To oxidize the iron in 1.00 gram of FeSO4·(NH4)2SO4·6 H2O requires 5.00 mL of HNO3. (Fe 2++ NO3― + H+→ Fe 3++ NO + H2O) How much water must be added to 500 mL of this acid to make the concentration as an acid exactly one-tenth normal?
To oxidize the iron in 1.00 gram of FeSO4·(NH4)2SO4·6 H2O requires 5.00 mL of HNO3. (Fe 2++ NO3― + H+→ Fe 3++ NO + H2O) How much water must be added to 500 mL of this acid to make the concentration as an acid exactly one-tenth normal?
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter4: Stoichiometry: Quantitative Information About Chemical Reactions
Section: Chapter Questions
Problem 111GQ: One half liter (500. mL) of 2.50 M HCl is mixed with 250. mL of 3.75 M HCl. Assuming the total...
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To oxidize the iron in 1.00 gram of FeSO4·(NH4)2SO4·6 H2O requires 5.00 mL of HNO3.
(Fe 2++ NO3― + H+→ Fe 3++ NO + H2O)
How much water must be added to 500 mL of this acid to make the concentration as an acid exactly one-tenth normal?
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