Chemistry equations for ICSE Class 10

©2015 All rights reserved. Srikanth KS and Shambavi Ganesh Learn and Achieve

CHEMISTRY EQUATIONS FOR ICSE CLASS 10

Contents Periodic table .......................................................................................................................................... 2

How to remember the first three periods .......................................................................................... 2

Oxidation vs. reduction: ............................................................................................................... 3

ACIDS BASES AND SALTS ......................................................................................................................... 3

ANALYTICAL CHEMISTRY ......................................................................................................................... 7

ELECTROLYSIS .......................................................................................................................................... 8

METALLURGY ........................................................................................................................................ 10

STUDY OF COMPOUNDS: HCl ................................................................................................................ 11

STUDY OF COMPOUNDS: AMMONIA.................................................................................................... 12

STUDY OF COMPOUNDS: NITRIC ACID .................................................................................................. 14

STUDY OF COMPOUNDS: SULPHURIC ACID .......................................................................................... 14

ORGANIC CHEMISTRY ........................................................................................................................... 16

ALKANES ............................................................................................................................................ 16

ALKENES ............................................................................................................................................ 17

ALKYNES ............................................................................................................................................ 17

ALCOHOLS ......................................................................................................................................... 18

ACETIC ACID ...................................................................................................................................... 18

CARBOXYLIC ACIDS ............................................................................................................................ 18



Periodic table

How to remember the first three periods

Hi He Lied Because Boron Could Not Oxidize Fluorine.

New Nations Might Also Sign Peace Security Clause. Arthur King Can

Hi Hydrogen Atomic No 1

He Helium Atomic No 2

Lied Lithium Atomic No 3

Because Berilium Atomic No 4

Boron Boron Atomic No 5

Could Carbon Atomic No 6

Not Nitrogen Atomic No 7

Oxidize Oxygen Atomic No 8

Fluorine Fluorine Atomic No 9

New Neon Atomic No 10

Nations Sodium (Na) Atomic No 11

Might Magnesium (Mg) Atomic No 12

Also Aluminium Atomic No 13

Sign Silicon Atomic No 14

Peace Phosphorous Atomic No 15

Security Sulphur Atomic No 16

Clause Chlorine (Cl) Atomic No 17

Arthur Argon Atomic No 18

King Potassium (K) Atomic No 19

Can Caclium Atomic No 20

Group 1 (alkali metals)

Li Na K Rb Cs Fr

Lithium, Sodium, Potassium, Rubidium, Cesium, Francium

LIttle NAsty Kids RuB CatS FuR



Group 17 (halogens)

F Cl Br I At

Fluorine, Chlorine, Bromine, Iodine, Astatine

Fish Can't Breathe In Air.

We can easily get confused with Cations and anions

Remember this Cats has Paws Cations positive Don’t need to remember Anion as -ve

Oxidation vs. reduction: What happens at the Anode and what happens at the cathode?

Remember AN OIL RIG CAT

At the ANode, Oxidation Involves Loss of electrons.

