For problem 5, the density of the sample is 0.9977 g/ml. and the molar mass of calcium carbonate is 100.0g/mol.5.As described in Topic 2 in the lab manual, the hardness of water is expressed in terms of amountof calcium carbonate according to the ppm expression.Calculate the mass of calcium carbonate present in a 50.00 mL sample of an aqueouscalcium carbonate standard, assuming the standard is known to have a hardness of75.0 ppm (hardness du to CaCO;).a.b.Calculate the number of moles of calcium ions present in this 50.00 mL sample ofaqueous calcium carbonate standard.C.The 50.00 mL sample (at pH 10) was titrated with a 0.00500 M EDTA solution,Write the balance net ionic equation for the reaction of EDTA“ with a calcium ion.Calculate the number of moles of EDTA“ needed to completely react with calciumions in the sample.What volume (in milliliters) of EDTA solution would be needed to reach theequivalence point?

a) 50 ml = 50/1000 L = 0.05 L ppm = mass…

Answered: balance net ionic equation for the…

balance net ionic equation for the reaction of EDTA“ with a calcium ion.

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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