Question

how is the temporary hardness of water removed by boiling method explain in brief​

Answer 1

Answer:

Hi mate

Temporary hardness

The presence of magnesium and calcium carbonates in water makes it temporarily hard.

Method to remove temporary Hardness

Temporary Hardness can be removed by boiling the water.When we boil water the soluble salts of Mg(HCO3)2 is converted to Mg(OH)2 which is insoluble and hence gets precipitated and is removed. After filtration, the water we get is soft water.

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Answer 2

Answer:

Temporary hardness is due to the presence of calcium hydrogencarbonate Ca(HCO3)2(aq) and magnesium hydrogencarbonate Mg(HCO3)2(aq).Both calcium hydrogencarbonate and magnesium hydrogencarbonate decompose when heated. The original insoluble carbonate is reformed. This happens when water is boiled. 

Step-by-step explanation:

Temporary hardness consists of the bicarbonates of calcium and magnesium. Heating water to 100 C decomposes the soluble bicarbonates to the carbonates, according to:Ca(HCO3)2 = CO2 + H2O + CaCO3,and similarly for Mg(HCO3)2. Both MgCO3 and CaCO3 are insoluble and precipitate out when the water is boiled.The bicarbonates are the compounds present in hard water and constitute the temporary hardness. If the water is either filtered or allowed to stand to ensure sedimentation of the insoluble carbonates then the drained water has a lower total hardness. What remains is the permanent hardness made up, predominantly, of calcium and magnesium chlorides and sulphates.If you boil water in one of those transparent kettles - or in a laboratory beaker - you will note that, for hard water, precipitation as the carbonates only occurs while the water is boiling: below the boiling point there is no obvious manifestation of precipitation which is just as well as, otherwise, our plumbing would become furred up in no time at all!You might also note hardness deposits on the visible side of a shower head. What happens there is that, unlike Mg(HCO3)2 which is soluble and easily removed with water, there is no Ca(HCO3)2 encrusted around the minute holes of the shower head caused by evaporation of residual water from the head. What you see is CaCO3 deposits: a solid form of Ca(HCO3)2 is too unstable to exist and breaks down to the insoluble carbonate that is readily removed with dilute acid (eg, citric or acetic acids available from lemon and vinegar, respectively).

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