Reduction Involves Gaining electrons at the CAThode

ACIDS BASES AND SALTS ACID

HCl + H2O H3O+ + Cl-

BASE

CuO + 2HCl → CuCl2 + H2O

ALKALI

NaOH[aq] Na+ + OH-

STRONG ACID

HNO3 + H2O H3O+ + NO3-

H2SO4 + 2H2O 2H3O+ + SO42-

WEAK ACID

CH3COOH CH3COO- + H+

STRONG ALKALI

NaOH[aq] Na+ + OH-

KOH[aq] K+ + OH-

WEAK ALKALI



NH4OH[aq] NH4+ + OH-

MONOBASIC ACID

HCl + H2O H3O+ + Cl-

NaOH + HCl NaCl + H2O

DIBASIC ACID

H2SO4 + 2H2O 2H3O+ + SO42-

NaOH + H2SO4 → NaHSO4 + H2O

2NaOH + H2SO4 → Na2SO4 + 2H2O

TRIBASIC ACID

H3PO4 + 3H2O 3H3O+ + PO43-

NaOH + H3PO4 → NaH2PO4 + H2O

2NaOH + H3PO4 Na2HPO4 + 2H2O

3NaOH + H3PO4 → Na3PO4 + 3H2O

MONOACIDIC BASE

NaOH[aq] Na+ + OH-

DIACIDIC BASE

Ca(OH)2[aq] Ca2+ + 2OH-

Cu(OH)2[aq] Cu2+ + 2OH-

ACIDS FROM NONMETALS

H2 + Cl2 → 2HCl

H2 + I2 → 2HI

ACIDS FROM ACIDIC OXIDES

CO2 + H2O → H2CO3

SO2 + H2O → H2SO3

SO3 + H2O → H2SO4

P2O5 + 3H2O → 2H3PO4

ACIDS FROM SALTS

KNO3 + H2SO4[conc.] KHSO4 + HNO3

NaCl + H2SO4[conc.] NaHSO4 + HCl

ACIDS BY OXIDATION OF NONMETALS

S + 6HNO3 → H2SO4 + 2H2O + 6NO2↑

BASES FROM METALS



4Na + O2 → 2Na2O

2Mg + O2 → 2MgO

BASES FROM BASIC OXIDES

K2O + H2O → 2KOH

Na2O + H2O → 2NaOH

BASES FROM ACTIVE METALS AND WATER

2K + 2H2O → 2KOH + H2↑

2Na + 2H2O → 2NaOH + H2↑

BASES FROM SALTS

AlCl3 + 3NaOH → 3NaCl + Al(OH)3↓

FeSO4 + 2NaOH → Na2SO4 + Fe(OH)2↓

BASES BY DECOMPOSITION OF SALTS

2Pb(NO3)2 → 2PbO +4NO2 + O2↑

REACTION OF CHLORIDES NITRATES BICARBONATES AND CARBONATES WITH ACIDS


NaNO3 + H2SO4[conc.] NaHSO4 + HNO3

2NaHCO3 + H2SO4[dil] → NA2SO4 + 2H2O + 2CO2↑

Na2CO3 + 2HCl[dil] → 2NaCl + H2O + CO2↑

FORMATION OF ACID RAIN

S + O2 → SO2

H2O + SO2 → H2SO3[aq]

2SO2 + O2 → 2SO3

H2O + SO3 → H2SO4[aq]

N2 + O2 → 2NO [at high temp.]

2NO + O2 → 2NO2

H2O + 2NO2 → HNO2 + HNO3

PREPARATION OF ACIDS

NEUTRALIZATION

CuO + H2SO4[dil] → CuSO4 + H2O

PbO + 2HNO3[dil] → Pb(NO3)2 + 2H2O

Cu(OH)2 + H2SO4[dil] → CuSO4 + 2H2O

Pb(OH)2 + 2HNO3[dil] → Pb(NO3)2 + 2H2O

PbCO3 + 2HNO3[dil] → Pb(NO3)2 + H2O + CO2↑

ZnCO3 + 2HNO3[dil] → Zn(NO3)2 + H2O + CO2↑

CuCO3 + H2SO4[dil] → CuSO4 + H2O + CO2↑



NEUTRALIZATON (TITRATION INVOLVED)

NaOH + HCl[dil] → NaCl + H2O

NaOH + HNO3[dil] → NaNO3 + H2O

NH4OH + HCl[dil] → NH4Cl + H2O

Na2CO3 + H2SO4[dil] → Na2SO4 + H2O + CO2↑

(NH4)2CO3 + 2HCl[dil] → 2NH4Cl + H2O + CO2↑

(NH4)2CO3 + H2SO4[dil] → (NH4)2SO4 + H2O + CO2↑

SIMPLE DISPLACEMENT

Fe + H2SO4[dil] →FeSO4 + H2↑

Fe + 2HCl[dil] → FeCl2 + H2↑

Zn + H2SO4[dil] → ZnSO4 + H2↑

Mg + 2HCl[dil] → MgCl2 + H2↑

DIRECT COMBINATION (SYNTHESIS)

2Fe + 3Cl2 → 2FeCl3

2Al + 3Cl2 → 2AlCl3

Fe + S → FeS↓

Zn + S → ZnS↓

Pb + S → PbS↓

DOUBLE DECOMPOSITION (PRECIPITATION)

