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
Expert Solution & Answer
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5. A student titrated a 25.00 mL sample of water with 0.0100 M EDTA. The titration required
16.40 mL of EDTA.
a.
Calculate the moles of EDTA used.
b. Calculate the moles of hardness in the water sample.
Calculate the moles of hardness per liter of water.
c.
d. Calculate the ppm hardness in the water sample.
BBe
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EXPERIMENT 4
3. A 100 mL sample of hard water is titrated with 22.4 mL of the EDTA solution from problem
2. The same amount of MgCI, is added as previously and the total volume of EDTA solution
required is 22.44 mL.
a) What volume of EDTA is used in titrating the Ca²* in the hard water?
b) How many moles of EDTA are there in that volume?
moles
2+
c) How many moles of Ca²“ are in 100 mL of water?
moles
50 mL of a sample known to contain Mg+2 was taken and titrated with 0.075 M EDTA standard solution by adding pH 10 buffer and EBT indicator. Since the EDTA consumption is 10.5 mL, which of the following is the amount of magnesium in the sample in ppm? (Mg:24 g/mol)
A.
378
B.
302
C.
214
D.
251
Chapter 28 Solutions
Chemical Principles in the Laboratory
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