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
Chemistry: Principles and Practice
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ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter4: Chemical Reactions In Solution
Section: Chapter Questions
Problem 4.51QE: What is the molarity of a solution of strontium chloride that is prepared by dissolving 4.11 g SrCl2...
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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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what are the numbers in scientific notation? where did they come from? Is there any chance you could elbaborate on step 2?! Thank you!
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