Pb(NO3)2 + 2NaCl → 2NaNO3 + PbCl2↓

CaCl2 + Na2CO3 → 2NaCl + CaCO3↓

ZnSO4 + (NH4)2CO3 → (NH4)2SO4 + ZnCO3↓

Zn(NO3)2 + Na2CO3 → 2NaNO3 + ZnCO3↓

Pb(NO3)2 + Na2SO4 → 2NaNO3 + PbSO4↓

PREPARATION OF PbCl2 FROM PbO

PbO + 2HNO3[dil] →Pb(NO3)2 + H2O

Pb(NO3)2 + 2NaCl → 2NaNO3 + PbCl2↓

PREPARATION OF PbSO4 FROM PbCO3

PbCO3 + 2HNO3 → Pb(NO3)2 + H2O + CO2↑

Pb(NO3)2 + Na2SO4→ 2NaNO3 + PbSO4↓

PREPARATION OF PbCl2 FROM PbCO3

PbCO3 + 2HNO3 → Pb(NO3)2 + H2O + CO2↑

Pb(NO3)2 + 2NaCl → 2 NaNO3 + PbCl2↓

HYDROLYSIS OF SALTS

NH4Cl + H2O → NH4OH + HCl



NaHCO3 + H2O → NaOH + H2CO3

Na2CO3 + 2H2O → 2NaOH + H2CO3

NaCl + H2O → NaOH + HCl

MgCl2 + 2H2O → Mg(OH)2 + 2HCl

ANALYTICAL CHEMISTRY REACTIONS OF NaOH SOLUTION ON SALTS

Ca(NO3)2 + 2NaOH → 2NaNO3 + Ca(OH)2↓(white ppt-slightly soluble)

MgCl2 + 2NaOH → 2NaCl + Mg(OH)2↓(dull white ppt-insoluble)

FeSO4 + 2NaOH → 2Na2SO4 + Fe(OH)2↓(dirty green ppt-insoluble)

FeCl3 + 3NaOH → 3NaCl + Fe(OH)3↓(reddish brown ppt-insoluble)

CuSO4 + 2NaOH → 2NaCl + Cu(OH)2↓(pale blue ppt-insoluble)

ZnSO4 + 2NaOH → 2Na2SO4 + Zn(OH)2↓(gelatinous white ppt-insoluble)

Zn(OH)2 + 2NaOH[excess] →2H2O + Na2ZnO2(colourless sol-soluble)

Pb(NO3)2 + 2NaOH → 2NaNO3 + Pb(OH)2↓(chalky white ppt-insoluble)

Pb(OH)2 + 2NaOH[excess] → 2H2O + Na2PbO2(colourless sol-soluble)

REACTIONS OF NH4OH SOLUTION ON SALTS

MgCl2 + 2NH4OH → 2NH4Cl + Mg(OH)2↓(dull white ppt-insoluble)

FeSO4 + 2NH4OH → (NH4)2SO4 + Fe(OH)2↓(dirty green ppt-insoluble)

FeCl3 + 2NH4OH → 3NH4Cl + Fe(OH)3↓(reddish brown ppt-insoluble)

CuSO4 + 2NH4OH → (NH4)2SO4 + Cu(OH)2↓(pale blue ppt-insoluble)

Cu(OH)2 + (NH4)2SO4 + 2NH4OH[excess] → 4H2O + [Cu(NH3)4]SO4(deep blue or inky

blue sol-soluble)

Cu(OH)2 + 4NH4OH[excess] → 4H2O + [Cu(NH3)4](OH)2(deep blue or inky blue sol-soluble)

ZnSO4 + 2NH4OH → (NH4)2SO4 + Zn(OH)2↓(gelatinous white ppt-insoluble)

Zn(OH)2 + (NH4)2SO4 + 2NH4OH[excess] →4H2O + [Zn(NH3)4]SO4(colourless sol-soluble)

Zn(OH)2 + 4NH4OH[excess] → 4H2O + [Zn(NH3)4](OH)2(colourless sol-soluble)

Pb(NO3)2 + 2NH4OH → 2NH4NO3 + Pb(OH)2↓(chalky white-insoluble)

