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13 Dec 2019

After a treated water sample of 1.00x10^6 L had a hardness of 156ppm CaCO3 it was reduced to 117ppm CaCO3 from cold lime softening. The question I have is taking this same sample of water after cold lime softening and removal of the precipated CaCO3, how many moles(show work) of EDTA are required to further reduced the water's hardness from 117ppm to 85ppm?

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Irving Heathcote
Irving HeathcoteLv2
17 Dec 2019

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Related questions

Please show all steps I need to understand this question. Make clear handwriting. I want it asap. Thanks

the density of the sample is 0.9977 g/mL and the molar mass of calcium carbonate is 100.0 g/mol.
2. Calculate the number of moles of calcium ions present in a 50.00 mL water
sample that has a hardness of 75.0 ppm (hardness due to CaCO3).
3. If the 50.00 mL sample from problem 2 above was titrated with a 0.00500 M
EDTA, what volume (in milliliters) of EDTA solution would be needed to reach
the endpoint?

If someone could show their work and help me out that would be great. I always seem to get hung up on setting the problem up.

Thank you.

1 A .5118 g sample of CaCO3 is disolve in concentrated HCl(12M). the solution was diluted to 250 mL in a volumetric flask toobtain a solution for standardizing the EDTA titrant.

a How many moles of CaCO3 are used (MW=100.1)? .0051mol

b What is the molarity of the Ca2+ (calcium ion) in the 250mL ofsolution? .020M
c How many moles of Ca2+ are in a 25 mL aliquot of the solution inpart b? .0005 mol

2. 25.00 mL aliquots of the solution from Part 1 are titratedwith EDTA to the Eriochrome Black T end point. A blank containing asmall measured amount of Mg2+ requires 2.60 mL of the EDTA to reachthe end point. An aliquot to which the same amount of Mg2+ is addedrequires 28.55 mL of the EDTA to reach the end point.

How many milliliters of EDTA are needed to titrate the Ca+2 ion inthe aliquot? 27.56mL

How many moles of EDTA are there in the volume obtained in theprevious question? .0051mol

What is the molarity of the EDTA solution? 0.185M

3. A 100.0 mL sample of hard water is titrated with theEDTA solution from Part 2. The same amount of Mg2+ is added aspreviously, and the volume of EDTA required is 22.44mL

What volume of EDTA is used in titrating the Ca2+ in thehard water?

How many moles of EDTA are there in thatvolume?

How many moles of Ca2+ are there in the 100.0 mL volume ofwater?

If the Ca2+ comes from CaCO3, how many moles of CaCO3 arethere in one liter of the water?

How many grams of CaCO3 per liter?

If 1 ppm (part-per-million) CaCO3 = 1 mg per liter, what isthe water hardness in ppm CaCO3?

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