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Chapter 15: Problem 6

Describe four ways in which the Br酶nsted-Lowry concept expands on the Arrhenius concept.

Short Answer

Expert verified
The Br酶nsted-Lowry concept expands on the Arrhenius concept by including non-aqueous environments, allowing neutral molecules as bases, encompassing more reactions with proton transfer, and introducing conjugate acid-base pairs.

Step by step solution

01

Definition of Arrhenius Concept

The Arrhenius concept defines acids as substances that ionize in water to produce hydrogen ions (H鈦�), and bases as substances that ionize in water to produce hydroxide ions (OH鈦�). It is limited to aqueous solutions.
02

Introduction to Br酶nsted-Lowry Concept

The Br酶nsted-Lowry concept broadens the definition of acids and bases beyond aqueous solutions. An acid is defined as a proton donor, while a base is a proton acceptor, allowing for the inclusion of reactions not occurring in water.
03

Protons Not Restricted to H鈦� in Water

Unlike the Arrhenius concept, where acids are specifically linked to H鈦� in water, the Br酶nsted-Lowry theory allows acids and bases to interact in any solvent or phase, even in the absence of water.
04

Neutral Molecules and Ions as Bases

The Br酶nsted-Lowry concept allows for neutral molecules, such as NH鈧�, or ions, such as Cl鈦�, to act as bases by accepting protons, whereas Arrhenius bases are strictly compounds that dissociate in water to produce OH鈦�.
05

Inclusion of Non-Aqueous Acid-Base Reactions

By considering any proton transfer between molecules, Br酶nsted-Lowry encompasses reactions that occur in gases, non-aqueous solvents, or solids, further broadening the scope from the aqueous-only Arrhenius framework.
06

Conjugate Acid-Base Pairs

Br酶nsted-Lowry introduces the idea of conjugate acid-base pairs, where the removal of a proton from an acid forms a base, and the addition of a proton to a base forms an acid, conceptually deepening understanding beyond Arrhenius.

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Key Concepts

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

Arrhenius Concept
The Arrhenius concept is one of the earliest theories to define acids and bases. According to this model, an acid is a substance that, when dissolved in water, increases the concentration of hydrogen ions (\( H^+ \)). Similarly, a base is defined as a substance that produces hydroxide ions (\( OH^- \)) in water. This concept is restricted to aqueous solutions, meaning it only considers reactions that take place in water. As helpful as the Arrhenius concept was in its time, it has limitations because it doesn't accommodate reactions that occur outside of water or those involving substances that don't release \( OH^- \) or \( H^+ \) directly in an aqueous environment.
Proton Donor and Acceptor
The Br酶nsted-Lowry theory expanded the definition of acids and bases beyond the aqueous limitations of the Arrhenius concept. In this model, acids are considered proton donors, meaning they can give up protons (hydrogen ions \( H^+ \)) in a chemical reaction. Conversely, bases are proton acceptors, which means they can accept these protons during the reaction. This comprehensive approach allows for understanding reactions in a variety of environments beyond just water
  • Includes gases and non-aqueous solutions
  • Recognizes a broader range of acid-base interactions
This more inclusive definition is pivotal for exploring chemical reactions in complex systems, such as biological processes that occur in non-aqueous environments like cell membranes.
Conjugate Acid-Base Pairs
An insightful addition by the Br酶nsted-Lowry model is the concept of conjugate acid-base pairs. When an acid donates a proton, it transforms into its conjugate base, while the base that accepts a proton forms its conjugate acid. This idea provides a flow of interaction and transformation, offering a dynamic view into acid-base chemistry.
  • Example: When hydrochloric acid (\( HCl \)) gives up a proton, it becomes chloride (\( Cl^- \)), its conjugate base.
  • Conversely, when ammonia (\( NH_3 \)) accepts a proton, it forms ammonium (\( NH_4^+ \)), its conjugate acid.
This concept helps students understand acid-base chemistry as an equilibrium process, where acids and bases continuously interact and transform within the reaction environment.
Non-Aqueous Reactions
The Br酶nsted-Lowry theory's ability to explain reactions beyond aqueous solutions represents one of its significant strengths. By considering proton transfer in non-aqueous environments, the model encompasses reactions in any phase鈥攂e it gas, liquid, or solid. This flexibility is instrumental for understanding reactions in various chemical processes and industrial applications.
  • Reactions in gases: For instance, in the atmosphere, reactions can involve proton transfers that aren't reliant on water
  • Industrial and laboratory settings where non-aqueous solvents are used
  • Solid-state reactions, observable in advanced material science
This broader scope makes the Br酶nsted-Lowry theory a versatile tool for chemists exploring diverse reactions in many scientific fields beyond basic aqueous chemistry.

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Most popular questions from this chapter

Pure liquid hydrogen fluoride ionizes in a way similar to that of water. a)Write the equilibrium reaction for the auto-ionization of liquid hydrogen fluoride. b) Will sodium fluoride be an acid or a base in liquid hydrogen fluoride? Why? c) Perchloric acid is a strong acid in liquid hydrogen fluoride. Write the chemical equation for the ionization reaction. What is the conjugate acid in this medium?

A detergent solution has a pH of 11.80 at \(25^{\circ} \mathrm{C}\). What is the hydroxide-ion concentration?

Obtain the pH corresponding to the following hydronium-ion concentrations. a) \(1.0 \times 10^{-8} M\) b) \(5.0 \times 10^{-12} M\) c) \(7.5 \times 10^{-3} M\) d) \(6.35 \times 10^{-9} M\)

You make a solution by dissolving \(0.0010 \mathrm{~mol}\) of \(\mathrm{HCl}\) in enough water to make \(1.0 \mathrm{~L}\) of solution. a) Write the chemical equation for the reaction of \(\mathrm{HCl}(a q)\) and water. b) Without performing calculations, give a rough estimate of the \(\mathrm{pH}\) of the \(\mathrm{HCl}\) solution. Justify your answer. c) Calculate the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration and the \(\mathrm{pH}\) of the solution. d) Is there any concentration of the base \(\mathrm{OH}^{-}\) present in this solution of \(\mathrm{HCl}(a q)\) ? If so, where did it come from? e) If you increase the \(\mathrm{OH}^{-}\) concentration of the solution by adding \(\mathrm{NaOH}\), does the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration change? If you think it does, explain why this change occurs and whether the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration increases or decreases.

Order each of the following pairs by acid strength, giving the weaker acid first. Explain your answer. a \(\mathrm{HNO}_{3}, \mathrm{HNO}_{2}\) \(\mathrm{b} \mathrm{HCO}_{3}^{-}, \mathrm{H}_{2} \mathrm{CO}_{3}\) c \(\mathrm{H}_{2} \mathrm{~S}, \mathrm{H}_{2} \mathrm{Te}\) d \(\mathrm{HCl}, \mathrm{H}_{2} \mathrm{~S}\) e \(\mathrm{H}_{3} \mathrm{PO}_{4}, \mathrm{H}_{3} \mathrm{AsO}_{4}\)
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