ACTION OF ALKALIS ON CERTAIN METALS

Zn + 2NaOH → Na2ZnO2 + H2↑

Zn + 2KOH → K2ZnO2 + H2↑

Pb + 2NaOH → Na2PbO2 + H2↑

Pb + KOH → K2PbO2 + H2↑

2Al + 2NaOH + 2H2O → 2NaAlO2 + 3H2↑

2Al + 2KOH + 2H2O → 2KAlO2 + 3H2↑

ACTION OF ALKALIS ON OXIDES AND HYDROXIDES OF CERTAIN METALS

ZnO + 2NaOH → Na2ZnO2 + H2O

Zn(OH)2 + 2NaOH → Na2ZnO2 + 2H2O

PbO + 2NaOH → Na2PbO2 + H2O

Pb(OH)2 + 2NaOH → Na2PbO2 + 2H2O



Al2O3 + 2NaOH → 2NaAlO2 + H2O

Al(OH)3 + NaOH → NaAlO2 + 2H2O

Al2O3 + 2KOH → 2KAlO2 + H2O

Al(OH)3 + KOH → KAlO2 + 2H2O

ELECTROLYSIS STRONG ELECTROLYTES

HCl[aq] H1+ + Cl1-

HNO3[aq] H1+ + NO31-

H2SO4[aq] 2H1+ + SO42-

KOH[aq] K1+ + OH1-

NaOH[aq] Na1+ + OH1-

LiOH[aq] Li1+ + OH1-

PbBr2[molten] Pb2+ + 2Br1-

CuCl2[aq] Cu2+ + 2Cl1-

AgNO3[aq] Ag1+ + NO31-

WEAK ELECTROLYTES

CH3COOH[aq] CH3COO1- + H1+

HCOOH[aq] HCOO1- + H1+

H2CO3[aq] 2H1+ + CO32-

Ca(OH)2[aq] Ca2+ + 2OH1-

Mg(OH)2[aq] Mg2+ + 2OH1-

NH4OH[aq] NH41+ + OH1-

Na2CO3[aq] 2Na1+ + CO32-

KHCO3 [aq] K1+ + HCO31-

(CH3COO)2Pb[aq] 2CH3COO1- + Pb2+

ELECTROLYSIS OF MOLTEN PbBr2

Electrolytic cell : Silica crucible

Electrolyte : Molten PbBr2

Electrodes : Graphite(inert)

Temperature : >380⁰C

Current : 3 amps

Dissociation : PbBr2 Pb2+ +2Br1-

Reaction at cathode : Pb2+ +2e- → Pb (silvery grey deposit)

Reaction at anode : Br1- - 1e- → Br

Br + Br → Br2 (reddish brown fumes)

ELECTROLYSIS OF ACIDIFIED WATER

Electrolyte : Acidified water with dil H2SO4

Electrodes : Platinum foil(inert)

Temperature : Ordinary temp



Current : 3 amps

Dissociation : H2SO4 2H1+ + SO42-

H2O H1+ + OH1-

Reaction at cathode : H1+ +1e- → H x 4

2H + 2H → 2H2 (hydrogen gas evolved)

Reaction at anode : OH1- -1e- → OH x 4

4OH → 2H2O + O2 (oxygen gas evolved)

ELECTROLYSIS OF Aq.CuSO4 (USING ACTIVE ELECTRODES)

Electrolyte : aq. CuSO4

Electrodes : Copper(active)


Current : 3 amps

Dissociation : CuSO4 Cu2+ + SO42-

H2O H1+ + OH1-

Reaction at cathode : Cu2+ + 2e- → Cu (brownish pink deposit)

Reaction at anode : Cu - 2e- → Cu2+ (no product-Cu2+ ions formed)

ELECTROLYSIS OF Aq.CuSO4 (USING INERT ELECTRODES)

Electrolyte : aq. CuSO4

Electrodes : Platinum or carbon(inert)


Current : 3 amps


H2O H1+ + OH1-

Reaction at cathode : Cu2+ + 2e- → Cu (brownish pink deposit)

Reaction at anode : OH1- - 1e- → OH x 2

4OH → 2H2O + O2 (oxygen gas evolved)

Note: With active electrode anode diminishes in mass because it loses electrons.

Blue colour of CuSO4 remains unchanged with copper electrode but fades with inert

electrode because if copper anode is used, for every copper ion discharged at cathode a

copper ion is added to the sol. by the anode. Total no. of copper ions remains same. This is

not the case with inert electrodes.

ELECTROPLATING WITH NICKEL

Electrolyte : aq. NiSO4

Cathode : Article to be electroplated

Anode : Block of nickel metal

Dissociation : NiSO4 Ni2+ +SO42-

H2O H1+ +OH1-

Reaction at cathode : Ni2+ +2e- → Ni (deposited)

Reaction at anode : Ni – 2e- → Ni2+ (no product-Ni2+ ions formed)

ELECTROPLATING WITH SILVER



Electrolyte : aq. Na[Ag(CN)2] (sodium silver cyanide)

Cathode : Cleaned article to be electroplated

Anode : Block of silver metal

Dissociation : Na[Ag(CN)2] Na1+ + Ag1+ + 2CN1-

H2O H1+ +OH1-

Reaction at cathode : Ag1+ +1e- → Ag (deposited)

Reaction at anode : Ag – 1e- → Ag1+ (no product-Ag1+ ions formed)

ELECTROREFINING OF COPPER

Electrolyte : Aq. CuSO4

Cathode : Pure thin sheet of copper

Anode : Impure block of copper


H2O H1+ +OH1-

Reaction at cathode : Cu2+ + 2e- → Cu (deposited)

