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Chapter 15: Problem 88

For each of the following, write the complete chemical equation for the acid- base reaction that occurs. Describe each using Br酶nsted language (if appropriate) and then using Lewis language (show electron-dot formulas). a The \(\mathrm{HS}^{-}\) ion reacts in water to produce \(\mathrm{H}_{2} \mathrm{~S}\). b) Cyanide ion, \(\mathrm{CN}^{-}\), reacts with \(\mathrm{Fe}^{3+}\)

Short Answer

Expert verified
a) \(\mathrm{HS}^{-} + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{H}_2\mathrm{S} + \mathrm{OH}^{-}\). b) \(6\mathrm{CN}^{-} + \mathrm{Fe}^{3+} \rightarrow \mathrm{[Fe(CN)_6]^{3-}}\).

Step by step solution

01

Identify Reactants and Products for Reaction a

In the reaction where \(\mathrm{HS}^{-}\) reacts with water to produce \(\mathrm{H}_{2}\mathrm{S}\), identify the reactants: \(\mathrm{HS}^{-}\) and \(\mathrm{H}_2\mathrm{O}\). The product is \(\mathrm{H}_{2}\mathrm{S}\). The other product formed in the reaction is \(\mathrm{OH}^{-}\).
02

Write the Chemical Equation for Reaction a

The balanced chemical reaction is: \[\mathrm{HS}^{-} + \mathrm{H}_2\mathrm{O} \rightarrow \mathrm{H}_2\mathrm{S} + \mathrm{OH}^{-}\] Here, \(\mathrm{HS}^{-}\) donates a hydrogen ion (acting as a Br酶nsted-Lowry acid) and \(\mathrm{H}_2\mathrm{O}\) accepts a hydrogen ion (acting as a Br酶nsted-Lowry base).
03

Describe Reaction a using Lewis Structures

\(\mathrm{HS}^{-}\) has a lone pair of electrons and is able to donate a pair to form a bond with \(\mathrm{H}^+\). \(\mathrm{H}_2\mathrm{O}\) has a lone pair of electrons, which it uses to form a bond with \(\mathrm{H}^+\), forming \(\mathrm{OH}^{-}\). The Lewis structures are shown: - \(\mathrm{HS}^-\): \(\cdot\cdot\mathrm{S}^-\) - \(\mathrm{H}_2\mathrm{S}:\) \(\mathrm{H}-\mathrm{S}\dot\dot\-\mathrm{H}\) - \(\mathrm{OH}^-\): \(\mathrm{O}\cdot\cdot\dot^-\) Lewis Acid/Base: \(\mathrm{HS}^{-}\) donates a pair making \(\mathrm{HS}^-\) Lewis acid, while \(\mathrm{H}_2\mathrm{O}\) accepts electrons as a base.
04

Identify Reactants and Products for Reaction b

For this reaction, \(\mathrm{CN}^{-}\), and \(\mathrm{Fe}^{3+}\) are the reactants. The reaction forms the complex ion \(\mathrm{[Fe(CN)_6]^{3-}}\) as the product.
05

Write the Chemical Equation for Reaction b

The balanced chemical reaction is: \[6\mathrm{CN}^{-} + \mathrm{Fe}^{3+} \rightarrow \mathrm{[Fe(CN)_6]^{3-}}\] Here, \(\mathrm{CN}^{-}\) acts as a ligand donating an electron pair to the central metal ion \(\mathrm{Fe}^{3+}\) acting as Lewis acid.
06

Describe Reaction b using Lewis Structures

\(\mathrm{CN}^{-}\) provides a lone pair of electrons from nitrogen (in \(\cdot\cdot C \equiv N^-\)) to the empty d-orbital of \(\mathrm{Fe}^{3+}\). The Lewis structures for the ligands and product: - \(\mathrm{CN}^{-}\): \(\cdot\cdot\mathrm{C}\equiv\mathrm{N}^-\) - \(\mathrm{Fe(CN)_6]^{3-}}:\) A central \(\mathrm{Fe}^{3+}\) ion with six \(\mathrm{CN}^{-}\) ligands surrounding it.

