Consider the reaction taking place between 20.0 mL of a 1.05 M aqueous solution of AgNO3 and 15.0 mL of a 1.00 M aqueous solution of K2CrO4. When these react, a precipitate is observed. a)What is the nature of the precipitate? Write down its formula AND its name. b)What is present in solution after the reaction is complete? Note: the solid is not considered to be in solution. c)Calculate the mass of solid obtained. d)Calculate the concentration of all the remaining ions in solution.
Consider the reaction taking place between 20.0 mL of a 1.05 M aqueous solution of AgNO3 and 15.0 mL of a 1.00 M aqueous solution of K2CrO4. When these react, a precipitate is observed. a)What is the nature of the precipitate? Write down its formula AND its name. b)What is present in solution after the reaction is complete? Note: the solid is not considered to be in solution. c)Calculate the mass of solid obtained. d)Calculate the concentration of all the remaining ions in solution.
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
Chapter4: Types Of Chemical Reactions And Solution Stoichiometry
Section: Chapter Questions
Problem 113AE: A student added 50.0 mL of an NaOH solution to 100.0 mL of 0.400 M HCl. The solution was then...
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Consider the reaction taking place between 20.0 mL of a 1.05 M aqueous solution of AgNO3 and 15.0 mL of a 1.00 M aqueous solution of K2CrO4. When these react, a precipitate is observed.
a)What is the nature of the precipitate? Write down its formula AND its name.
b)What is present in solution after the reaction is complete? Note: the solid is not considered to be in solution.
c)Calculate the mass of solid obtained.
d)Calculate the concentration of all the remaining ions in solution.
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