Daily use Chemical Compounds and Their Properties
Chemical Compound – Salammoniac
Sal Ammoniac
Ammonium Chloride : NH4Cl
Ammonium Chloride is a chemical compound which found in abundance in nature. Ammonium chloride is obtained when ammonia gas is passed through hydrochloric acid (HCl).
NH3 + HCl → NH4Cl
Ammonium Chloride Properties
Properties: Its main physical and chemical properties are as follows –
Physical properties :
Ammonium Chloride is a white colored crystal solid.
It is soluble in water. Heat is absorbed when soluble in water. Hence its solution remains cold.
Chemical properties
Heat effect : On heating, it decomposes into ammonia and hydrogen chloride without melting. On cooling, Salammoniac is obtained again.
NH4Cl ⇌ NH3 + HCl
Reaction with slaked lime : On heating ammonia chloride with dry slaked lime [Ca(OH)2], ammonia gas is evolved.
2NH4Cl + Ca(OH)2 → CaCl2 + 2H2O + 2NH3
Reaction with slaked lime : On heating ammonia chloride with dry slaked lime [Ca(OH)2], ammonia gas is evolved.
2NH4Cl + PbO → PbCl2 + H2O + 2NH3
Reaction with NaOH : On heating salmoniac with caustic soda, ammonia gas is evolved.
NH4Cl + NaOH → NaCl + H2O + 2NH3
Ammonium Chloride Uses
- As reagent in laboratory.
- In the manufacture of dry cells, for wiping utensils and in soldering.
- In the manufacture of fertilizers and ammonia etc.
- For dyeing and calico printing.
- as medicine.
Chemical Compound – Quick Lime
Quick Lime – Calcium oxide – CaO
On heating quick lime stone (CaCO3), calcium oxide is obtained.
CaCO3 → CaO + CO2
Calcium Oxide Properties
Physical properties :
Quick lime is a white colored amorphous solid.
It does not melt on heating in oxy hydrogen flame because it burns with intense light, which is called Limelight.
Its melting point is 2570°C.
chemical properties
When left open in air: – When lime is left open in air, it absorbs moisture and carbon dioxide from the air to form calcium hydroxide [Ca(OH)2] and then calcium carbonate(CaCO3).
CaO + H2O → Ca(OH)2
Ca(OH)2 + CO2 → CaCO3 + H2O
Reaction with water : When quick lime is added to water, there is a bubbling sound and calcium hydroxide is formed. Also 15,540 calories of heat is liberated.
CaO + H2O → Ca(OH)2 + 15540 cal
Quenched lime reacts with chlorine to form bleaching powder.
Reaction with carbon : It reacts with carbon at high temperature in an electric furnace to form calcium carbide (CaC2).
CaO + 3C → CaC2 + CO
Reaction with chlorine : Reaction with chlorine in the chosen red hot state forms calcium chloride and oxygen is liberated.
2CaO + 2Cl2 → 2CaCl2 + O2
Reaction with ammonium chloride : On reaction with ammonium chloride, ammonia gas is obtained.
CaO + 2NH4Cl → 2CaCl2 + H2O + 2NH3
Reaction with acids: Being alkaline in nature, it reacts with acids to form salts.
CaO + 2HCl → CaCl2 + H2O
CaO + H2SO4 → CaSO4 + H2O
Calcium Oxide Uses
- As reagent in laboratory.
- In the manufacture of ammonia.
- In industrial manufacture of bleaching powder, calcium carbide, basic calcium nitrate, cement and lead.
- As flux in metallurgy.
- It is used for purification of coal gas, softening of water, tanning industry, bactericidal and disinfectant.
- In petromax for mental making, in the lining of furnaces and in absorbing moisture.
- In the manufacture of sodalime reagent.
Chemical Compound – Cupric Sulfate
In this compound, ionic, covalent and subcovalent bonds are present, hence its structure is as follows –
Preparation method : On heating copper with concentrated H2SO4 –
On crystallization of the obtained solution, crystals of CuSO4.5H2O are obtained.
