1. (a). Gravimetric analysis is very useful for routine monitoring of ions present in relatively high concentrations. Why is gravimetric analysis not used for determining trace amounts of ions? (b). Discuss the sources of error in this experiment. 2. From 0.323 g of an unknown chloride sample (M-Cly), it produces 0.523 g of AgCl(s) solid under gravimetric analysis. What is the percentage of Cl- in the unknown sample? What is the theoretical molar weight of the metal in the chlorite salt sample M-Cly for the following given conditions? a. x = 1, y = 1; b. x = 1, y = 2; x = 2, y = 4. C.
1. (a). Gravimetric analysis is very useful for routine monitoring of ions present in relatively high concentrations. Why is gravimetric analysis not used for determining trace amounts of ions? (b). Discuss the sources of error in this experiment. 2. From 0.323 g of an unknown chloride sample (M-Cly), it produces 0.523 g of AgCl(s) solid under gravimetric analysis. What is the percentage of Cl- in the unknown sample? What is the theoretical molar weight of the metal in the chlorite salt sample M-Cly for the following given conditions? a. x = 1, y = 1; b. x = 1, y = 2; x = 2, y = 4. C.
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Transcribed Image Text:Include answers to the following questions in your discussion.
1. (a). Gravimetric analysis is very useful for routine monitoring of ions present in relatively high
concentrations. Why is gravimetric analysis not used for determining trace amounts of ions?
(b). Discuss the sources of error in this experiment.
From 0.323 g of an unknown chloride sample (M.Cly), it produces 0.523 g of AgCl(s) solid under
gravimetric analysis. What is the percentage of Cl in the unknown sample? What is the theoretical
molar weight of the metal in the chlorite salt sample M.Cly for the following given conditions?
a. x= 1, y = 1;
b.
x = 1, y = 2;
2.
c.
x = 2, y = 4.
23
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