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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鈦�) and hydrazine (N鈧侶鈧�) forms ammonia (NH鈧�), which then reacts with chloride ions (Cl鈦�) 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鈦� is greater than that of the reaction involving N鈧侶鈧�, the ClO鈦� half-reaction is the reduction (gain of electrons), and the N鈧侶鈧� 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鈦� half-reaction accepts 2 electrons, and the N鈧侶鈧� 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 (NH鈧�). 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.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Household Chemicals
Household chemicals are common substances found in nearly every home. These chemicals range from cleaning agents like bleach and ammonia to personal care products and garden fertilizers. But just because they're commonly used, doesn't mean they're always safe. It鈥檚 crucial to understand their properties and how they interact with each other.
  • Bleach (Sodium Hypochlorite): A powerful disinfectant and stain remover, bleach is highly alkaline and known for its ability to whiten and sanitize.
  • Ammonia: Commonly found in glass cleaners, ammonia is a strong cleaner for surfaces without leaving streaks. It effectively removes grease and grime.
While each chemical has useful individual applications, it's essential to use them with caution and knowledge to avoid risky combinations.
Bleach and Ammonia Reaction
Mixing bleach with ammonia, although might seem like an effective cleaning duo, is unfortunately a recipe for danger. When these two are combined, they undergo a chemical reaction that releases harmful gases. This reaction is a classic example of a redox reaction, where electrons are transferred between molecules. In simpler terms, bleach, which acts as an oxidizing agent, reacts with ammonia forming chloramine gas and potentially hydrazine (N鈧侶鈧�), both hazardous substances.
  • Bleach reacts with ammonia to produce chloramine gases.
  • In less common scenarios, a more dangerous chemical, hydrazine, could form. Hydrazine is a very toxic compound.
Understanding this reaction is crucial to prevent accidents and health hazards at home. Always handle these chemicals separately.
Chemical Safety
Safety with household chemicals can prevent accidents and health issues. Here are some vital tips for using chemicals like bleach and ammonia:
  • Always read the labels and instructions before use.
  • Avoid mixing cleaning products unless it's confirmed safe.
  • Use personal protective equipment like gloves and masks, especially when using strong chemicals.
  • Ensure good ventilation when using substances that produce fumes.
Educating yourself about chemical safety reduces risks of exposure to toxic substances. Simple precautions can go a long way in safeguarding your health and that of others around you.
Chloramine Gas
Chloramine gas is produced when bleach is mixed with ammonia. It appears in various forms, such as monochloramine (NH鈧侰l), and is well noted for its distinctive and irritating odor. Exposure to chloramine can cause:
  • Respiratory distress
  • Throat irritation
  • Skin and eye irritation
The symptoms can be more severe with increased exposure and inhalation. Always take caution to ensure that these chemicals do not come into contact, as chloramine gas can accumulate quickly and be harmful even at low concentrations. By understanding the risk associated with chloramine, one can effectively avoid creating dangerous environments, particularly in closed spaces like bathrooms.

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Most popular questions from this chapter

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 \(1+\).

It takes \(15 \mathrm{kWh}\) (kilowatt-hours) of electrical energy to produce 1.0 kg aluminum metal from aluminum oxide by the HallHeroult process. Compare this to the amount of energy necessary to melt \(1.0 \mathrm{~kg}\) aluminum metal. Why is it economically feasible to recycle aluminum cans?

Given the following two standard reduction potentials, $$\mathrm{M}^{3+}+3 \mathrm{e}^{-} \longrightarrow \mathrm{M} \quad \mathscr{E}^{\circ}=-0.10 \mathrm{~V}$$ $$\mathrm{M}^{2+}+2 \mathrm{e}^{-} \longrightarrow \mathrm{M} \quad \mathscr{E}^{\circ}=-0.50 \mathrm{~V}$$ solve for the standard reduction potential of the half- reaction$$\mathrm{M}^{3+}+\mathrm{e}^{-} \longrightarrow \mathrm{M}^{2+}$$

When copper reacts with nitric acid, a mixture of \(\mathrm{NO}(\mathrm{g})\) and \(\mathrm{NO}_{2}(g)\) is evolved. The volume ratio of the two product gases depends on the concentration of the nitric acid according to the equilibrium \(2 \mathrm{H}^{+}(a q)+2 \mathrm{NO}_{3}^{-}(a q)+\mathrm{NO}(g) \rightleftharpoons 3 \mathrm{NO}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l)\) Consider the following standard reduction potentials at \(25^{\circ} \mathrm{C}\) : \(3 \mathrm{e}^{-}+4 \mathrm{H}^{+}(a q)+\mathrm{NO}_{3}^{-}(a q) \longrightarrow \mathrm{NO}(g)+2 \mathrm{H}_{2} \mathrm{O}(l)\) $$\begin{array}{r}\mathscr{E}^{\circ}=0.957 \mathrm{~V}\end{array}$$ \(\mathrm{e}^{-}+2 \mathrm{H}^{+}(a q)+\mathrm{NO}_{3}^{-}(a q) \longrightarrow \mathrm{NO}_{2}(g)+2 \mathrm{H}_{2} \mathrm{O}(l)\) $${8}^{\circ}=0.775 \mathrm{~V}$$ a. Calculate the equilibrium constant for the above reaction. b. What concentration of nitric acid will produce a NO and \(\mathrm{NO}_{2}\) mixture with only \(0.20 \% \mathrm{NO}_{2}\) (by moles) at \(25^{\circ} \mathrm{C}\) and \(1.00 \mathrm{~atm}\) ? Assume that no other gases are present and that the change in acid concentration can be neglected.

How can one construct a galvanic cell from two substances, each having a negative standard reduction potential?
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