Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 16: Problem 38

List the factors on which the \(K_{\mathrm{a}}\) of a weak acid depends.

Short Answer

Expert verified
The factors influencing the \(K_{\mathrm{a}}\) of a weak acid include temperature, inherent strength of the acid, and type of solvent used.

Step by step solution

01

Factor 1: Temperature

Temperature is a significant factor affecting the \(K_{\mathrm{a}}\) of a weak acid. Factors affecting chemical equilibrium, such as the \(K_{\mathrm{a}}\) value, are themselves influenced by temperature. Generally, a rise in temperature will cause an increase in the \(K_{\mathrm{a}}\) value of a weak acid, thus enhancing the ionization of the acid.
02

Factor 2: Strength of the Acid

The second factor to consider is the inherent strength of the acid. A stronger acid will have a larger \(K_{\mathrm{a}}\) value, signifying that it produces more ions when it dissociates in solution. The strength of the acid depends on its molecular structure, particularly the stability of the ion formed when the acid molecule loses a proton (H+). The more stable the ion, the stronger the acid and the larger the \(K_{\mathrm{a}}\) value.
03

Factor 3: Type of Solvent

The third factor is the type of solvent in which the acid is dissolved. \(K_{\mathrm{a}}\) values are typically measured in water, but if another solvent is used, the \(K_{\mathrm{a}}\) value and so the degree of dissociation of the weak acid could change. The dielectric constant of the solvent, which is a measure of its ability to reduce the force between charged particles, influences the \(K_{\mathrm{a}}\) value of the weak acid in solution.

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.

Start your free trial

Over 30 million students worldwide already upgrade their learning with Vaia!

One App. One Place for Learning.

All the tools & learning materials you need for study success - in one app.

Get started for free

Most popular questions from this chapter

Which of the following is the stronger acid: \(\begin{array}{llll}\mathrm{CH}_{2} \mathrm{ClCOOH} & \text { or } \mathrm{CHCl}_{2} \mathrm{COOH} ? & \text { Explain your }\end{array}\) choice.

List four factors that affect the strength of an acid.

To which of the following would the addition of an equal volume of \(0.60 \mathrm{M} \mathrm{NaOH}\) lead to a solution having a lower \(\mathrm{pH} ?\) (a) water, (b) \(0.30 \mathrm{M} \mathrm{HCl}\), (c) \(0.70 \mathrm{M} \mathrm{KOH}\) (d) \(0.40 \mathrm{M} \mathrm{NaNO}_{3}\).

Most of the hydrides of Group \(1 \mathrm{~A}\) and Group \(2 \mathrm{~A}\) metals are ionic (the exceptions are \(\mathrm{BeH}_{2}\) and \(\mathrm{MgH}_{2}\), which are covalent compounds). (a) Describe the reaction between the hydride ion \(\left(\mathrm{H}^{-}\right)\) and water in terms of a Bronsted acid-base reaction. (b) The same reaction can also be classified as a redox reaction. Identify the oxidizing and reducing agents.

Calculate the concentrations of \(\mathrm{H}^{+}, \mathrm{HCO}_{3}^{-},\) and \(\mathrm{CO}_{3}^{2-}\) in a \(0.025 \mathrm{M} \mathrm{H}_{2} \mathrm{CO}_{3}\) solution.
See all solutions

Recommended explanations on Chemistry Textbooks

Ionic and Molecular Compounds

Read Explanation

Chemistry Branches

Read Explanation

Chemical Analysis

Read Explanation

Organic Chemistry

Read Explanation

The Earths Atmosphere

Read Explanation

Physical Chemistry

Read Explanation
View all explanations

What do you think about this solution?

We value your feedback to improve our textbook solutions.

Study anywhere. Anytime. Across all devices.

Sign-up for free