Write a balanced equation for this reaction and include phases. B. Write the net ionic equation. C. If 55.0mL of 0.125M ammonium chromate and 35.0mL of 0.175M lead (II) nitrate are mixed in the reaction above, what mass of solid will precipitate? D. How many moles of excess reactant remains? E. If 1.65g of solid product are isolated, what is the percent yield?
Write a balanced equation for this reaction and include phases. B. Write the net ionic equation. C. If 55.0mL of 0.125M ammonium chromate and 35.0mL of 0.175M lead (II) nitrate are mixed in the reaction above, what mass of solid will precipitate? D. How many moles of excess reactant remains? E. If 1.65g of solid product are isolated, what is the percent yield?
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 14ALQ
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A student mixes an aqueous solution of ammonium chromate and an aqueous solution of lead (II) nitrate and notices a precipitation form.
A. Write a balanced equation for this reaction and include phases.
B. Write the net ionic equation.
C. If 55.0mL of 0.125M ammonium chromate and 35.0mL of 0.175M lead (II) nitrate are mixed in the reaction above, what mass of solid will precipitate?
D. How many moles of excess reactant remains?
E. If 1.65g of solid product are isolated, what is the percent yield?
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