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.
A water sample is approximated to have a total hardness equal to 120.0ppm. How many milliliters of 0.01000N EDTA will be needed to titrate 250.00mL of the said water sample?(MM CaCO3=100.09g/mol).
** Need asap pls. Thanks.
A student titrated a 25.00 mL sample of water with 0.0200 M EDTA. The titration required 20.40 mL of EDTA. Calculate the ppm hardness in the water sample
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Chemical Principles in the Laboratory
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