Cu + 2H2SO4 → CuSO4 + 2H2O + SO2
On heating copper with dilute H2SO4 in the presence of air –
On crystallization of the obtained solution, crystals of CuSO4.5H2O are obtained.
Cu + H2SO4 + ½ O2 → CuSO4 + H2O
On heating copper oxide, hydrooxide or carbonate with dilute H2SO4 –
CuO + H2SO4 → CuSO4 + H2O
Cu(OH)2 + H2SO4 → CuSO4 + 2H2O
CuCO3 + H2SO4 → CuSO4 + H2O + CO2
On heating copper oxide, hydrooxide or carbonate with dilute H2SO4 –
CuFeS2 + 4O2 → CuSO4 + FeSO4
Cupric Sulfate Properties
Physical properties:
It is a blue colored crystal solid material. It crystallizes in triclinic lattice. It is soluble in water, but gets decomposed quickly. Therefore, its aqueous solution is formed in the presence of glycial acetic acid.
It is insoluble in alcohol. Its aqueous solution exhibits acidic property. It is also a strong poison. It is a colorless and brittle substance with astringent taste.
Chemical properties:
Heat effect: On heating it at about 100°C, 4 molecules of water get separated from it. Thereafter, at 230°C it gives anhydrous CuSO4 which is a white solid.
CuSO4.5H2O → CuSO4.H2O → CuSO4
This anhydrous CuSO4 is used in the test of water, because it reacts with water to turn blue colored CuSO4.5H2O.
CuSO4 + 5H2O → CuSO4.5H2O
It decomposes on heating anhydrous CuSO4 at a high temperature(>720°C).
Reaction with Potassium iodide: It first reacts with aqueous solution to give temporary CuI2 which on decomposition gives a white precipitate of cuprus iodide.
2CuSO4 → 2CuS + 2SO2 + O2
Reaction with ammonium hydroxide solution : In this, a greenish blue precipitate of Cu(OH)2 is obtained by the first reaction which dissolves in excess of NH4OH to form a hybrid salt of cupromonium sulfate.
CuSO4 + 2NH4OH → Cu(OH)2 + (NH4)2SO4
Cu(OH)2 + (NH4)2SO4 + 2NH4OH → [Cu(NH3)4SO4] + 4H2O
Reaction with potassium cynide solution : In this reaction, first a temporary compound Cu(CN)2 is formed which decomposes into a white precipitate of CuCN and in excess of KCN forms a hybrid salt of potassium cuprocyanide.
CuSO4 + 2KCN → Cu(CN)2 + K2SO4
2Cu(CN)2 → CuCN + CN-CN
CuCN + 3KCN → K3[Cu(CN)4]
Reaction with Potassium thiocyanate solution(KCNS) :
CuSO4 + 2KCNS → Cu(CNS)2 + K2SO4
Reaction with Potassium ferrocyanide solution[K4(Fe(CN)6)] : A reddish brown precipitate of cupric ferocynide is formed.
2CuSO4 + [K4(Fe(CN)6)] → Cu2[F2(CN)6] + 2K2SO4
Reaction with NaOH solution : A dark yellow precipitate of Cu(OH)2 is obtained.
CuSO4 + 2NaOH → Cu(OH)2 + Na2SO4
Reaction with iron shavings : Copper gets displaced.
CuSO4(l) + Fe(s) → FeSO4(l) + Cu(s)
Reaction with hydrogen sulfide gas : A black precipitate of CuS is obtained by reaction with H2S gas.
CuSO4 + H2S →
CuS + H2SO4
In aqueous solution it gives the test of sulfate radicals.
CuSO4 + BaCl2 → BaSO4 + CuCl2
Cupric Sulfate Uses
A mixture of CuSO4 and CaO (Bordeaux mixture) is used as a fungicide.
In the formulation of fahling and benedict solutions.
In determining the presence of water.
in the manufacture of medicines.
In the making of Mordant.
In the dye industry and calico printing.