(a) the molarity of Ag* ions in 100 mL of solution, which corresponds to 0.0001 g of remaining Ag* ions; (b) the molarity of (NH4)2CrO, needed to get saturated solution of Ag2CrOA (pK° sp = 11.92) with remaining concentration of Ag* equal to found on the previous step.
(a) the molarity of Ag* ions in 100 mL of solution, which corresponds to 0.0001 g of remaining Ag* ions; (b) the molarity of (NH4)2CrO, needed to get saturated solution of Ag2CrOA (pK° sp = 11.92) with remaining concentration of Ag* equal to found on the previous step.
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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The precipitation of some ion can be treated as completed if the mass of the remaining ions in precipitated
solution will be less than 0.0001 g (the minimal mass can be weighed using typical lab balance). Calculate:
(a) the molarity of Ag* ions in 100 mL of solution, which corresponds to 0.0001 g of remaining Ag* ions;
(b) the molarity of (NH4)2CrO, needed to get saturated solution of Ag2CrOA (pK° sp = 11.92) with remaining
concentration of Ag* equal to found on the previous step.
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