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Chapter 15: Problem 162

Why is the conjugate base of a weak acid like acetic acid often referred to as a salt of the acid?

Short Answer

Expert verified
The conjugate base of a weak acid, such as acetic acid (CH₃COOH), is referred to as a salt of the acid because it is a negatively charged anion (e.g., acetate ion, CH₃COO⁻) that can form a salt when it reacts with a positively charged cation. Salts are products of neutralization reactions between acids and bases. The acetate ion, as the conjugate base of acetic acid, is an essential component of the salt formed in the neutralization reaction, such as the formation of sodium acetate (CH₃COONa) when acetate ion reacts with sodium ion (Na⁺). This relationship between the conjugate base and the formation of salts is why it is often referred to as a salt of the acid.

Step by step solution

01

Understand Acetic Acid and Conjugate Base

Acetic acid (CH₃COOH) is a weak acid that can donate a proton (H⁺) to form its conjugate base. The conjugate base of acetic acid is formed by removing a proton (H⁺) from the acid. This results in Acetate ion (CH₃COO⁻). The process can be represented by the following chemical equation: CH₃COOH → CH₃COO⁻ + H⁺
02

Define Salts

A salt is an ionic compound formed from the neutralization reaction between an acid and a base. Salts typically consist of a positively charged cation and a negatively charged anion. In a complete neutralization reaction, the acid donates a proton to the base, which in turn results in the production of water and a salt. The general equation for this reaction is: Acid + Base → Salt + Water
03

Relate Conjugate Base and Salts

The conjugate base of a weak acid is a negatively charged anion that can form a salt when it reacts with a positively charged cation. For instance, in the case of acetic acid, its conjugate base is the acetate ion (CH₃COO⁻). When the acetate ion reacts with a positively charged cation, such as a sodium ion (Na⁺), it forms the salt sodium acetate (CH₃COONa). CH₃COO⁻ + Na⁺ → CH₃COONa The acetate ion (CH₃COO⁻), which is the conjugate base of acetic acid, is a fundamental component of the salt formed in the neutralization reaction. This is the reason why the conjugate base of weak acids like acetic acid is often referred to as salts of the acid.

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Most popular questions from this chapter

Ethanol, \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{OH}\), and hydride ion, \(\mathrm{H}^{-}\), react to produce \(\mathrm{H}_{2}\) gas and the \(\mathrm{C}_{2} \mathrm{H}_{5} \mathrm{O}^{-}\) anion. Arrhenius could not tell you what is going on, but Bronsted and Lowry would have no trouble. How would they explain this reaction?

An aqueous solution has an \(\mathrm{H}_{3} \mathrm{O}\) ' concentration of \(1.0 \mathrm{M}\). What is the OH concentration? Is this solution acidic or basic? Justify your answer.

What is the molar concentration of hydronium ion and hydroxide ion in pure water at \(25{ }^{\circ} \mathrm{C}\) ?

Without using a calculator, what is the base- 10 logarithm of \(10^{0}\) ? Of 1?

To be a weak base in water, a molecular compound must also be a weak electrolyte. What must be one of the ions it produces in water?
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