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Chapter 21: Problem 18

Write a balanced net ionic equation for the disproportionation reaction of (a) hypochlorous acid to chlorine gas and chlorous acid in acidic solution. (b) chlorate ion to perchlorate and chlorite ions.

Short Answer

Expert verified
Question: Write the balanced net ionic equations for the following disproportionation reactions: (a) The reaction of hypochlorous acid to chlorine gas and chlorous acid in acidic solution. (b) The reaction of chlorate ion to perchlorate and chlorite ions. Answer: (a) 3 HOCl + 4H⁺ → Cl₂ + 2 HClO₂ + H₂O (b) 3 ClO₃⁻ → 2 ClO₄⁻ + 2 ClO₂⁻

Step by step solution

01

Write half-reactions for oxidation and reduction

The oxidation half-reaction is the conversion of hypochlorous acid to chlorine gas: \(2 \text{HOCl} \rightarrow \text{Cl}_2 + 2 \text{H}^+ +2e^-\) The reduction half-reaction is the conversion of hypochlorous acid to chlorous acid: \(\text{HOCl} + e^- \rightarrow \text{HClO}_2\)
02

Balance the half-reactions

The oxidation half-reaction is already balanced. The reduction half-reaction must be balanced by adding water. \(\text{HOCl} + e^- + 2H^+ \rightarrow \text{HClO}_2 + H_2O\)
03

Add the balanced half-reactions

To add the half-reactions, first multiply to get equal numbers of electrons, and then combine the half-reactions: \(2 (\text{HOCl} + e^- + 2H^+ \rightarrow \text{HClO}_2 + H_2O) + (2 \text{HOCl} \rightarrow \text{Cl}_2 + 2 \text{H}^+ +2e^-)\)
04

Cancel out the common species and get the net ionic equation

After cancelling out the common species, we get the net ionic equation: \(3 \text{HOCl} + 4H^+ \rightarrow \text{Cl}_2 + 2 \text{HClO}_2 + H_2O\) (b) Chlorate ion to perchlorate and chlorite ions.
05

Write half-reactions for oxidation and reduction

The oxidation half-reaction is the conversion of chlorate ion to perchlorate ion: \(2\text{ClO}_3^- \rightarrow 2\text{ClO}_4^- +2e^-\) The reduction half-reaction is the conversion of chlorate ion to chlorite ion: \(\text{ClO}_3^- + 2e^- \rightarrow \text{ClO}_2^-\)
06

Balance the half-reactions

Both oxidation and reduction half-reactions are already balanced.
07

Add the balanced half-reactions

To add both half-reactions, first multiply the reduction half-reaction by 2 to get equal numbers of electrons, and then combine the half-reactions: \((2\text{ClO}_3^- \rightarrow 2\text{ClO}_4^- +2e^-) + 2 (\text{ClO}_3^- + 2e^- \rightarrow \text{ClO}_2^-)\)
08

Cancel out the common species and get the net ionic equation

After cancelling out the common species, we get the net ionic equation: \(3 \text{ClO}_3^- \rightarrow 2 \text{ClO}_4^- + 2 \text{ClO}_2^-\)

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Most popular questions from this chapter

Consider the equilibrium system $$\mathrm{HF}(a q) \rightleftharpoons \mathrm{H}^{+}(a q)+\mathrm{F}^{-}(a q)$$ Given \(\Delta H_{\mathrm{f}}^{\circ} \mathrm{HF}(a q)=-320.1 \mathrm{~kJ} / \mathrm{mol}\), $$\begin{aligned} \Delta H_{\mathrm{f}}^{\circ} \mathrm{F}^{-}(a q) &=-332.6 \mathrm{~kJ} / \mathrm{mol} ; S^{\circ} \mathrm{F}^{-}(a q)=-13.8 \mathrm{~J} / \mathrm{mol} \cdot \mathrm{K} \\ K_{\mathrm{a}} \mathrm{HF} &=6.9 \times 10^{-4} \text { at } 25^{\circ} \mathrm{C} \end{aligned}$$ calculate \(S^{\circ}\) for \(\mathrm{HF}(a q)\).

Given $$\begin{array}{ll} \mathrm{HF}(a q) \rightleftharpoons \mathrm{H}^{+}(a q)+\mathrm{F}^{-}(a q) & K_{\mathrm{a}}=6.9 \times 10^{-1} \\ \mathrm{HF}(a q)+\mathrm{F}^{-}(a q) \rightleftharpoons \mathrm{HF}_{2}-(a q) & K=2.7 \end{array}$$ calculate \(K\) for the reaction $$ 2 \mathrm{HF}(a q) \rightleftharpoons \mathrm{H}^{+}(a q)+\mathrm{HF}_{2}^{-}(a q) $$

What is the concentration of fluoride ion in a water solution saturated with \(\mathrm{BaF}_{2}, K_{s \mathrm{p}}=1.8 \times 10^{-7}\) ?

The average concentration of bromine (as bromide) in seawater is \(65 \mathrm{ppm} .\) Calculate (a) the volume of seawater \(\left(d=64.0 \mathrm{lb} / \mathrm{ft}^{3}\right)\) in cubic feet required to produce one kilogram of liquid bromine. (b) the volume of chlorine gas in liters, measured at \(20^{\circ} \mathrm{C}\) and \(762 \mathrm{~mm}\) \(\mathrm{Hg}\), required to react with this volume of sea water.

Complete and balance the following equations. If no reaction occurs, write NR. (a) \(\mathrm{Cl}_{2}(g)+\mathrm{I}^{-}(a q) \longrightarrow\) (b) \(\mathrm{F}_{2}(g)+\mathrm{Br}^{-}(a q) \longrightarrow\) (c) \(\mathrm{I}_{2}(s)+\mathrm{Cl}^{-}(a q) \longrightarrow\) (d) \(\mathrm{Br}_{2}(l)+\mathrm{I}^{-}(a q) \longrightarrow\)
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