Chemistry: Principles and Reactions
8th Edition
ISBN: 9781305079373
Author: William L. Masterton, Cecile N. Hurley
Publisher: Cengage Learning
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Chapter 20, Problem 29QAP
Using Table 20.4, calculate, for the disproportionation of Fe2+,
(a) the equilibrium constant, K.
(b) the concentration of Fe3+ in equilibrium with 0.10 M Fe2+.
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1. A sample of iron ore weighing 0.6428 g is dissolved in acid The iron is reduced to Fe*2 and titrated
with 36.30 mL of a 0.1052 N solution of K2Cr207. (a) Calculate the percentage of iron (Fe) in the
sample. (b) Express the percentage as Fe,03 rather than Fe.
Hint: The reaction of Fe2+ with Cr,0,2 involves one electron to oxidize it to Fe*.
1. A sample of iron ore weighing 0.6428 g is dissolved in acid The iron is reduced to Fe* and titrated
with 36.30 mL of a 0.1052 N solution of K,Cr207. (a) Calculate the percentage of iron (Fe) in the
sample. (b) Express the percentage as Fe,03 rather than Fe.
Hint: The reaction of Fe2+ with Cr,0,2 involves one electron to oxidize it to Fe*.
Explain how the diphosphate ion, [O3P−O−PO3]4−, can function as a water softener that prevents the precipitation of Fe2+ as an insoluble iron salt.
Chapter 20 Solutions
Chemistry: Principles and Reactions
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