Chemical Principles in the Laboratory
11th Edition
ISBN: 9781305264434
Author: Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Publisher: Brooks Cole
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Experiment 28
Advance Study Assignment: Determination of the Hardness of Water
1. A 0.3946 g sample of CaCO, is dissolved in 12 M HCI and the resulting solution is diluted to 250.0 mL
in a volumetric flask.
a. How many moles of CACO, are used (formula mass = 100.1)?
moles
b. What is the molarity of the Ca²* in the 250 mL of solution?
M
c. How many moles of Ca" are in a 25.00-mL aliquot of the solution in Ib?
moles
.. moles 아 Cacos 드
Weight in gram
formula mass
0-3946
1001
E3.942 x 10-3 mol
moles of solute
Molanity
Volume of solution (L)
3.942 x 1o-3
x 1000
250
0.0158 M
Imol Caco, produce
I mol
Cast ion
0.0158 M
Moles off Ca²+ =
Molarity x
0.0158
Vo lume lin L)
25
1000
3.94 X10-4mol.
A 25.00 mL unknown water sample is titrated with a standardized 0.0140 M EDTA solution. It is determined that 8.54 mL of EDTA is required to reach the end point. The blank titre was determined to be 1.50 mL. Determine the concentration of Calcium in the water sample in ppm. (mwt. of CaCO3 = 100.0892 g/mol).
25.00 mL aliquots of the solution in problem 1 are titrated with EDTA to the calmagite end point. A blank containing a small measured amount of Mg^2+ requires 2.12 mL of the EDTA to reach the end point. An aliquot to which the same amount of Mg^2+ is added requires 25.88 mL of the EDTA to reach the end point.
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- A 5.00 mL tap water sample was measured out with a volumetric pipette, and added to a 25 mL Erlenmeyer flask. It was then titrated with a 0.0100 M Na2EDTA.2H2O solution, and found to take 0.635 mL of the EDTA solution to reach the blue endpoint. a.) How many moles of the 0.0100 M Na2EDTA.2H2O were added in the titration reaction? Show calculation. b.) How many moles of calcium ions were reacted?arrow_forward4.50 mL of 0.1 M Ca2+ ion was titrated at pH 10 with 0.1 M EDTA. What will be the concentration of Ca2+ ions in the solution when 25 mL, 50 mL and 75 mL EDTA is added(a4 = 0.35, Kf = 5.0x1010)?arrow_forward25 ml of 0.05M Hg2(NO3)2 was titrated with 0.06M KIO3 Hg2*2 + 2103 Hg(103)2 Ksp= 1.3x10-18 == Calculate the Hg2*2 concentration after adding 40ml KIO3 a. 1.69x10-15M O b. 0.06M O c. 2.98x10-4 O d. 7.69x10-4 Marrow_forward
- A 5.00 mL tap water sample was measured out with a volumetric pipette, and added to a 25 mL Erlenmeyer flask. It was then titrated with a 0.0100 M Na2EDTA.2H2O solution, and found to take 0.635 mL of the EDTA solution to reach the blue endpoint. How many moles of the 0.0100 M Na2EDTA.2H2O were added in the titration reaction? Show calculation. How many moles of calcium ions were reacted? Show calculation.arrow_forward20. Assume you are using 0.1 M EDTA to titrate a 0.2 M Ca2t solution (25 mL) at pH 10.0. W molarity of free Ca* ions in the solution after 50 mL of the EDTA is added? K=5.0X101º. A. 2.11 X 106 M B. 8.16 X 10 M C. 4.97 X 106 M D. 8.36 X 10 6 Marrow_forwardAn unknown solution containing 25.00 mL of Ni2+ in dilute HCl is treated with a known excess of 25.00 mL of 0.05382 M EDTA solution. The solution turns yellow when a few drops of indicator are added. The excess unreacted EDTA back titrated with 0.02299 M Zn2+, which requires 17.00 mL to reach the red end point. What is the molarity of Ni2+ in the unknown solution?arrow_forward
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