If 150.0 mL of 2.5 mol/L Na2SO4 is mixed with 125 mL of 0.26 mol/L AgNO3, determine the concentration of excess reactant remaining after the reaction has taken place. Excess potassium sufide is added to 1.25 L of iron (II) nitrate solution. The mass of precipitate that forms is 4.26 g. What was the concentration of nitrate ions in the original solution?
If 150.0 mL of 2.5 mol/L Na2SO4 is mixed with 125 mL of 0.26 mol/L AgNO3, determine the concentration of excess reactant remaining after the reaction has taken place. Excess potassium sufide is added to 1.25 L of iron (II) nitrate solution. The mass of precipitate that forms is 4.26 g. What was the concentration of nitrate ions in the original 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
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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If 150.0 mL of 2.5 mol/L Na2SO4 is mixed with 125 mL of 0.26 mol/L AgNO3, determine the concentration of excess reactant remaining after the reaction has taken place.
Excess potassium sufide is added to 1.25 L of iron (II) nitrate solution. The mass of precipitate that forms is 4.26 g. What was the concentration of nitrate ions in the original solution?
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