Question

A water sample using FeSO4.7H2O as a coagulant at the rate of 278 ppm, gave the following data on analysis of raw water: Ca+2 = 240 ppm, Mg+2 = 96 ppm CO2 = 44 ppm and HCO3– = 732 ppm. Calculate the lime and soda required to soften 2,50,000 litres of water.
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Answer 1

Answer:

a water sample using feso4.7h2o as a coagulant at the rate of 139 ppm gave the following result on analysis : ca 2+= 160ppm,co3 2- =88ppm,mg2+=72 ppm,hco3 - =488 ppm . calculate the lime and soda requ

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Answer 2

Answer:

The lime and soda that would be required to soften 2,50,000 litres of  Water is 43.2012. kg,  30.5080 kg.

Explanation:

Lime required is calculated to be as

= $\frac{74}{10} [38.72+298.08+200+50]\times\frac{10^5}{10^5}\times\frac{100}{100}$

It derived as  = $\frac{74}{10} [38.72+298.08+200+50]\times\frac{1}{10^3}$

lime required to soften the water(water softner) is   = 43.2012. kg

Soda required is calculated to be

=$\frac{10}{100} [160+295.08-200+50]\times\frac{10^5}{10^5} \times\frac{100}{100}$

It derives    =$305.08\times10^3$

Soda required to soften the water  is  = 30.5080 kg.

To learn more about of water softener, visit:

https://brainly.com/question/6765225

To learn more about of soda , visit:

https://brainly.com/question/13539235

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