A chemist must prepare of nitric acid solution with a pH of at . He will do this in three steps: Fill a volumetric flask about h
alfway with distilled water. Measure out a small volume of concentrated () stock nitric acid solution and add it to the flask. Fill the flask to the mark with distilled water. Calculate the volume of concentrated nitric acid that the chemist must measure out in the second step. Round your answer to significant digits.
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<u>Answer:</u> The given amount of iron reacts with 9.0 moles of and produce 6.0 moles of
<u>Explanation:</u>
We are given:
Moles of iron = 12.0 moles
The chemical equation for the rusting of iron follows:
- <u>For oxygen gas:</u>
By Stoichiometry of the reaction:
4 moles of iron reacts with 3 moles of oxygen gas
So, 12.0 moles of iron will react with = of oxygen gas
- <u>For iron (III) oxide:</u>
By Stoichiometry of the reaction:
4 moles of iron produces 2 moles of iron (III) oxide
So, 12.0 moles of iron will produce = of iron (III) oxide
Hence, the given amount of iron reacts with 9.0 moles of and produce 6.0 moles of