Mass of CaO will be required to remove the hardness of 1000 litres of water containing 1.62 g of calcium bicarbonate per litre is A. Find value of A

Calculate the amount of lime Ca(OH)_2 required to remove the hardness of 60,000 litres of well water containing 16.2 g of calcium bicarbonate per hundred litre. (Atomic masses Ca = 40, C = 12, O = 16, H = 1)

Find the value 3.75% of 1000 litre

Calculate the weight of CaO required to remove hardness of 10^(6) L of water containing 1.62 g of Ca (HCO_(3))_(2) in 1.0 L . (Mw of Ca (HCO_(3))_(2) = 162, mw of CaO = 56)

A sample of hard water contains 96 pp m."of" SO_(4)^(2-) and 183 pp m "of" HCO_(3)^(-) , with Ca^(2+) as the only cation. How many moles of CaO will be required to remove HCO_(3)^(-) from 1000 kg of this water? If 1000 kg of this water is treated with the amount of CaO calculated above, what will be the concentration (in ppm)of residual Ca^(2+) ions (Assume CaCO_(3) to be completely insoluble in water)? If the Ca^(2+) ions in one litre of the treated water are completely exchange with hydrogen ions, what will be its pH (One ppm means one part of the substance in one million part of water, weight // weight)?