2Hg + SnCl4
When Cu turnings are placed in its contact a shining grey film of mercury deposits over them.
HgCl2 + Cu → Hg + CuCl2
Uses of Mercury (II) Chloride
It is used for preserving wood and hides and for making fungicides.
Preparation of Mercury (II) Iodide
It is prepared by treating HgCl2 with KI.
HgCl2 + 2Kl → Hgl2 + 2KCl
Properties of Mercury (II) Iodide
Mercuric iodide exists in two forms, i.e. red and yellow. The yellow form is stable above 400 K white the red form is stable below this temperature.
It readily dissolves in KI forming a complex
HgI2 + 2KI → K2[HgI4]
An alkaline solution of K2HgI4 is called Nessler’s reagent and is used to detect the presence of NH4+ with which it gives a brown precipitate due to the formation of iodide of Million’s base.
Uses of Mercury (II) Iodide
It is used to prepare Nessler’s reagent and for making ointments for treating skin infections.
Preparation of Potassium Dichromate
It is prepared from the ore called chromate or ferrochrome or chrome iron, FeO.Cr2O3. The various steps involved are
(a) Preparation of sodium chromate
4FeO.Cr2O3 + O2 → Fe2O3 + 4Cr2O3
4Na2CO3 + 2Cr2O3 + 3O2 → 4Na2CrO4 + 4CO2
(b) Conversion of sodium chromate into sodium dichromate.
2Na2CrO4 + H2SO4 → Na2Cr2O7 + Na2SO4 + H2O
(c) Conversion of sodium dichromate into potassium dichromate.
Na2Cr2O7 + 2KCl → K2Cr2O7 + 2NaCl
It forms orange red crystals. It is moderately soluble in cold water but freely soluble in hot water.
1. Action of heat
When heated, it decomposed to its chromate
4K2Cr2O7 4K2CrO4 + 2Cr2O3 + 3O2
2. Action of alkalis
With alkalis it is converted into chromate which on acidifying gives back dichromate.
K2Cr2O7 + 2KOH → 2K2CrO4 + H2O
2K2Cr2O7 + H2SO4 → K2Cr2O7 + K2SO4 + H2O
In dichromate solution the Cr2O72– ions are in equilibrium with Cr2O72– ions at pH = 4.
Cr2O72– + H2O 2CrO42– + 2Hl
orange red yellow
3. Action of conc. H2SO4 solution
In cold conditions K2Cr2O7 + 2H2SO4 ———→ 2CrO3 + 2KHSO4 + H2O
In hot conditions 2K2Cr2O7 + 8H2SO4 ———→ 2K2SO4 + 2Cr2(SO4)3 + 8H2O + 3O2
4. Oxidising properties
It is a powerful oxidising agent. In the presence of dil. H2SO4 it furnishes 3 atoms of available oxygen.
K2Cr2O7 + 4H2SO4 → K2SO4 + Cr2(SO4)3 + 4H2O + 3O
Some of the oxidizing properties of K2Cr2O7 are
It liberates I2 from KI K2Cr2O7 + 7H2SO4 + 6Kl → 4K2SO4 + Cr2(SO4)3 + 3l2 + 7H2O It oxidises ferrous salts to ferric salts K2Cr2O7 + 7H2SO4 + 6FeSO4 → K2SO4 + Cr2(SO4)3 + 3Fe2(SO4)3 + 2H2O It oxidises S-2 to S K2Cr2O7 + 4H2SO4 + 3H2S → K2SO4 + Cr2(SO4)3 + 7H2O + 3S It oxidises nitrites to nitrates K2Cr2O7 + 4H2SO4 + 3NaNO2 → K2SO4 + Cr2(SO4)3 + 3NaNO3 + 4H2O It oxidises SO2 to SO42– K2Cr2O7 + H2SO4 + 3SO2 → K2SO4 + Cr2(SO4)3 + 3H2O It oxidises ethyl alcohol to acetaldehyde and acetic acid.
It liberates I2 from KI K2Cr2O7 + 7H2SO4 + 6Kl → 4K2SO4 + Cr2(SO4)3 + 3l2 + 7H2O
It oxidises ferrous salts to ferric salts K2Cr2O7 + 7H2SO4 + 6FeSO4 → K2SO4 + Cr2(SO4)3 + 3Fe2(SO4)3 + 2H2O
It oxidises S-2 to S K2Cr2O7 + 4H2SO4 + 3H2S → K2SO4 + Cr2(SO4)3 + 7H2O + 3S
It oxidises nitrites to nitrates K2Cr2O7 + 4H2SO4 + 3NaNO2 → K2SO4 + Cr2(SO4)3 + 3NaNO3 + 4H2O
It oxidises SO2 to SO42– K2Cr2O7 + H2SO4 + 3SO2 → K2SO4 + Cr2(SO4)3 + 3H2O
It oxidises ethyl alcohol to acetaldehyde and acetic acid.
5. Chromyl Chloride Test
When heated with conc. HCl or with a chloride in the presence of sulphuric acid, reddish brown vapours of chromyl chloride are obtained.
K2Cr2O7 + 4KCl + 6H2SO4 → 2CrO2Cl2 + 6KHSO4 + 3H2O
Thus reaction is used in the detection of chloride ions in qualitative analysis.
Uses of Potassium Dicromate
In volumetric analysis for the estimation of Fe2+ and I-. In chrome tanning in leather industry. In photography and in hardening gelatin film.
In volumetric analysis for the estimation of Fe2+ and I-.
In chrome tanning in leather industry.
In photography and in hardening gelatin film.
It is prepared from the mineral pyrolusite, MnO2. The preparation involves the following steps
Conversion of MnO2 into potassium manganate.
