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Chapter 7: Problem 2

What is the Br贸nsted acid-base theory?

Short Answer

Expert verified
The Br枚nsted theory defines acids as proton donors and bases as proton acceptors.

Step by step solution

01

Introduction to Br枚nsted Acid-Base Theory

The Br枚nsted acid-base theory was proposed by Johannes Br枚nsted and Thomas Lowry in 1923. According to this theory, an acid is a proton donor, and a base is a proton acceptor.
02

Acid Definition

In the context of the Br枚nsted theory, an acid is defined as any substance that can donate a proton (\( H^+ \)) to another substance. For example, hydrochloric acid (\( HCl \)) in water donates a \( H^+ \) ion to water, forming \( H_3O^+ \) and \( Cl^- \).
03

Base Definition

A base, per Br枚nsted's theory, is any substance capable of accepting a proton (\( H^+ \)). For instance, in the reaction of ammonia (\( NH_3 \)) with water, ammonia accepts a proton from water, forming \( NH_4^+ \) and hydroxide ions (\( OH^- \)).
04

Example of an Acid-Base Reaction

Consider the reaction between hydrochloric acid and ammonia:\[ HCl + NH_3 \rightarrow NH_4^+ + Cl^- \]In this reaction, \( HCl \) acts as a Br枚nsted acid by donating a proton to \( NH_3 \), which acts as a Br枚nsted base accepting the proton to form \( NH_4^+ \).
05

Significance

The Br枚nsted theory expanded our understanding of acid-base reactions beyond aqueous solutions, allowing for the description of reactions where proton transfer occurs in non-aqueous solutions as well.

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Key Concepts

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

Proton Donor
In the Br枚nsted Acid-Base Theory, an acid is well-described as a proton donor. This means that any molecule or ion that can give away a hydrogen ion (proton, or \( H^+ \)) acts as an acid. Being a proton donor is at the heart of how acids behave in chemical reactions.
  • When an acid donates a proton, it transforms into its conjugate base.
  • Consider hydrochloric acid (\( HCl \)) in water. It donates a proton to water and converts into \( Cl^- \), its conjugate base.
A proton donor's ability to give away a proton typically depends on its strength and the nature of its chemical bonds. Acids vary in strength, with strong acids readily donating protons, while weak acids donate protons less easily. The concept of proton donation remains central to understanding not only simple chemical reactions but also more complex ones in non-aqueous environments.
Proton Acceptor
A proton acceptor, under the Br枚nsted Acid-Base Theory, is a base. This is any substance capable of receiving a proton from an acid. Being a proton acceptor involves forming a conjugate acid from a base when it accepts a proton.
  • Ammonia (\( NH_3 \)) is a classic example of a proton acceptor. When it encounters water, it accepts a proton, forming ammonium (\( NH_4^+ \)).
  • The hydroxide ion (\( OH^- \)) is another common proton acceptor, forming water when it accepts a proton.
Understanding bases as proton acceptors helps in recognizing how they neutralize acids and participate in various reactions, including those beyond aqueous solutions. This model is expansive enough to explain a wide variety of chemical interactions where proton transfer is involved.
Acid-Base Reactions
Acid-base reactions are integral to the Br枚nsted Theory, focusing on the transfer of protons from acids to bases. This transfer process is what defines an acid-base reaction.For instance:
  • In the reaction between hydrochloric acid (\( HCl \)) and ammonia (\( NH_3 \)), the acid, \( HCl \), donates a proton to \( NH_3 \) converting \( NH_3 \) into its conjugate acid, ammonia (\( NH_4^+ \)), and forming chloride ions (\( Cl^- \)).
  • Reactions where acids and bases neutralize each other, often forming water and salts, are typical examples.
These reactions happen in various environments, adjusting for the availability of proton donors and acceptors. Comprehending acid-base reactions allows us to predict and manipulate chemical behavior in both industrial processes and biological systems.
Non-aqueous Solutions
While Br枚nsted Acid-Base Theory is frequently discussed in the context of aqueous solutions, its reach extends into non-aqueous environments as well. Non-aqueous solutions involve solvents other than water, bringing new dynamics into how acids and bases interact. Here are some important points:
  • In non-aqueous solvents like benzene, or sulfur dioxide, the availability of protons for transfer can considerably impact reaction pathways.
  • Some reactions require non-aqueous conditions to maintain stability or enable a desired reaction pathway that doesn't occur well in water.
Considering non-aqueous environments helps in understanding complex chemical systems where traditional water-based models aren't applicable. Professionals often rely on these environments to optimize reactions and create products that are sensitive to water.

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Most popular questions from this chapter

Write the ionization reaction of aniline, \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{NH}_{2}\), in glacial acetic acid, and identify the conjugate acid of aniline. Write the ionization reaction of phenol. \(\mathrm{C}_{6} \mathrm{H}_{5} \mathrm{OH},\) in ethylene diamine, \(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2},\) and identify the conjugate base of phenol.

Calculate the \(\mathrm{pH}\) of a solution obtained by mixing equal volumes of a strong acid solution of \(\mathrm{pH} 3.00\) and a strong base solution of \(\mathrm{pH} 12.00\).

Calculate the \(\mathrm{pH}\) and \(\mathrm{pOH}\) of the following strong base solutions: (a) \(0.050 M\) \(\mathrm{NaOH},\) (b) \(0.14 \mathrm{MBa}(\mathrm{OH})_{2}\) (c) \(2.4 \mathrm{M} \mathrm{NaOH}\), (d) \(3.0 \times 10^{-7} M \mathrm{KOH}\) (e) \(3.7 \times\) \(10^{-3} M \mathrm{KOH}\).

Calculate the \(\mathrm{pH}\) of a solution that is \(0.050 \mathrm{M}\) in formic acid and \(0.10 \mathrm{M}\) in sodium formate.

Aspirin (acetylsalicylic acid) is absorbed from the stomach in the free (nonionized) acid form. If a patient takes an antacid that adiusts the \(\mathrm{nH}\) of the stomach contents to 2.95 and then takes two 5 -grain aspirin tablets (total \(0.65 \mathrm{~g}\) ) how many grams of aspirin are available for immediate absorption from the stomach, assuming immediate dissolution? Also assume that aspirin does not change the \(\mathrm{pH}\) of the stomach contents. The \(\mathrm{p} K_{\sigma}\) of aspirin is 3.50 . and its formula weight is 180.2
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