If a sample of tap water contains 400 ppm of Ca2+ and 80 ppm of Mg2+,...
If a sample of tap water contains 400 ppm of Ca2+ and 80 ppm of Mg2+, what is the hardness of this water sample in terms of equivalent concentration CaCO3, in mg/L?
Homework Answers
MCaCo3/MCa=100/40=2.5....... as because the molar mass of calcium carbonate is 100 and atomic weight of Ca is 40
MCaCo3/MMg=100/24.3=4.1.......Molar mass of Magnesium is 24.3
We know,
Hardness= 2.5[Ca2+]+4.1[Mg2+] =2.5*400+4.1*80=1328 ppm
Hence the answer is 1328 ppm in CaCO3 scale and it is of high hardness.
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If a sample of tap water contains 400 ppm of Ca2+ and 80 ppm of
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Ca(OH)2 is added to water to reach a concentration of 53 mg/L. Initially, the water had 3.09 mg/L of Mg2+ and it reacts...
Ca(OH)2 is added to water to reach a concentration of
53 mg/L. Initially, the water had 3.09 mg/L of Mg2+ and
it reacts with Ca(OH)2 according to equation 61a. Assume
SO4-2 is in excess. What are the final
dissolved Ca2+and Mg 2+ concentrations? What
is the initial and final hardness? What is the Mg(OH)2
precipitate concentration? (28.6 mg/L, 0 mg/L, 12.5 mg CaCO3/L,
71.5 mg CaCO3 /L, 7.28 mg/L).
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Ca(OH)2 is added to water to reach a concentration of
53 mg/L. Initially, the water had 3.09 mg/L of Mg2+ and
it reacts with Ca(OH)2 according to equation 61a. Assume
SO4-2 is in excess. What are the final
dissolved Ca2+and Mg 2+ concentrations? What
is the initial and final hardness? What is the Mg(OH)2
precipitate concentration? (28.6 mg/L, 0 mg/L, 12.5 mg CaCO3/L,
71.5 mg CaCO3 /L, 7.28 mg/L).
Precipitation of noncarbonate Mg, leaving Ca from lime in solution. Mf+...
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