Reaction ay anode : Cu - 2e- → Cu2+ (no product-Cu2+ ions formed)

METALLURGY CONCENTRATED ORE TO OXIDE

ROASTING

2ZnS + 3O2 → 2ZnO + 2SO2↑

4FeS + 7O2 → 2Fe2O3 + 4SO2↑

CALCINATION

ZnCO3 → ZnO + CO2↑

FeCO3 → FeO + CO2↑

REDUCTION OF METALLIC OXIDES

BY ELECTROLYSIS

Al2O3 2Al3+ + 3O2-

At cathode : 2Al3+ + 6e- → 2Al

At anode : 3O2- - 6e- → 3[O] → 3O2↑

BY REDUCING AGENTS

ZnO + C Zn + CO↑

2PbO + C 2Pb + CO2↑

Fe2O3 + 3CO 2Fe + 3CO2↑

FeO + CO Fe + CO2↑

BY THERMAL DECOMPOSITION



2HgO 2Hg + O2↑

2Ag2O 4Ag + O2↑

METALLURGY OF ZINC

Roasting : 2ZnS + 3O2 2ZnO + 2SO2↑

Calcination : ZnCO3 2ZnO + CO2↑

Reduction : ZnO + C Zn + CO↑

METALLURGY OF IRON

Lower region : C + O2 → CO2 + Δ

Middle region : CO2 + C → 2CO – Δ

CaCO3 → CaO + CO2↑

CaO + SiO2 → CaSiO3 [slag]

Upper region : Fe2O3 + 3CO → 2Fe + 3CO2↑

METALLURGY OF ALUMINIUM

CONCENTRATION OF ORE – BAEYER’S PROCESS

Al2O3 . 2H2O 2NaAlO2 + 3H2O

NaAlO2 + 2H2O NaOH + Al(OH)3↓

2Al(OH)3 Al2O3 + 3H2O[vap]

ELECTROLYTIC REDUCTION OF ALUMINA – HALL HEROULT’S PROCESS

Electrolyte : Fused alumina-1part, cryolite-3 parts, fluorspar-1 part

Electrolytic cell : Rectangular steel tank with carbon lining

Cathode : Gas carbon

Anode : Thick carbon rods (graphite) attached to copper clamps

Temperature : 950⁰C

Current : 100 amps

Dissociation : Na3AlF6 3Na1+ + Al3+ + 6F1-

CaF2 Ca2+ + 2F1-

Al2O3 2Al3+ + 3O2-

At cathode : 2Al3+ + 6e- → 2Al(pure metal deposited)

At anode : 3O2- - 6e- → 3[O] →3O2(oxygen gas evolved)

Thermite welding : Fe2O3 + 2Al → Al2O3 + 2Fe + Δ

RUSTING: 4Fe + 3O2 + xH2O → 2Fe2O3 . xH2O

STUDY OF COMPOUNDS: HCl PREPARATION

BY SYNTHESIS: H2 + Cl2 2HCl↑

IN LABORATORY: NaCl + H2SO4 [conc] NaHSO4 + HCl↑



CaO + 2HCl → CaCl2 + H2O

2P2O5 + 3HCl → POCl3 + 3HPO3

ACIDIC PROPERTY

Mg + 2HCl → MgCl2 + H2↑

Zn + 2HCl → ZnCl2 + H2↑

Fe + 2HCl → FeCl2 + H2↑

CuO + 2HCl →CuCl2 + H2O

NH4OH + HCl → NH4Cl + H2O

Na2CO3 + HCl → NaCl + H2O + CO2↑

Ca(HCO3)2 + 2HCl → CaCl2 + 2H2O + 2CO2↑

Na2SO3 + 2HCl → 2NaCl + H2O + SO2↑

NaHSO3 + HCl → NaCl + H2O + SO2↑

Na2S + 2HCl → NaCl + H2S↑

FeS + 2HCl → FeCl2 + H2S↑

CuS + 2HCl → CuCl2 + H2S↑

AgNO3 + HCl → AgCl↓ + HNO3

Pb(NO3)2 + 2HCl → PbCl2↓ + 2HNO3

Na2S2O3 + 2HCl → 2NaCl + SO2 + S + H2O

REACTIONS WITH OXIDISING AGENTS

MnO2 + 4HCl MnCl2 + 2H2O + Cl2

PbO2 + 4HCl PbCl2 + 2H2O + Cl2

Pb3O4 + 8HCl 3PbCl2 + 4H2O + Cl2

2KMnO4 + 16HCl 2KCl + 2MnCl2 + 8H2O + 5Cl2

K2Cr2O7 + 14HCl 2KCl + 2CrCl3 + 7H2O + 3Cl2

AQUA REGIA REACTION

HNO3 + 3HCl → NOCl + 2H2O + 2[Cl]

