Home | | Chemistry 11th std | Important compounds of calcium

Chapter: 11th Chemistry : Alkali and Alkaline Earth Metals

Preparation, Properties, Uses, Formula | Chemistry | Study Material, Lecturing Notes, Assignment, Reference, Wiki description explanation, brief detail |

Important compounds of calcium

Chemistry : Alkali and Alkaline Earth Metals

Important compounds of calcium

 

Quick lime, CaO

 

Preparation

It is produced on a commercial scale by heating limestone in a lime kiln in the temperature range 1070-1270K.

 

CaCO3  CaO + CO2

 

The reaction being reversible, carbon dioxide is removed as soon as it is produced to enable the reaction to proceed to completion.

 

Properties

 

Calcium oxide is a white amorphous solid.

It has a melting point of 2870 K.

It absorbs moisture and carbon dioxide on exposure to atmosphere.

 

CaO + H2O  → Ca(OH)2

CaO + CO2  → CaCO3

 

The addition of limited amount of water breaks the lump of lime. This process is called slaking of lime and the product is slaked lime.

 

CaO + H2O  → Ca(OH)2

 

Quick lime mixed with soda gives solid soda lime. It combines with acidic oxides such as SiO2 and P4O10 to form CaSiO3 and Ca3(PO4)2, respectively.


CaO + SiO2  → CaSiO3

6CaO + P4O10  → 2Ca3(PO4)2

 

Uses

 

Calcium oxide is used

i.              to manufacture cement, mortar and glass.

ii.               in the manufacture of sodium carbonate and slaked lime.

iii.               in the purification of sugar.

iv.               as a drying agent.


Calcium hydroxide

 

Preparation

 

Calcium hydroxide is prepared by adding water to quick lime, CaO.

 

Properties

 

It is a white powder. It is sparingly soluble in water. The aqueous solution is known as lime water and a suspension of slaked lime in water is known as milk of lime.

 

When carbon dioxide is passed through lime water, it turns milky due to the formation of calcium carbonate.

 

Ca(OH)2 + CO2  → CaCO3 + H2O

 

On passing excess of carbon dioxide, the precipitate dissolves to form calcium hydrogen carbonate.

 

CaCO3 + CO2 + H2O  → Ca(HCO3)2

 

Milk of lime reacts with chlorine to form hypochlorite, a constituent of bleaching powder.

 

2Ca (OH)2 + 2Cl2  → CaCl2 + Ca(OCl)2 + 2H2O

 

Uses:

 

Calcium hydroxide is used

 

i.               in the preparation of mortar, a building material.

ii.               in white wash due to its disinfectant nature.

iii.               in glass making, in tanning industry, in the preparation of bleaching powder and for the purification of sugar.

 

Gypsum (CaSO4.2H2O)

 

Gypsum beds were formed due to the evaporation of water from the massive prehistoric sea basins. When water evaporates, the minerals present in it become concentrated, and crystallise.


 

Properties of Gypsum

 

·           Gypsum is a soft mineral, which is moderately soluble in water. The solubility of this mineral in water is affected by temperature. Unlike other salts, gypsum becomes less soluble in water as the temperature increases. This is known as retrograde solubility, which is a distinguishing characteristic of gypsum.

 

·           Gypsum is usually white, colorless, or gray in color. But sometimes, it can also be found in the shades of pink, yellow, brown, and light green, mainly due to the presence of impurities.

 

·           Gypsum crystals are sometimes found to occur in a form that resembles the petals of a flower. This type of formation is referred to as ‘desert rose’, as they mostly occur in arid areas or desert terrains.

 

·           Gypsum is known to have low thermal conductivity, which is the reason why it is used in making drywalls or wallboards. Gypsum is also known as a natural insulator.


 

·           Alabaster is a variety of gypsum, that is highly valued as an ornamental stone. It has been used by the sculptors for centuries. Alabaster is granular and opaque.

 

·           Gypsum has hardness between 1.5 to 2 on Moh’s Hardness Scale. Its specific gravity is 2.3 to 2.4.

 

Uses of Gypsum

 

·           The alabaster variety of gypsum was used in ancient Egypt and Mesopotamia by the sculptors. The ancient Egyptians knew how to turn gypsum into plaster of Paris about 5,000 years ago. Today, gypsum has found a wide range of uses and applications in human society, some of which are enlisted below.

 

·           Gypsum is used in making drywalls or plaster boards. Plaster boards are used as the finish for walls and ceilings, and for partitions.

 

·           Another important use of gypsum is the production of plaster of Paris. Gypsum is heated to about 300 degree Fahrenheit to produce plaster of Paris, which is also known as gypsum plaster. It is mainly used as a sculpting material.

 

·           Gypsum is used in making surgical and orthopedic casts, such as surgical splints and casting moulds.

 

·           Gypsum plays an important role in agriculture as a soil additive, conditioner, and fertilizer. It helps loosen up compact or clay soil, and provides calcium and sulphur, which are essential for the healthy growth of a plant. It can also be used for removing sodium from soils having excess salinity.

 

·           Gypsum is used in toothpastes, shampoos, and hair products, mainly due to its binding and thickening properties.

 

·           Gypsum is a component of Portland cement, where it acts as a hardening retarder to control the speed at which concrete sets.

 

·           To sum up, gypsum is one of the most abundant minerals that have endless uses and applications. Mining of gypsum is simple and easy, as the mineral occurs in large thick beds near the Earth’s surface. However, large-scale mining of gypsum involves considerable damage to the environment. Gypsum can also be recycled, but not much importance has been given to recycle this mineral due to its abundance.


 


Plaster of paris

Calcium Sulphate (Plaster of Paris), CaSO4·½ H2O


It is a hemihydrate of calcium sulphate. It is obtained when gypsum, CaSO4·2H2O, is heated to 393 K.

 

2CaSO4 .2H2O(s)  →2CaSO4 .H2O+ 3H2O

 

Above 393 K, no water of crystallisation is left and anhydrous calcium sulphate, CaSO4 is formed. This is known as ‘dead burnt plaster’.

It has a remarkable property of setting with water. On mixing with an adequate quantity of water it forms a plastic mass that gets into a hard solid in 5 to 15 minutes.

 

Uses:

 

The largest use of Plaster of Paris is in the building industry as well as plasters. It is used for immobilising the affected part of organ where there is a bone fracture or sprain. It is also employed in dentistry, in ornamental work and for making casts of statues and busts.


 

Tags : Preparation, Properties, Uses, Formula | Chemistry Preparation, Properties, Uses, Formula | Chemistry
Study Material, Lecturing Notes, Assignment, Reference, Wiki description explanation, brief detail


Copyright © 2018-2020 BrainKart.com; All Rights Reserved. Developed by Therithal info, Chennai.