Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 18: Problem 61

Hydrazine is somewhat toxic. Use the half-reactions shown below to explain why household bleach (a highly alkaline solution of sodium hypochlorite) should not be mixed with household ammonia or glass cleansers that contain ammonia. \(\mathrm{ClO}^{-}+\mathrm{H}_{2} \mathrm{O}+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{OH}^{-}+\mathrm{Cl}^{-} \quad \mathscr{E}^{\circ}=0.90 \mathrm{~V}\) \(\mathrm{N}_{2} \mathrm{H}_{4}+2 \mathrm{H}_{2} \mathrm{O}+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{NH}_{3}+2 \mathrm{OH}^{-} \quad \mathscr{E}^{\circ}=-0.10 \mathrm{~V}\)

Short Answer

Expert verified
Mixing bleach with ammonia or glass cleansers containing ammonia leads to the formation of toxic chloramine gas. This is because the redox reaction between bleach (containing sodium hypochlorite, ClO⁻) and hydrazine (N₂H₄) forms ammonia (NH₃), which then reacts with chloride ions (Cl⁻) to produce chloramine: \(\mathrm{ClO}^{-}+\mathrm{N}_{2} \mathrm{H}_{4}+3 \mathrm{H}_{2} \mathrm{O} \longrightarrow\mathrm{Cl}^{-}+2 \mathrm{NH}_{3}+4 \mathrm{OH}^{-}\) \(\mathrm{NH}_{3}+\mathrm{Cl}^{-} \longrightarrow \mathrm{NH}_{2} \mathrm{Cl}+(\mathrm{H}^{+}+ \mathrm{e}^{-})\) Chloramine can cause respiratory problems, throat irritation, and other health issues.

Step by step solution

01

Determine the overall spontaneous redox reaction

To find the overall redox reaction, we must combine the two half-cell reactions. Because the reduction potential of the reaction involving ClO⁻ is greater than that of the reaction involving N₂H₄, the ClO⁻ half-reaction is the reduction (gain of electrons), and the N₂H₄ half-reaction is the oxidation (loss of electrons).
02

Balance the half-reactions

We need to balance the electrons in each half-reaction. The ClO⁻ half-reaction accepts 2 electrons, and the N₂H₄ half-reaction loses 2 electrons: Reduction: \(\mathrm{ClO}^{-}+\mathrm{H}_{2} \mathrm{O}+2 \mathrm{e}^{-} \longrightarrow 2 \mathrm{OH}^{-}+\mathrm{Cl}^{-}\) Oxidation: \(\mathrm{N}_{2} \mathrm{H}_{4}+2 \mathrm{H}_{2} \mathrm{O} \rightarrow 2 \mathrm{NH}_{3}+2 \mathrm{OH}^{-} + 2\mathrm{e}^{-}\)
03

Combine the half-reactions

Now, we can combine the half-reactions to find the overall redox reaction. Cancelling out the electrons, we get: \(\mathrm{ClO}^{-}+\mathrm{H}_{2} \mathrm{O}+\mathrm{N}_{2} \mathrm{H}_{4}+2 \mathrm{H}_{2} \mathrm{O} \longrightarrow 2 \mathrm{OH}^{-}+\mathrm{Cl}^{-}+2 \mathrm{NH}_{3}+2 \mathrm{OH}^{-}\) Simplify by combining like terms: \(\mathrm{ClO}^{-}+\mathrm{N}_{2} \mathrm{H}_{4}+3 \mathrm{H}_{2} \mathrm{O} \longrightarrow\mathrm{Cl}^{-}+2 \mathrm{NH}_{3}+4 \mathrm{OH}^{-}\)
04

Explain the danger of the reaction

The important part of the overall redox reaction is the formation of ammonia (NH₃). When bleach, containing sodium hypochlorite, is mixed with ammonia or glass cleansers containing ammonia, a toxic gas called chloramine is produced: \(\mathrm{NH}_{3}+\mathrm{Cl}^{-} \longrightarrow \mathrm{NH}_{2} \mathrm{Cl}+(\mathrm{H}^{+}+ \mathrm{e}^{-})\) Chloramine is a harmful gas that can cause respiratory problems, throat irritation, and other health issues. This is why household bleach should not be mixed with ammonia or glass cleansers containing ammonia.

Unlock Step-by-Step Solutions & Ace Your Exams!

  • Full Textbook Solutions

    Get detailed explanations and key concepts

  • Unlimited Al creation

    Al flashcards, explanations, exams and more...

  • Ads-free access

    To over 500 millions flashcards

  • Money-back guarantee

    We refund you if you fail your exam.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Sketch the galvanic cells based on the following half-reactions. Show the direction of electron flow, show the direction of ion migration through the salt bridge, and identify the cathode and anode. Give the overall balanced equation, and determine \(\mathscr{E}^{\circ}\) for the galvanic cells. Assume that all concentrations are \(1.0 M\) and that all partial pressures are \(1.0 \mathrm{~atm}\). a. \(\mathrm{Cl}_{2}+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{Cl}^{-} \quad \mathscr{E}^{\circ}=1.36 \mathrm{~V}\) \(\mathrm{Br}_{2}+2 \mathrm{e}^{-} \rightarrow 2 \mathrm{Br}^{-} \quad 8^{\circ}=1.09 \mathrm{~V}\) b. \(\mathrm{MnO}_{4}^{-}+8 \mathrm{H}^{+}+5 \mathrm{e}^{-} \rightarrow \mathrm{Mn}^{2+}+4 \mathrm{H}_{2} \mathrm{O}\) \(\mathscr{b}^{\circ}=1.51 \mathrm{~V}\) \(\mathrm{IO}_{4}^{-}+2 \mathrm{H}^{+}+2 \mathrm{e}^{-} \rightarrow \mathrm{IO}_{3}^{-}+\mathrm{H}_{2} \mathrm{O} \quad \mathscr{E ^ { \circ }}=1.60 \mathrm{~V}\)

What volumes of \(\mathrm{H}_{2}(g)\) and \(\mathrm{O}_{2}(g)\) at STP are produced from the electrolysis of water by a current of \(2.50 \mathrm{~A}\) in \(15.0 \mathrm{~min} ?\)

You are told that metal \(\mathrm{A}\) is a better reducing agent than metal \(\mathrm{B}\). What, if anything, can be said about \(\mathrm{A}^{+}\) and \(\mathrm{B}^{+}\) ? Explain.

It took \(150 . \mathrm{s}\) for a current of \(1.25 \mathrm{~A}\) to plate out \(0.109 \mathrm{~g}\) of \(\mathrm{a}\) metal from a solution containing its cations. Show that it is not possible for the cations to have a charge of \(1+\).

Gold metal will not dissolve in either concentrated nitric acid on concentrated hydrochloric acid. It will dissolve, however, in aqua regia, a mixture of the two concentrated acids. The products of the reaction are the \(\mathrm{AuCl}_{4}^{-}\) ion and gaseous NO. Write a balanced equation for the dissolution of gold in aqua regia.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Chemical Analysis

Read Explanation

Inorganic Chemistry

Read Explanation

Making Measurements

Read Explanation

Physical Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free