91Ó°ÊÓ

The following equilibrium is established when hydrogen chloride is dissolved in acetic acid. \(\mathrm{HCl}+\mathrm{CH}_{3} \mathrm{COOH} \leftrightarrow \mathrm{Cl}^{-}+\mathrm{CH}_{3} \mathrm{COOH}_{2}^{+}\) The set that characterizes the conjugate acid base pair is a. \(\left(\mathrm{HCl}, \mathrm{CH}_{3} \mathrm{COOH}\right)\) and \(\left(\mathrm{CH}_{3} \mathrm{COOH}_{2}^{+}, \mathrm{Cl}^{-}\right)\) b. \(\left(\mathrm{HCl}, \mathrm{CH}_{3} \mathrm{COOH}_{2}^{+}\right)\)and \(\left(\mathrm{HCl}, \mathrm{CH}_{3} \mathrm{COOH}_{2}^{+}\right)\) and \(\left(\mathrm{CH}_{3} \mathrm{COOH}, \mathrm{Cl}^{2}\right)\) c. \(\left(\mathrm{CH}_{3} \mathrm{COOH}_{2}^{*}, \mathrm{HCl}\right)\) and \(\left(\mathrm{Cl}^{-}, \mathrm{CH}_{3} \mathrm{COOH}\right)\) d. \(\left(\mathrm{HCl}, \mathrm{Cl}^{-}\right)\)and \(\left(\mathrm{CH}_{3} \mathrm{COOH}_{2}^{+}, \mathrm{CH}_{3} \mathrm{COOH}\right)\)

Step by step solution

01

Identify the Bronsted-Lowry Acid and Base

In the given reaction \( \mathrm{HCl} + \mathrm{CH}_3 \mathrm{COOH} \leftrightarrow \mathrm{Cl}^- + \mathrm{CH}_3 \mathrm{COOH}_2^+ \), \( \mathrm{HCl} \) donates a proton and becomes \( \mathrm{Cl}^- \), making it the acid. \( \mathrm{CH}_3 \mathrm{COOH} \) accepts a proton to become \( \mathrm{CH}_3 \mathrm{COOH}_2^+ \), making it the base.

02

Define Conjugate Pairs

A conjugate acid-base pair consists of two species that transform into each other by the gain or loss of a proton. Thus, the conjugate pairs here are \( (\mathrm{HCl}, \mathrm{Cl}^-) \) and \( (\mathrm{CH}_3 \mathrm{COOH}, \mathrm{CH}_3 \mathrm{COOH}_2^+) \).

03

Match Conjugate Pairs to Options

Now, check which given options match the determined pairs:- Option d: \((\mathrm{HCl}, \mathrm{Cl}^-)\) and \((\mathrm{CH}_3\mathrm{COOH}_2^+, \mathrm{CH}_3\mathrm{COOH})\) matches our identified conjugate pairs.Thus, option d correctly describes the sets of conjugate acid-base pairs.

Unlock Step-by-Step Solutions & Ace Your Exams!

• Full Textbook Solutions

  Get detailed explanations and key concepts

• Unlimited Al creation

  Al flashcards, explanations, exams and more...

• Ads-free access

  To over 500 millions flashcards

• Money-back guarantee

  We refund you if you fail your exam.

Over 30 million students worldwide already upgrade their learning with 91Ó°ÊÓ!

Key Concepts

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

Bronsted-Lowry acid

The Bronsted-Lowry theory is a fundamental concept in chemistry. It describes acids and bases based on their behavior in chemical reactions. According to this theory:

• An acid is a substance that donates protons (H⁺ ions) to another substance.
• A base is a substance that accepts protons.

In the given equilibrium reaction, we can observe this behavior clearly. Hydrogen chloride (HCl) acts as a Bronsted-Lowry acid because it donates a proton to acetic acid, transforming into chloride ion (Cl^-).
On the other hand, acetic acid (CH₃COOH) demonstrates its role as a Bronsted-Lowry base by accepting the proton donated by HCl. This understanding helps us identify which molecules act as acids or bases in a reaction, making it easier to balance equations and predict reaction outcomes.

proton donation

Proton donation is a key feature of acid-base reactions, particularly in the context of the Bronsted-Lowry theory. The ability of a molecule to donate a proton is what characterizes it as an acid. In a chemical reaction, when an acid donates a proton, it transforms into its conjugate base. For instance:

• In the reaction \[\mathrm{HCl} + \mathrm{CH}_3\mathrm{COOH} \leftrightarrow \mathrm{Cl}^- + \mathrm{CH}_3\mathrm{COOH}_2^+\]Hydrogen chloride (HCl) donates a proton to acetic acid, turning into chloride ion.

Proton donation alters the balance of charge in the molecule, affecting both the physical and chemical properties. Understanding this concept helps you predict and manipulate reactions that are central to physical chemistry.
Whether you're adjusting pH or synthesizing new compounds, recognizing the role of proton donors is essential.

equilibrium reaction

In physical chemistry, equilibrium reactions are those that can proceed in both directions, meaning reactants are continuously being converted to products and vice versa. This is shown by the double arrow (\(\leftrightarrow\)) in equations. In the context of our exercise:

• The reaction \[\mathrm{HCl} + \mathrm{CH}_3\mathrm{COOH} \leftrightarrow \mathrm{Cl}^- + \mathrm{CH}_3\mathrm{COOH}_2^+\]involves forward and reverse reactions happening simultaneously.

Reaching equilibrium means that the rates of the forward and reverse reactions are equal, resulting in constant concentrations of reactants and products.
Moreover, equilibrium does not mean that the amounts are equal, but rather stable. These reactions are influenced by changes in concentration, temperature, and pressure, enabling control over the system's behavior.
Understanding equilibrium is essential for predicting how reactions respond to external changes, crucial for designing chemical processes and industrial applications.

physical chemistry

Physical chemistry bridges the gap between physics and chemistry, focusing on the interplay of energy and materials on a molecular and atomic level. It includes the study of reaction mechanisms, thermodynamics, quantum chemistry, and more.
In our context, the equilibrium reaction of HCl and CH₃COOH offers a glimpse into how physical chemistry principles explain the behavior of molecules in different states and environments.

• Reaction kinetics helps us understand the rate of the reaction and factors affecting speeds.
• Thermodynamics explains how energy is transferred and conserved within these reactions.

Physical chemistry provides the tools to model and predict how chemical systems will respond under varied conditions, which is critical in fields like materials science and biochemistry. Understanding these principles allows chemists to create efficient industrial processes, develop new materials, and innovate in fields like pharmaceuticals.