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Key Concepts

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

Br酶nsted-Lowry Theory
The Br酶nsted-Lowry Theory revolutionized our understanding of acid-base reactions by defining them through the transfer of protons. According to this theory, an acid is any substance that can donate a proton (\( ext{H}^+ \)), while a base is a substance that can accept a proton. In our example from the exercise, the reaction of \( ext{HS}^- \) with water demonstrates this concept beautifully.
When \( ext{HS}^- \) interacts with water, it donates a proton to water, forming \( ext{H}_2 ext{S} \) and hydroxide ion (\( ext{OH}^- \)). This demonstrates that \( ext{HS}^- \) acts as a Br酶nsted-Lowry acid, while water acts as a Br酶nsted-Lowry base.
  • Acids donate protons.
  • Bases accept protons.
Understanding these simple yet powerful definitions can help you break down even the most complex chemical equations into simpler interactions involving proton transfers.
Lewis Acid-Base Theory
The Lewis Acid-Base Theory broadens the concept of acids and bases beyond proton transfer by focusing on electron pairs instead. In this framework, an acid is a substance that can accept a pair of electrons, while a base is one that can donate a pair of electrons. This theory is particularly useful for explaining reactions that do not involve protons.
In the example of \( ext{CN}^- \) reacting with \( ext{Fe}^{3+} \), the cyanide ion (\( ext{CN}^- \)) acts as a Lewis base by donating a pair of electrons to the iron ion (\( ext{Fe}^{3+} \)), which acts as a Lewis acid.
  • Acids accept electron pairs.
  • Bases donate electron pairs.
Lewis structures offer visual insights into these reactions, depicting how electron pairs are shared or transferred, leading to the formation of complex ions or molecular compounds.
Chemical Equations
Chemical equations serve as the language of chemistry, depicting the reactants, products, and their relationships during a reaction. A balanced chemical equation reflects the conservation of mass, ensuring that the number of atoms for each element is equal on both sides of the equation.
In the given exercise, understanding the chemical equations is key. The reaction \( ext{HS}^- + ext{H}_2 ext{O} ightarrow ext{H}_2 ext{S} + ext{OH}^- \) and \( 6 ext{CN}^- + ext{Fe}^{3+} ightarrow [ ext{Fe(CN)}_6]^{3-} \) must be balanced to accurately reflect the reacting species and products.
  • Identify the reactants and products.
  • Ensure equations are balanced in terms of atoms and charge.
These equations are crucial to understanding the stoichiometry and energetics of reactions, providing a complete picture of the chemical processes.
Complex Ion Formation
Complex ion formation is an intriguing topic that involves the union of simple ions into a larger, complex ion, often involving transition metals. In these reactions, metal ions are typically at the center, surrounded by ligands that donate electron pairs to form coordinate covalent bonds.
Examining the reaction involving \( ext{CN}^- \) and \( ext{Fe}^{3+} \), six cyanide ions act as ligands, each donating a pair of electrons to the iron ion to form the complex ion \( [ ext{Fe(CN)}_6]^{3-} \).
  • Ligands are ions or molecules with lone pairs that form bonds with the central metal ion.
  • Complex ions exhibit unique properties, often influencing solubility and color.
These reactions demonstrate the versatility and richness of coordination chemistry, highlighting how simple ions can interact to form highly stable and intricate structures.

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Most popular questions from this chapter

Liquid ammonia undergoes autoionization similar to that of water: $$ \mathrm{NH}_{3}(l)+\mathrm{NH}_{3}(l) \rightleftharpoons \mathrm{NH}_{4}^{+}(l)+\mathrm{NH}_{2}^{-}(l) $$ How would you define an acid and a base similar to the way these terms are defined by the Br酶nsted-Lowry concept for aqueous solutions? Write the expression for the ionproduct constant, \(K_{a m},\) for this autoionization. The value of \(K_{a m}\) is \(5.1 \times 10^{-27}\). What is the concentration of \(\mathrm{NH}_{4}^{+}\) in a neutral solution of liquid ammonia? Suppose you dissolve \(\mathrm{NH}_{4} \mathrm{I}\) in liquid ammonia to give \(\mathrm{NH}_{4}{ }^{+}\) and \(\mathrm{I}^{-}\) ions. Similarly, you dissolve \(\mathrm{KNH}_{2}\) (potassium amide) in liquid ammonia to give a solution of \(\mathrm{K}^{+}\) and \(\mathrm{NH}_{2}^{-}\) ions. Which of these two solutions is acidic and which basic according to your definitions? Now, suppose you add the two solutions together. Write an equation for the neutralization reaction.

For the following reactions, label each species as an acid or a base. Indicate the species that are conjugates of one another. a) \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}+\mathrm{HCO}_{3}^{-} \rightleftharpoons \mathrm{HPO}_{4}^{2-}+\mathrm{H}_{2} \mathrm{CO}_{3}\) \(\mathrm{b)} \mathrm{F}^{-}+\mathrm{HSO}_{4}^{-} \rightleftharpoons \mathrm{HF}+\mathrm{SO}_{4}^{2-}\) c) \(\mathrm{HSO}_{4}^{-}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{SO}_{4}^{2-}+\mathrm{H}_{3} \mathrm{O}^{+}\) d) \(\mathrm{H}_{2} \mathrm{~S}+\mathrm{CN}^{-} \rightleftharpoons \mathrm{HS}^{-}+\mathrm{HCN}\)

The conjugate base of hydrofluoric acid dissolved in water is: a) \(\mathrm{F}^{-}\) b) \(\mathrm{OH}^{-}\) c) \(\mathrm{H}_{3} \mathrm{O}^{+}\) d) \(\mathrm{HF} \) e) \(\mathrm{F}_{2}\)

Write a reaction for each of the following in which the species acts as a Bronsted acid. The equilibrium should favor the product side. a) \(\mathrm{H}_{2} \mathrm{O}_{2}\) b \(\mathrm{HCO}_{3}^{-}\) c \(\mathrm{NH}_{4}^{+}\) d \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\)

A solution is \(0.030 \mathrm{M} \mathrm{HNO}_{3}\) (nitric acid). What is the hydronium-ion concentration at \(25^{\circ} \mathrm{C} ?\) What is the hydroxide-ion concentration at \(25^{\circ} \mathrm{C} ?\)
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