A 5.351 g solid sample containing only KNO₂ (FW = 85.104 g/mol) and KNO3 (FW = 101.103 g/mol) is dissolved in 500.0 mL of water. A 50.00 mL aliquot of the solution is treated with 48.00 mL of 0.1171 M Ce** in strong acid to oxidize the nitrite (NO₂) ion and form the nitrate (NO3) ion. After 5 minutes, the excess Ce4+ is back-titrated with 33.57 mL of 0.04141 M Fe²+. Calculate the mass percent of KNO₂ in the solid.

A 5.351 g solid sample containing only KNO₂ (FW = 85.104 g/mol) and KNO3 (FW = 101.103 g/mol) is dissolved in 500.0 mL of water. A 50.00 mL aliquot of the solution is treated with 48.00 mL of 0.1171 M Ce** in strong acid to oxidize the nitrite (NO₂) ion and form the nitrate (NO3) ion. After 5 minutes, the excess Ce4+ is back-titrated with 33.57 mL of 0.04141 M Fe²+. Calculate the mass percent of KNO₂ in the solid.

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter4: Reactions In Aqueous Solution

Section: Chapter Questions

Problem 57QAP: A sample of limestone weighing 1.005 g is dissolved in 75.00 mL of 0.2500 M hydrochloric acid. The...

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