Chemical Principles in the Laboratory
Chemical Principles in the Laboratory
11th Edition
ISBN: 9781305264434
Author: Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Publisher: Brooks Cole
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Textbook Question
Chapter 28, Problem 3ASA

A 100-mL sample of hard water is titrated with the EDTA solution in Problem 2. The same amount of Mg2+ is added as previously, and the volume of EDTA required is 31.84 mL.

a. What volume of EDTA is used in titrating the Ca2+ in the hard water? _____________mL

b. How many moles of EDTA are there in that volume? _____________ moles

c. How many moles of Ca2+ are there in the 100 mL of water? _____________ moles

d. If the Ca2+ comes from CaCO3, how many moles of CaCO3 are there in one liter of the water? How many grams of CaCO3 are present per liter of the water? _____________ mol / L _____________ g / L

e. If 1 ppm CaCO3 = 1 mg per liter, what is the water hardness in ppm CaCO3? _____________ ppm CaCO3

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If you have a sample of 100 mg/L of calcium, and you have two standardized EDTA solutions of 0.005 M and 0.001 M, which one is more adequate to spend approximately 15.00 mL of the titrant if 25.00 mL of sample are added in the Erlenmeyer flask? How many mL of titrant will be used? Solution: The 0.005 M solution. 12.5 mL will be used.
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Chemical Principles in the Laboratory

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  • You took 25.00 mL of unknown water solution and titrated it with EDTA. The EDTA solution molarity was 0.01 M, and it took 16.50 mL to reach the end point. With the blank it took only 0.98 mL to reach end point. A) How many milliliters of EDTA solution were used to titrate hardness that actually came from the unknown?  B) How many moles of EDTA reacted with hardness-causing ions from the unknown sample? C) How many moles of hardness-causing ions were present in the unknown sample? D) Assuming that the total hardness of water is due to CaCO3, how many grams CaCO3 does it correspond to? E) What is the total hardness of the unknown water in ppm CaCO3?
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    100 mL of mineral water containing Mg2+ and Ca2+ is taken and titrated with 86.65 mL of 0.06120 M EDTA. NH4F was added to the second 100 mL portion taken from the mineral water to mask the magnesium in the sample as MgF2, and when this sample was titrated with the same EDTA solution, 38.56 mL was spent. Find the concentration of CaCO3 and MgCO3 in the sample in ppm.
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