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Chapter 22: Problem 127

Write a plausible chemical equation to represent the reaction of \((\mathrm{a}) \mathrm{Cl}_{2}(\mathrm{g}) \quad\) with cold \(\quad \mathrm{NaOH}(\mathrm{aq})\) (b) \(\mathrm{NaI}(\mathrm{s})\) with hot \(\mathrm{H}_{2} \mathrm{SO}_{4}(\text { concd aq }) ;\) (c) \(\mathrm{Cl}_{2}(\mathrm{g})\) with \(\mathrm{KI}_{3}(\mathrm{aq}) ; \quad\) (d) \(\quad \mathrm{NaBr}(\mathrm{s}) \quad\) with hot \(\mathrm{H}_{3} \mathrm{PO}_{4}\) \((\text { concd aq })\) (e) \(\mathrm{NaHSO}_{3}(\mathrm{aq})\) with \(\mathrm{MnO}_{4}^{-1}(\mathrm{aq})\) in dilute \(\mathrm{H}_{2} \mathrm{SO}_{4}(\mathrm{aq})\).

Short Answer

Expert verified
The equations representing the reactions are:\n1) \( \mathrm{Cl}_{2} + 2 \mathrm{NaOH} \to \mathrm{NaClO} + \mathrm{NaCl} + \mathrm{H}_{2} \mathrm{O} \); \n\n2) \( \mathrm{NaI} + \mathrm{H}_{2} \mathrm{SO}_{4} \to \mathrm{HI} + \mathrm{NaHSO}_{4} \); \n\n3) \( \mathrm{Cl}_{2} + 2 \mathrm{KI}_{3} \to 2 \mathrm{I}_{2} + 2 \mathrm{KCl} \); \n\n4) \( \mathrm{NaBr} + \mathrm{H}_{3} \mathrm{PO}_{4} \to \mathrm{HBr} + \mathrm{NaH}_{2} \mathrm{PO}_{4} \); \n\n5) \( 2 \mathrm{MnO}_{4}^{-1} + 5 \mathrm{NaHSO}_{3} + 3 \mathrm{H}_{2} \mathrm{SO}_{4} \to 2 \mathrm{MnSO}_4 + 5 \mathrm{NaHSO}_4 + 3 \mathrm{H}_2 \mathrm{O} \)

Step by step solution

01

Reaction of \( \mathrm{Cl}_{2}(\mathrm{g}) \) with \( \mathrm{NaOH}(\mathrm{aq}) \)

Chlorine reacts with cold aqueous sodium hydroxide to produce bleach or sodium hypochlorite and sodium chloride. The chemical equation is: \[ \mathrm{Cl}_{2} + 2 \mathrm{NaOH} \to \mathrm{NaClO} + \mathrm{NaCl} + \mathrm{H}_{2}\mathrm{O} \]
02

Reaction of \( \mathrm{NaI}(\mathrm{s}) \) with hot \( \mathrm{H}_{2}\mathrm{SO}_{4}(\mathrm{aq}) \)

Sodium iodide reacts with hot concentrated sulfuric acid to produce hydrogen iodide and sodium hydrogen sulphate. The chemical equation is: \[ \mathrm{NaI} + \mathrm{H}_{2}\mathrm{SO}_{4} \to \mathrm{HI} + \mathrm{NaHSO}_{4} \]
03

Reaction of \( \mathrm{Cl}_{2}(\mathrm{g}) \) with \( \mathrm{KI}_{3}(\mathrm{aq}) \)

Chlorine gas reacts with potassium iodide to produce iodine and potassium chloride. The chemical equation is: \[ \mathrm{Cl}_{2} + 2 \mathrm{KI}_{3} \to 2 \mathrm{I}_{2} + 2\mathrm{KCl} \]
04

Reaction of \( \mathrm{NaBr}(\mathrm{s}) \) with hot \( \mathrm{H}_{3}\mathrm{PO}_{4}(\mathrm{aq}) \)

Sodium bromide reacts with hot concentrated phosphoric acid to produce hydrogen bromide and sodium hydrogen phosphate. The chemical equation is: \[ \mathrm{NaBr} + \mathrm{H}_{3}\mathrm{PO}_{4} \to \mathrm{HBr} + \mathrm{NaH}_{2}\mathrm{PO}_{4} \]
05

Reaction of \( \mathrm{NaHSO}_{3}(\mathrm{aq}) \) with \( \mathrm{MnO}_{4}^{-1}(\mathrm{aq}) \) in dilute \( \mathrm{H}_{2}\mathrm{SO}_{4}(\mathrm{aq}) \)

Sodium hydrogen sulphite reacts with permanganate ion in dilute sulfuric acid to produce manganese sulphate, sodium sulphate and water. The chemical equation is: \[ 2 \mathrm{MnO}_{4}^{-1} + 5 \mathrm{NaHSO}_{3} + 3 \mathrm{H}_{2}\mathrm{SO}_{4} \to 2 \mathrm{MnSO}_{4} + 5 \mathrm{NaHSO}_{4} + 3 \mathrm{H}_{2} \mathrm{O} \]

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Most popular questions from this chapter

The oxides of the phosphorus(III), antimony(III), and bismuth(III) are \(\mathrm{P}_{4} \mathrm{O}_{6}, \mathrm{Sb}_{4} \mathrm{O}_{6},\) and \(\mathrm{Bi}_{2} \mathrm{O}_{3} .\) Only one of these oxides is amphoteric. Which one? Which of these oxides is most acidic? Which is most basic?

Write balanced equations for the following important commercial reactions involving nitrogen and its compounds. (a) the principal artificial method of fixing atmospheric \(\mathrm{N}_{2}\) (b) oxidation of ammonia to \(\mathrm{NO}\) (c) preparation of nitric acid from \(\mathrm{NO}\).

The boiling points of oxygen and argon are \(-183^{\circ} \mathrm{C}\) and \(-189^{\circ} \mathrm{C},\) respectively. Because the boiling points are so similar, argon obtained from the fractional distillation of liquid air is contaminated with oxygen. The following three-step procedure can be used to obtain pure argon from the oxygen-contaminated sample: (1) Excess hydrogen is added to the mixture and then the mixture is ignited. (2) The mixture from step (1) is then passed over hot copper(II) oxide. (3) The mixture from step (2) is passed over a dehydrated zeolite material (see Chapter 21 ). Explain the purpose of each step, writing chemical equations for any reactions that occur.

All of the following have a tetrahedral shape except (a) \(\mathrm{SO}_{4}^{2-} ;\) (b) \(\mathrm{XeF}_{4} ;\) (c) \(\mathrm{CCl}_{4} ;\) (d) \(\mathrm{XeO}_{4} ;\) (e) \(\mathrm{NH}_{4}^{+}\)..

In \(1988,\) G. J. Schrobilgen, professor of chemistry at McMaster University in Canada, reported the synthesis of an ionic compound, \([\mathrm{HCNKrF}]\left[\mathrm{AsF}_{6}\right],\) which consists of \(\mathrm{HCNKr} \mathrm{F}^{+}\) and \(\mathrm{AsF}_{6}^{-}\) ions. In the \(\mathrm{HCNKr} \mathrm{F}^{+}\) ion, the krypton is covalently bonded to both fluorine and nitrogen. Draw Lewis structures for these ions, and estimate the bond angles.
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