10. A 50.0ml solution containing Ni2+ and Zn2+ was treated with 25.0 ml 0.0452M EDTA to bind all the metals. The excess unreacted EDTA required 12.4 ml 0.0123M Mg2+ for complete reaction. An excess reagent is added again to replace EDTA from Zn2+. Another 29.2 ml of 0.0123M Mg2+ were required for reaction with the liberated EDTA. Calculate the molarity of Ni2+ and Zn2+ in the original solution. a) Ni2+ = 0.0110 M, Zn2+ = 7.1832 x 10^-3 M O b) Ni2+ = 7.18 x10-^3 M, Zn2+ = 5.57x 10^-3 M c) Ni2+ = 9.09 x10 ^-4 M, Zn2+ = 1.0625x 10^-3 M d) none of the above results Option 5
10. A 50.0ml solution containing Ni2+ and Zn2+ was treated with 25.0 ml 0.0452M EDTA to bind all the metals. The excess unreacted EDTA required 12.4 ml 0.0123M Mg2+ for complete reaction. An excess reagent is added again to replace EDTA from Zn2+. Another 29.2 ml of 0.0123M Mg2+ were required for reaction with the liberated EDTA. Calculate the molarity of Ni2+ and Zn2+ in the original solution. a) Ni2+ = 0.0110 M, Zn2+ = 7.1832 x 10^-3 M O b) Ni2+ = 7.18 x10-^3 M, Zn2+ = 5.57x 10^-3 M c) Ni2+ = 9.09 x10 ^-4 M, Zn2+ = 1.0625x 10^-3 M d) none of the above results Option 5
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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Transcribed Image Text:10. A 50.0ml solution containing Ni2+ and Zn2+ was treated with 25.0 ml
0.0452M EDTA to bind all the metals. The excess unreacted EDTA required 12.4
ml 0.0123M Mg2+ for complete reaction. An excess reagent is added again to
replace EDTA from Zn2+. Another 29.2 ml of 0.0123M Mg2+ were required for
reaction with the liberated EDTA. Calculate the molarity of Ni2+ and Zn2+ in the
original solution.
O a) Ni2+ = 0.0110 M, Zn2+ = 7,1832 x 10^-3 M
O b) Ni2+ =7.18 x10-^3 M, Zn2+ = 5.57x 10^-3 M
O C) Ni2+ = 9.09 x10 ^-4 M, Zn2+ = 1.0625x 10^-3 M
O d) none of the above results
Option 5
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