Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 15: Problem 49

A \(0.040 M\) solution of a monoprotic acid is 14 percent ionized. Calculate the ionization constant of the acid.

Short Answer

Expert verified
The ionization constant of the acid is \(Ka = 0.000814\).

Step by step solution

01

Converting Percentage Ionization into Concentration

Firstly, calculate the concentration of the ionized acid. Given that the 0.040 M solution of acid is 14 percent ionized, the concentration of ionized acid ([H+] = [A-]) would be 0.14 * 0.040 M = 0.0056 M.
02

Substitute Values into the Ka Formula

Secondly, substitute the values into the equilibrium constant expression for ionization of a monoprotic acid which is \(Ka = [H+][A-]/[HA]\). Given that [H+] = [A-] and the remaining concentration of HA is ([HA] initial - [H+]), the Ka can be calculated as follows: \(Ka = (0.0056)^2 / (0.040 - 0.0056)\).
03

Calculate the Ionization Constant

Finally, carrying out the computation from Step 2 yields Ka. This gives \(Ka = 0.000814\).

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

Calculate the \(\mathrm{pH}\) of a \(0.20 \mathrm{M} \mathrm{NaHCO}_{3}\) solution. (Hint: As an approximation, calculate hydrolysis and ionization separately first, followed by partial neutralization.)

A solution is made by dissolving \(18.4 \mathrm{~g}\) of \(\mathrm{HCl}\) in \(662 \mathrm{~mL}\) of water. Calculate the \(\mathrm{pH}\) of the solution. (Assume that the volume remains constant.)

What are the Lewis definitions of an acid and a base? In what way are they more general than the Brønsted definitions?

When the concentration of a strong acid is not substantially higher than \(1.0 \times 10^{-7} M,\) the ionization of water must be taken into account in the calculation of the solution's pH. (a) Derive an expression for the \(\mathrm{pH}\) of a strong acid solution, including the contribution to \(\left[\mathrm{H}^{+}\right]\) from \(\mathrm{H}_{2} \mathrm{O}\). (b) Calculate the \(\mathrm{pH}\) of a \(1.0 \times 10^{-7} M \mathrm{HCl}\) solution.

\(\mathrm{H}_{2} \mathrm{SO}_{4}\) is a strong acid, but \(\mathrm{HSO}_{4}^{-}\) is a weak acid. Account for the difference in strength of these two related species.
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Making Measurements

Read Explanation

The Earths Atmosphere

Read Explanation

Chemical Analysis

Read Explanation

Nuclear Chemistry

Read Explanation

Inorganic 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