Au + 3[Cl] →AuCl3

Pt + 4[Cl] → PtCl4

STUDY OF COMPOUNDS: AMMONIA PREPARATION

FROM AMMONIUM SALTS

(NH4)2SO4 + 2NaOH Na2SO4 + 2H2O + 2NH3↑

(NH4)2SO4 + Ca(OH)2 CaSO4 + 2H2O + 2NH3↑

NH4Cl + NaOH NaCl + H2O + NH3↑

IN LAB: 2NH4Cl + Ca(OH)2 CaCl2 + 2H2O + 2NH3↑



2NH3 + H2SO4[conc.] → (NH4)2SO4

6NH3 + P2O5 + 3H2O → 2(NH4)3PO4

8NH3 + CaCl2 [fused] → CaCl2 . 8NH3

FROM METAL NITRIDES

3Mg + N2 → Mg3N2

Mg3N2 + 6H2O[warm] → 3Mg(OH)2 + 2NH3↑

3Ca + N2 → Ca3N2

Ca3N2 + 6H2O[warm] → 3Ca(OH)2 + 2NH3↑

2Al + N2 → 2AlN

AlN + 3H2O[warm] →Al(OH)3 + NH3↑

HABER’S PROCESS

Temperature : 450-500⁰C

Pressure : 200-900 atms

If catalyst finely divided Fe then promotor Mo

If catalyst Fe2O3 then promotor 1% K2O and 3% Al2O3

Impurities : CO, CO2, H2S

PREPARATION OF AMMONIUM SALTS

NH3 + HCl → NH4Cl

NH3 + HNO3 →NH4NO3

2NH3 + H2SO4 → (NH4)2SO4

NH4OH + HCl → NH4Cl + H2O

NH4OH + HNO3 → NH4NO3 + H2O

2NH4OH + H2SO4 → (NH4)2SO4 + 2H2O

COMBUSTION: 4NH3 + 3O2 → 2N2 + 6H2O

CATALYTIC OXIDATION: 4NH3 + 5O2 4NO + 6H2O + Δ

2NO + O2 → 2NO2

BASIC NATURE

NH3 + H2O → NH4OH

NH4OH NH4+ + OH-

FeSO4 + 2NH4OH → (NH4)2SO4 + Fe(OH)2↓(dirty green ppt-insoluble)

FeCl3 + 2NH4OH → 3NH4Cl + Fe(OH)3↓(reddish brown ppt-insoluble)

CuSO4 + 2NH4OH → (NH4)2SO4 + Cu(OH)2↓(pale blue ppt-insoluble)

Cu(OH)2 + (NH4)2SO4 + 2NH4OH[excess] → 4H2O + [Cu(NH3)4]SO4(deep blue or inky

blue sol-soluble)

Cu(OH)2 + 4NH4OH[excess] → 4H2O + [Cu(NH3)4](OH)2(deep blue or inky blue sol-soluble)

ZnSO4 + 2NH4OH → (NH4)2SO4 + Zn(OH)2↓(gelatinous white ppt-insoluble)

Zn(OH)2 + (NH4)2SO4 + 2NH4OH[excess] →4H2O + [Zn(NH3)4]SO4(colourless sol-soluble)

Zn(OH)2 + 4NH4OH[excess] → 4H2O + [Zn(NH3)4](OH)2(colourless sol-soluble)



REDUCING NATURE

2NH3 + 3CuO →Cu + 3H2O + N2↑

2NH3 + 3PbO → 3Pb + 3H2O + N2↑

8NH3[excess] + 3Cl2 → 6NH4Cl + N2

NH3 + 3Cl2[excess] → 3HCl + NCl3

STUDY OF COMPOUNDS: NITRIC ACID PREPARATION

IN LAB

KNO3 + H2SO4[conc.] KHSO4 + HNO3[vap]

NaNO3 + H2SO4[conc.] NaHSO4 + HNO3[vap]

DECOMPOSITION OF HNO3: 4HNO3 → 4NO2 + 2H2O + O2

OXIDISING NATURE

2HNO3[conc.] → H2O + 2NO2 + [O]

