20.0 mL of a 0.450 M solution of BaCl2(aq) is added to 40.0 mL of a 0.250 M solution of K2SO4(aq). a. what is the total ionic equation for this reaction and physical states? b. What is the mass (g) of any precipate(s) that form? c. What is the concentration (in Molarity) of each anion that remains in solution
20.0 mL of a 0.450 M solution of BaCl2(aq) is added to 40.0 mL of a 0.250 M solution of K2SO4(aq). a. what is the total ionic equation for this reaction and physical states? b. What is the mass (g) of any precipate(s) that form? c. What is the concentration (in Molarity) of each anion that remains in solution
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter7: Reactions In Aqueous Solutions
Section: Chapter Questions
Problem 9CR: n general terms, what are the spectator ions in a precipitation reaction? Why are the spectator ions...
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20.0 mL of a 0.450 M solution of BaCl2(aq) is added to 40.0 mL of a 0.250 M solution of K2SO4(aq).
a. what is the total ionic equation for this reaction and physical states?
b. What is the mass (g) of any precipate(s) that form?
c. What is the concentration (in Molarity) of each anion that remains in solution
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