When finely powdered MnO2 is fused with KOH. K2MnO4 is obtained.
2MnO2 + 4KOH + O2 → 2K2MnO4 + 2H2O
Oxidation of potassium manganate into permanganate
(a) Chemical oxidation
K2MnO4 is oxidised to KMnO4 by bubbling CO2 or Cl2 or ozone into the former.
3K2MnO4 + 2CO2 → 2KMnO4 + MnO2 + 2K2CO3
(b) Electrolytic oxidation
The manganate solution is electrolysed between iron electrodes. The oxygen evolved at anode converts manganate into permanganate.
2K2MnO2 + H2O + O → 2K2MnO4 + 2KOH
Properties of Potassium Permanganate
KMnO4 exists as deep purple prisms. It is moderately soluble in water at room temperature and its solubility in water increases with temperature.
(i) Action of heat
When heated it decomposes to K2MnO4.
2KMnO4 → K2MnO4 + MnO2 + O2
(ii) Action of conc. H2SO4
With cold conc. H2SO4 it gives Mn2O7 which on warming decomposes to MnO2.
2MnO2 + 2H2SO4 → Mn2O7 + 2KHSO4 + 2H2O
2Mn2O7 4MnO2 + 3O2
With hot Conc. H2SO4 O2 is evolved
4KMnO4 + 6H2SO4 → 2K2SO4 + 4MnSO4 + 6H2O + 5O2
(iii) Oxidising properties
KMnO4 is a powerful oxidizing agent. The actual oxidizing action depends upon the medium i.e. acidic, basic or neutral.
In neutral solution, it acts as moderate oxidizing agent.
2KMnO4 + H2O → 2KOH + 2MnO2 + 3O
Some oxidizing properties of KMnO4 in neutral medium are
2KMnO4 + 3Na2S2O3 + H2O → 3K2SO4 + 8MnO2 + 3Na2SO4 + 2KOH
In strong alkaline solution, it is converted into
2KMnO4 + 2KOH → 2K2MnO4 + H2O + O
2KMnO4 + H2O + Kl → 2MnO2 + 2KOH + KlO3
In acidic medium, Mn+7 is converted into Mn+2
Some other reactions are
2KMnO4 + 3H2SO4 + 5H2S → K2SO4 + 2MnSO4 + 3H2O + 5S 2KMnO4 + 5SO2 + 2H2O → K2SO4 + 2MnSO4 + 2H2SO4 2KMnO4 + 3H2SO4 + 5KNO2 → K2SO4 + 2MnSO4 + 3H2O + 5KNO3 2KMnO4 + 3H2SO4 + 5C2H2O4 → K2SO4 + 2MnSO4 + 8H2O + 10CO2 2KMnO4 + 8H2SO4 + 10FeSO4 → K2SO4 + 2MnSO4 + 5Fe2(SO4)3 + 8H2O 2KMnO4 + 3H2SO4 + 10Kl → K2SO4 + 2MnSO4 + 8H2O + 5l2
2KMnO4 + 3H2SO4 + 5H2S → K2SO4 + 2MnSO4 + 3H2O + 5S
2KMnO4 + 5SO2 + 2H2O → K2SO4 + 2MnSO4 + 2H2SO4
2KMnO4 + 3H2SO4 + 5KNO2 → K2SO4 + 2MnSO4 + 3H2O + 5KNO3
2KMnO4 + 3H2SO4 + 5C2H2O4 → K2SO4 + 2MnSO4 + 8H2O + 10CO2
2KMnO4 + 8H2SO4 + 10FeSO4 → K2SO4 + 2MnSO4 + 5Fe2(SO4)3 + 8H2O
2KMnO4 + 3H2SO4 + 10Kl → K2SO4 + 2MnSO4 + 8H2O + 5l2
Uses of Potassium Permanganate
It is used in volumetric analysis for the estimation of ferrous salts, oxalates, iodides and H2O2. It is used as oxidizing agent in the laboratory as well as in industry. It is also used as disinfectant and germicide.
It is used in volumetric analysis for the estimation of ferrous salts, oxalates, iodides and H2O2.
It is used as oxidizing agent in the laboratory as well as in industry.
It is also used as disinfectant and germicide.
Question 1: CuSO4.5H2O
a. CuSO4.H2O
b. CuSO4
c. CuO +SO2
d. Cu +SO3
Question 2: When heated with conc. HCl or with a chloride in the presence of sulphuric acid, reddish brown vapours of
a. potassium dichromate
b. chromyl chloride
c. chromic acid
d. chlorine
Question 3: Potassium dicromate oxidises nitrites to
a. nitrates
b. dinitrogen
c. nitrogen dioxide
d. nitrogen trioxide
Question 4: Hydrated ferric chloride (FeCl3.6H2O) can be prepared by dissolving iron, Fe(OH)3 or ferric oxide in
a. dil. HCl.
b. dil NaOH
c. H2O
d. NH3
Q.1
Q.2
Q.3
Q.4
a
b
Its always helpful to have a look at past year papers of IIT JEE
Click here to refer the syllabus of chemistry for IIT JEE
You can also refer to general characteristics of transition elements
Get your questions answered by the expert for free
You will get reply from our expert in sometime.
We will notify you when Our expert answers your question. To View your Question
General Properties of the Transition Elements...
Electronic Configuration of Elements Table of...
Position in the Periodic Table Table of Content...
Solved Problems on Transition Elements Problem 1:...
The Actinoids Table of Content Introduction to The...
General Characteristics of Transition Elements...
The Lanthanoids Table of Content Position in the...
Some Applications of d- and f- Block Elements...
Lanthanides and Actinides Table of Content...