Question

. A water sample contains 16.2 mg/L Ca(HCO3)2, 7.3 mg/L Mg(HCO3)2, 9.5 mg/L MgCl2 and
13.6 mg/L CaSO4. Calculate the temporary and permanent hardness of water and what will
happen if 10.6 mg/L NaHCO3 is added

Answer 1

Answer:

. A water sample contains 16.2 mg/L Ca(HCO3)2, 7.3 mg/L Mg(HCO3)2, 9.5 mg/L MgCl2 and

. A water sample contains 16.2 mg/L Ca(HCO3)2, 7.3 mg/L Mg(HCO3)2, 9.5 mg/L MgCl2 and 13.6 mg/L CaSO4. Calculate the temporary and permanent hardness of water and what will

. A water sample contains 16.2 mg/L Ca(HCO3)2, 7.3 mg/L Mg(HCO3)2, 9.5 mg/L MgCl2 and 13.6 mg/L CaSO4. Calculate the temporary and permanent hardness of water and what will happen if 10.6 mg/L NaHCO3 is added

Answer 2

Answer:

1

Explanation:

mole of Ca(HCO3 ) 2= 162×10 ^−3mg/162gm

​ =1×10 ^−moles

Mole of Ca(SO4 )= 136×10 ^−3g/136gm/mol

=1×10 ^3mole

Total mole of Ca=2×10^−3mole

mass of CaCO3=2×10^−3×100=0.2g

∴ ppm (permanent hardness) = 6.2/1000×10^6

=200ppm

Mole of MgCl 2=95×10^−3/95

=1×10^-3mole

Mole Mg (HCg) 2= 73×10^−3/146

=5×10^−4mole

mole Mg =1.5×10^−4 mole

Mole g CaCO 3 (In terms of mg) =1.5×10^−3

mass =1.5×10^−3

=0.150g

ppm (temporary hardness) = 0.150/1000×106=150ppm