A50.00 ml sample of groundwater is titrated with 0.0750 m edta . if 10.30 ml of edta is required to titrate the 50.00 ml sample, what is the hardness of the groundwater in molarity and in parts per million of caco3 by mass? assume that ca2+ accounts for all of the hardness in the groundwater.

Concentration = 1545 ppm

Explanation:

Hardness of the water is generally due to the presence of in water.

At equivalence point

Moles of = Moles of EDTA

Considering

Given  that:

So,  

It means that 0.01545 moles are present in 1 L of the solution.

Molar mass of = 100 g/mol

The formula for the calculation of moles is shown below:

Thus, moles are:

Also, 1 g = 0.001 mg

So, mass = 1545 mg

Concentration = 1545 mg/L

1 mg/L = 1 ppm

So, Concentration = 1545 ppm

Hey There!

To solve this question remember that 1 mole of ammonia is equal to 17G of ammonia.

Using that, we first multiply 17 by 7 = 24

Then we multiply 7 by .27 = 1.89

Finally, taking those and adding them together gives you the answer...

25.89 grams :)

Have a great day, I hope I helped.

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