Question

50 liter of water containing Ca(HCO3)2 when converted into soft water required 22.2g of Ca(OH)2 . Calcultated the amount of Ca(bHCO3)2 per liter of hand water.​

Answer 1

0.3 moles of Ca(HCO3)2

ie. 47g

And per litre will be 47/50

So... 0.94g approx..

Please do it yourself

It's your exam question, don't look on internet.

Answer 2

Answer:

0.972 gram/litre

Explanation:

Let us first write the chemical equation for better understanding;

Ca(HCO3)2 + Ca(OH)2 == 2CaCO3 + 2H2O

Here we can see that one mole of each reactant is required to product 2 moles of each product produced.

Molar mass of Ca(HCO3)2 is 162 and molar mass of Ca(OH)2 is 74

Number of mole in 22.2 gram of Ca(OH)2 = 22.2 / 74 = 0.3

Hence we will require 0.3 moles of  Ca(HCO3)2

Weight of 0.3 moles of Ca(HCO3)2 = 0.3 x 162 = 48.6 grams

So gram per litre of Ca(HCO3)2 = 48.6 / 50 = 0.972 gram/litre

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