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a. Write the net ionic equation. b. Find the mass of the precipitate in the solution. c. How many moles of excess reagent will remain at the end of the reaction? d. Find the molar concentration of all the ions in the final solution.

a. Write the net ionic equation. b. Find the mass of the precipitate in the solution. c. How many moles of excess reagent will remain at the end of the reaction? d. Find the molar concentration of all the ions in the final solution.

Introductory Chemistry: A Foundation
Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter15: Solutions
Section: Chapter Questions
Problem 116AP
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7. 100.0 mL of 0.445 M potassium hydroxide is mixed with 90.0 mL of 0.215 M magnesium nitrate. a. Write the net ionic equation. b. Find the mass of the precipitate in the solution. c. How many moles of excess reagent will remain at the end of the reaction? d. Find the molar concentration of all the ions in the final solution.
Transcribed Image Text:7. 100.0 mL of 0.445 M potassium hydroxide is mixed with 90.0 mL of 0.215 M magnesium nitrate. a. Write the net ionic equation. b. Find the mass of the precipitate in the solution. c. How many moles of excess reagent will remain at the end of the reaction? d. Find the molar concentration of all the ions in the final solution.
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