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Chapter 5: Problem 77

Balance these equations for reactions in acidic solution. (a) $\mathrm{IBr}+\mathrm{BrO}_{3}^{-}+\mathrm{H}^{+} \longrightarrow \mathrm{IO}_{3}^{-}+\mathrm{Br}^{-}+\mathrm{H}_{2} \mathrm{O}$ (b) $\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{NO}_{3}+\mathrm{Sn} \longrightarrow$ $\mathrm{NH}_{2} \mathrm{OH}+\mathrm{CH}_{3} \mathrm{CH}_{2} \mathrm{OH}+\mathrm{Sn}^{2+}$ (c) $\mathrm{As}_{2} \mathrm{S}_{3}+\mathrm{NO}_{3}^{-} \longrightarrow \mathrm{H}_{3} \mathrm{AsO}_{4}+\mathrm{S}+\mathrm{NO}$ (d) $\mathrm{H}_{5} \mathrm{IO}_{6}+\mathrm{I}_{2} \longrightarrow \mathrm{IO}_{3}^{-}+\mathrm{H}^{+}+\mathrm{H}_{2} \mathrm{O}$ (e) $\mathrm{S}_{2} \mathrm{F}_{2}+\mathrm{H}_{2} \mathrm{O} \longrightarrow \mathrm{S}_{8}+\mathrm{H}_{2} \mathrm{S}_{4} \mathrm{O}_{6}+\mathrm{HF}$

Short Answer

Expert verified
Balanced equations: (a) \(2IBr + BrO_{3}^{-} + 6H^{+} \rightarrow 2IO_{3}^{-} + 5Br^{-} + 3H_{2}O\); (b) \(2CH_{3}CH_{2}NO_{3} + 2Sn \rightarrow 2NH_{2}OH + 2CH_{3}CH_{2}OH + 2Sn^{2+}\); (c) \(2As_{2}S_{3} + 13NO_{3}^{-} + 16H^{+} \rightarrow 2H_{3}AsO_{4} + 8S + 3NO + 10H_{2}O\); (d) \(H_{5}IO_{6} + 5I_{2} + 6H^{+} \rightarrow 6IO_{3}^{-} + 3H_{2}O\); (e) \(16S_{2}F_{2} + 48H_{2}O \rightarrow 8S_{8} + 16H_{2}S_{4}O_{6} + 32HF\).

Step by step solution

01

Determine oxidation states

Identify the oxidation states of the atoms in the reactants and products.
02

Write down the half-reactions

The atoms that change the oxidation states are participating in the redox reaction. Write down the two half-reactions, one for oxidation and one for reduction.
03

Balance the half-reactions

Using the mass balance, ensure that each atom appears the same number of times on both sides of the equation. To balance the charges, add protons \(H^{+}\) to the side that needs positive charges or add water molecules \(H_{2}O\) to provide the required amount of oxygen atoms, and if needed, add water molecules to the other side of the equation to compensate for the excess of hydrogen atoms generated.
04

Combine the half-reactions

Combine the two half-reactions into one equation, ensuring that the electrons are balanced. Multiply the reactions if necessary until the number of electrons on both sides is the same. Make sure to cancel out the same substances on both sides of the equation whenever possible.
05

Verify the balance

Check the complete balanced equation to ensure each atom and the overall charge are balanced.

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Most popular questions from this chapter

In this chapter, we described an acid as a substance capable of producing \(\mathrm{H}^{+}\) and a salt as the ionic compound formed by the neutralization of an acid by a base. Write ionic equations to show that sodium hydrogen sulfate has the characteristics of both a salt and an acid (sometimes called an acid salt).

In the half-reaction in which \(\mathrm{NpO}_{2}^{+}\) is converted to \(\mathrm{Np}^{4+},\) the number of electrons appearing in the half-equation is (a) \(1 ;(b) 2 ;(c) 3 ;\) (d) 4.

A \(110.520 \mathrm{g}\) sample of mineral water is analyzed for its magnesium content. The \(\mathrm{Mg}^{2+}\) in the sample is first precipitated as \(\mathrm{MgNH}_{4} \mathrm{PO}_{4},\) and this precipitate is then converted to \(\mathrm{Mg}_{2} \mathrm{P}_{2} \mathrm{O}_{7},\) which is found to weigh 0.0549 g. Express the quantity of magnesium in the sample in parts per million (that is, in grams of \(\mathrm{Mg}\) per million grams of \(\mathrm{H}_{2} \mathrm{O}\) ).

Write a balanced equation for the redox reactions. (a) The reaction of aluminum metal with hydroiodic acid. (b) The reduction of vanadyl ion ( \(\mathrm{VO}^{2+}\) ) to vanadic ion \(\left(\mathrm{V}^{3+}\right)\) in acidic solution with zinc metal as the reducing agent. (c) The oxidation of methanol by chlorate ion in acidic solution, producing carbon dioxide gas, water, and chlorine dioxide gas as products.

A piece of marble (assume it is pure \(\mathrm{CaCO}_{3}\) ) reacts with \(2.00 \mathrm{L}\) of \(2.52 \mathrm{M} \mathrm{HCl}\). After dissolution of the marble, a \(10.00 \mathrm{mL}\) sample of the resulting solution is withdrawn, added to some water, and titrated with 24.87 mL of 0.9987 M NaOH. What must have been the mass of the piece of marble? Comment on the precision of this method; that is, how many significant figures are justified in the result?
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