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Chapter 7: Problem 3

What is a conjugate acid? Conjugate base?

Short Answer

Expert verified
A conjugate acid is the species formed when a base gains a proton. A conjugate base is the species that remains after an acid donates a proton.

Step by step solution

01

Understand the Concept of Acids and Bases

In a chemical reaction, an acid donates a proton (H鈦�) and a base accepts a proton. This forms the foundation for understanding conjugate acids and bases.
02

Define Conjugate Acid

A conjugate acid is formed when a base accepts a proton. After the base gains a proton during the reaction, it becomes the conjugate acid of that base.
03

Define Conjugate Base

A conjugate base is what remains after an acid has donated a proton. Once the acid loses its proton, it becomes the conjugate base of that acid.

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Key Concepts

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

Conjugate Acid
When we talk about the concept of a conjugate acid in the context of acid-base chemistry, it's all about the transformation that occurs when a base accepts a proton. This can be thought of as a base gaining a small, positively charged particle - the proton (H鈦�). Once this happens, the result is a conjugate acid.
To visualize this, consider a base like ammonia (NH鈧�). If NH鈧� accepts a proton from an acid, it becomes NH鈧勨伜, which is its conjugate acid. This new structure, NH鈧勨伜, has one more hydrogen atom compared to the original base and a positive charge.
  • The base plus a proton equals its conjugate acid.
  • Always remember: base + H鈦� (proton) = conjugate acid.
Conjugate Base
The process of forming a conjugate base is the reverse of conjugate acid formation. When an acid donates a proton during a chemical reaction, what remains is called a conjugate base. Essentially, the acid loses a hydrogen ion, leaving behind its conjugate base.
Think of hydrochloric acid (HCl) as an example. When it donates a proton, what remains is Cl鈦�, the conjugate base. This ion is now ready to potentially accept a proton in a future reaction.
  • Acid minus a proton equals its conjugate base.
  • Remember: acid - H鈦� = conjugate base.
Proton Transfer
Proton transfer is a fundamental concept in acid-base reactions, showcasing the exchange of protons between substances. This transfer is central to understanding how acids and bases interact.
In any given acid-base reaction:
  • The acid will donate a proton to the base.
  • The base will accept this proton.
This proton exchange defines whether a substance acts as an acid or a base. Water, for instance, can both donate and accept protons, allowing it to act as either an acid or a base depending on the reaction context. Proton transfer is the heart of what makes acid-base chemistry dynamic.
Br酶nsted-Lowry Theory
The Br酶nsted-Lowry theory revolutionized our understanding of acids and bases by focusing on the movement of protons. According to this theory:
  • An acid is a proton donor.
  • A base is a proton acceptor.
This perspective emphasizes the role of protons in defining acidic and basic behavior.
One of the key strengths of the Br酶nsted-Lowry theory is its flexibility. It doesn't limit acids and bases to specific types of substances. Instead, it looks at the behavior of molecules during reactions and identifies them by their ability to donate or accept protons. This makes it a powerful tool for understanding a wide array of chemical reactions beyond traditional acidic and basic solutions.

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Most popular questions from this chapter

Calculate the \(\mathrm{pH}\) and \(\mathrm{pOH}\) of a solution obtained by mixing equal volumes of \(0.10 \mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4}\) and \(0.30 \mathrm{M} \mathrm{NaOH}\).

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

Calculate the \(\mathrm{pOH}\) of a blood sample whose \(\mathrm{pH}\) is 7.40 at \(37^{\circ} \mathrm{C} .\)

The \(\mathrm{pH}\) of a \(0.20 \mathrm{M}\) solution of a primary amine, \(\mathrm{RNH}_{2}\), is 8.42 . What is the \(\mathrm{p} K_{b}\) of the amine?

The first proton of sulfuric acid is completely ionized, but the second proton is onlv partially dissociated, with an acidity constant \(K_{a 2}\) of \(1.2 \times 10^{-2} .\) Calculate the hydrogen ion concentration in a \(0.0100 M \mathrm{H}_{2} \mathrm{SO}_{4}\) solution.
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