Question
What is the $\mathrm{mEq}$ wt of ferrous ion $\left(\mathrm{Fe}^{2+} ; \mathrm{g}\right.$-atomic wt of $55.85 \mathrm{~g}$ )?
Step 1
The valency of Fe$^{2+}$ is 2, which means it has a charge of +2. Show more…
Show all steps
Your feedback will help us improve your experience
Adriano Chikande and 60 other educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
The amount of $\mathrm{Fe}^{2+}(a q)$ in an $\mathrm{FeSO}_{4}(a q)$ solution can be determined by titration with a solution containing a known concentration of $\mathrm{Ce}^{4+}(a q)$. The determination is based on the reaction described by $$ \mathrm{Fe}^{2+}(a q)+\mathrm{Ce}^{4+}(a q) \rightarrow \mathrm{Fe}^{3+}(a q)+\mathrm{Ce}^{3+}(a q) $$ Given that it requires $37.5 \mathrm{~mL}$ of $0.0965 \mathrm{M} \mathrm{Ce}^{4+}(a q)$ to completely oxidize the $\mathrm{Fe}^{2+}(a q)$ in a $35.0-\mathrm{mL}$ sample to $\mathrm{Fe}^{3+}(a q)$, calculate the molarity of $\mathrm{Fe}^{2+}(a q)$ and the number of milligrams of iron in the sample.
To analyze an iron-containing compound, you convert all the iron to $\mathrm{Fe}^{2+}$ in aqueous solution and then titrate the solution with standardized $\mathrm{KMnO}_{4} .$ The balanced, net ionic equation is $$\begin{aligned} \mathrm{MnO}_{4}^{-}(\mathrm{aq})+5 \mathrm{Fe}^{2+}(\mathrm{aq})+8 \mathrm{H}_{3} \mathrm{O}^{+}(\mathrm{aq}) & \rightarrow \\ \mathrm{Mn}^{2+}(\mathrm{aq})+5 \mathrm{Fe}^{3+}(\mathrm{aq})+& 12 \mathrm{H}_{2} \mathrm{O}(\ell) \end{aligned}$$ A 0.598 -g sample of the iron-containing compound requires $22.25 \mathrm{mL}$ of $0.0123 \mathrm{M} \mathrm{KMnO}_{4}$ for titration to the equivalence point. What is the mass percent of iron in the sample?
An alternative procedure to that given in Problem $4.122$ for determining the amount of iron in a sample is to convert the iron to $\mathrm{Fe}^{2+}$ and then titrate it with a solution of $\mathrm{Ce}\left(\mathrm{NH}_{4}\right)_{2}\left(\mathrm{NO}_{3}\right)_{6}$ $\mathrm{Fe}^{2+}(a q)+\mathrm{Ce}^{4+}(a q) \longrightarrow \mathrm{Fe}^{3+}(a q)+\mathrm{Ce}^{3+}(a q)$ What is the mass percent of iron in a sample if $1.2284 \mathrm{~g}$ of the sample requires $54.91 \mathrm{~mL}$ of $0.1018 \mathrm{M} \mathrm{Ce}\left(\mathrm{NH}_{4}\right)_{2}\left(\mathrm{NO}_{3}\right)_{6}$ for complete reaction?
Reactions in Aqueous Solution
Some Applications of Redox Reactions
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD