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Chapter 21: Q21.85P (page 976)

In an aqueous electrolytic cell, nitrate ions never react at the anode, but nitrite ions do. Explain.

Short Answer

Expert verified

Unlike nitrites, nitrates can no longer be oxidised.

Step by step solution

01

Step 1:

In nitrates, the oxidation number of Nitrogen is $+ 5$ , while in nitrites, the oxidation number of Nitrogen is only $+ 3$ ,therefore it can still be further oxidized and have its oxidation number increase.

Nitrates do not react in the anode because they can no longer be oxidized, unlike nitrites. Hence nitrate can no Longer be oxidized, unlike nitrites.

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Most popular questions from this chapter

How is a standard reference electrode used to determine unknown $E^{o}$ half-cell values?

During the redox balancing process, what step is taken to ensure thatloss equalsgain?

Use the emf series (Appendix D) to arrange the species.

(a) In order of decreasing strength as oxidizing agents: ${Fe}^{3+} {,Br}_{2} {,Cu}^{2+}$

(b) In order of increasing strength as oxidizingagents : ${Ca}^{2+},$ ${Cr}_{2} O_{7}^{2-}$ , ${Ag}^{+}$

Balance the following skeleton reactions and identify the oxidizing and reducing agents:

(a) ${ClO}_{3}^{-} (aq) + I^{-} (aq) \to I_{2} (s) + {Cl}^{-} (aq) [acidic]$

(b) ${MnO}_{4}^{-} (aq) + {SO}_{3}^{2 -} (aq) \to {MnO}_{2} (s) + {SO}_{4}^{2 -} (aq) [basic]$

(c) ${MnO}_{4}^{-} (aq) + H_{2} O_{2} (aq) \to {Mn}^{2 +} (aq) + O_{2} (g) [acidic]$

What is the value of the equilibrium constant for the reaction between each pair at $25 ° C$ ?

$\begin{array}{l} {(a)Al(s)andCd}^{2+} (aq) \\ {(b)I}_{2} {(s)andBr}^{-} (aq) \end{array}$

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