Cu + [O] → CuO

CuO + 2HNO3 → Cu(NO3)2 + H2O

Cu + 4HNO3 → Cu(NO3)2 + 2H2O + NO2

Cu + 4HNO3[conc.] → Cu(NO3)2 + 2H2O + 2NO2

C + 4HNO3[conc.] → CO2 + 2H2O + 4NO2

S + 6HNO3[conc.] → H2SO4 + 2H2O + 6NO2

3Cu + 8HNO3[dil.] → 3Cu(NO3)2 + 4H2O + 2NO

Cu + 4HNO3[conc.] → Cu(NO3)2 +2H2O +2NO2

C7H8 + 3HNO3[conc.] → C7H5(NO2)3 + 3H2O

BROWN RING TEST

6FeSO4 + 3H2SO4[conc.] + 2HNO3[dil.] → 3Fe2(SO4)3 + 4H2O + 2NO

FeSO4 + NO → FeSO4 . NO

STUDY OF COMPOUNDS: SULPHURIC ACID PREPARATION

CONTACT PROCESS

SULPHUR OR PYRITE BURNERS

S + O2 → SO2

2FeS + 3O2 → 2FeO + 2SO2

CONTACT TOWER

2SO2 + O2 2SO3 + Δ

ABSORPTION TOWER

SO3 + H2SO4 → H2S2O7



DILUTION TANK

H2S2O7 + H2O → 2H2SO4

ACIDIC NATURE

H2SO4 + 2H2O 2H3O+ + SO42-

REACTIONS OF DIL. H2SO4

Zn + H2SO4 → ZnSO4 + H2↑

Fe + H2SO4 → FeSO4 + H2↑

Na2O + H2SO4 → Na2SO4 + H2O

MgO + H2SO4 → MgSO4 + H2O

ZnO + H2SO4 → ZnSO4 + H2O

CuO + H2SO4 → CuSO4 +H2O

2NaOH + H2SO4→ Na2SO4 + 2H2O

Zn(OH)2 + H2SO4 → ZnSO4 + 2H2O

Na2CO3 + H2SO4 → Na2SO4 + H2O + CO2↑

CuCO3 + H2SO4 → CuSO4 + H2O + CO2↑

2KHCO3 + H2SO4 → K2SO4 + 2H2O + 2CO2↑

Na2SO3 + H2SO4 → Na2SO4 + H2O + SO2↑

2NaHSO3 + H2SO4 → Na2SO4 + 2H2O + 2SO2↑

Na2S + H2SO4 → Na2SO4 + H2S↑

ZnS + H2SO4 → ZnSO4 + H2S↑

FeS + H2SO4 → FeSO4 + H2S↑

DIBASIC ACID

DISSSOCIATES IN TWO STEPS

H2SO4 H+ + HSO4-

HSO4- H+ + SO42-

H2SO4 2H+ + SO42-

FORMS TWO TYPES OF SALTS

NaOH + H2SO4 → NaHSO4[acid salt] + H2O

2NaOH[excess] + H2SO4 → Na2SO4[normal salt] + 2H2O

NON VOLATILE ACID


KCl + H2SO4[conc.] KHSO4 + HCl

NaNO3 + H2SO4[conc.] NaHSO4 + HNO3

KNO3 + H2SO4[conc.] KHSO4 + HNO3

OXIDISING AGENT

H2SO4 → H2O + SO2 + [O]

Cu + [O] → CuO



CuO + H2SO4 → CuSO4 + H2O

Cu + 2H2SO4 → CuSO4 + 2H2O + SO2↑

C + 2H2SO4[conc.] → CO2 + 2H2O + 2SO2↑

S + 2H2SO4[conc.] → 3SO2↑ + 2H2O

2P + 5H2SO4[conc.] → 2H3PO4 + 2H2O + 5SO2↑

Cu + 2H2SO4[conc.] → CuSO4 + 2H2O + SO2↑

Zn + 2H2SO4[conc.] → ZnSO4 + 2H2O + SO2↑

STRONG DEHYDRATING AGENT

C6H12O6 6C + 6H2O

C12H22O11 12C + 11H2O

[C6H10O5]n 6[C]n + 5[H2O]n

CuSO4 . 5H2O CuSO4 + 5H2O

ORGANIC CHEMISTRY

ALKANES PREPARATION

IN LAB

CH3COONa + NaOH CH4 + Na2CO3

C2H5COONa + NaOH C2H6 + Na2CO3

GENERAL METHOD – FROM ALKYL HALIDES

CH3I + 2[H] CH4 + HI

C2H5Br + 2[H] C2H6 + HBr

2CH3I + 2Na C2H6 + 2NaI

SUBSTITUTION REACTION

CH4 + Cl2 CH3Cl + HCl

CH3Cl + Cl2[excess] →CH2Cl2 + HCl

CH2Cl2 + Cl2 → CHCl3 + HCl

CHCl3 + Cl2 → CCl4 + HCl

C2H6 + Cl2 C2H5Cl + HCl

C2H5Cl + Cl2[excess] →C2H4Cl2 + HCl

C2H4Cl2 + Cl2 →C2H3Cl3 + HCl

C2H3Cl3 + Cl2 → C2H2Cl4 + HCl

C2H2Cl4 + Cl2 → C2HCl5 + HCl

C2HCl5 + Cl2 → CCl6 + HCl

OXIDATION

COMPLETE

CH4 + 2O2[excess] → CO2 + 2H2O + Δ

2C2H6 + 7O2[excess] → 4CO2 + 6H2O + Δ



INCOMPLETE

2CH4 + 3O2[limited] → 2CO + 4H2O + Δ

2C2H6 + 5O2[limited] → 4CO + 6H2O +Δ

2C2H6 + 3O2[very limited] →4C + 6H2O

ALKENES PREPARATION

IN LAB

BY DEHYDRATION OF C2H5OH

C2H5OH C2H4 + H2O

BY DEHYDROHALOGENATION OF C2H5Br

C2H5Br + KOH[alcoholic] C2H4 + KBr + H2O

GENERAL METHOD BY CRACKING

C2H6 C2H4 + H2

ADDITION REACTIONS

HALOGENATION

C2H4 + Cl2 C2H4Cl2

C2H2 + Br2 C2H4Br2

C2H4 + I2 C2H4I2

OXIDATION

With cold dil. KMnO4 sol-Baeyer’s Reagent

C2H4 + H2O + [O] → C2H4(OH)2

Combustion

C2H4 + 3O2 → 2CO2 + 2H2O + Δ

ALKYNES PREPARATION

IN LAB

CaC2 + 2H2O → C2H2 + Ca(OH)2

C2H4Br2 + 2KOH[alcoholic] C2H2 + 2KBr + 2H2O

GENERAL METHOD

FROM METHANE

2CH4 C2H2 + 3H2

ADDITION REACTIONS

CATALYTIC HYDROGENATION

C2H2 + H2 C2H4 + H2 C2H6

HALOGENATION

C2H2 + Cl2 C2H2Cl2 + Cl2 C2H2Cl4

C2H2 + Br2 C2H2Br2 + Br2 C2H2Br4

C2H2 + I2 C2H2I2



OXIDATION

With dil. Alkaline KMnO4

C2H2 + 4[O] → OH-COOH

Combustion

2C2H2 + 5O2 → 4CO2 + 2H2O + Δ

AMMONIACAL SILVER NITRATE

C2H2 + 2AgNO3 + 2NH4OH → Ag-C≡C-Ag + 2NH4NO3 + 2H2O

ALCOHOLS PREPARATION

IN LAB

C2H5Cl + NaOH[aq] C2H5OH + NaCl

C2H5Br + KOH[aq] C2H5OH + KBr

INDUSTRIAL METHOD

C2H4 + H2SO4 C2H5-HSO4

C2H5-HSO4 + H2O → C2H5OH + H2SO4

COMBUSTION

C2H5OH + 3O2 → 2CO2 + 3H2O

OXIDATION

C2H5OH CH3CHO CH3COOH

SODIUM

2C2H5OH + 2Na → 2C2H5ONa + H2

ACETIC ACID C2H5OH + CH3COOH CH3COO-C2H5 + H2O

SULPHURIC ACID

C2H5OH C2H4 + H2O

2C2H5OH[excess] C2H5-O-C2H5 + H2O

3C2H5OH +PCl3 → 3C2H5Cl + H3PO3

CARBOXYLIC ACIDS PREPARATION

C2H5OH + [O] CH3CHO + H2O

CH3CHO + [O] CH3COOH

ACIDIC NATURE

CH3COOH + NaOH → CH3COONa + H2O



2CH3COOH + Ca(OH)2 → (CH3COO)2Ca + 2H2O

CH3COOH + NH4OH → CH3COONH4 + H2O

ALCOHOLS

C2H5OH + CH3COOH CH3COO-C2H5 + H2O

Education

Chemistry equations for ICSE Class 10