Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 15: Problem 18

Why are weak acids and weak bases poor electrical conductors?

Short Answer

Expert verified
Weak acids and bases are poor electrical conductors because they only partially ionize in solution, resulting in a lower concentration of ions, which are the charge carriers necessary for electrical conductivity.

Step by step solution

01

Understanding the concept of conductivity

Electrical conductivity in a solution depends on the ions present in the solution. Ions form when a substance dissociates or breaks up into charged particles. The greater the ion concentration in the solution, the greater the conductivity.
02

What defines a weak acid and a weak base

Weak acids and bases partially ionize in solution, meaning that in a solution of a weak acid or base, there are not only ions, but also a substantial amount of the original, non-ionized substance (molecules). Because of this, the concentration of ions in a solution of a weak acid or base is relatively low.
03

Comparing the conductivity

Comparatively, solutions of strong acids and bases, which fully ionize in solution, have a higher concentration of ions, which makes them better electrical conductors. As a result, weak acids or bases are poor conductive materials, since they generate fewer ions which can carry the electrical charge.

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

What is \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) in a solution whose pH is 1.9\(?\)

What is the \(\mathrm{pH}\) of aqueous solutions of the strong acid \(\mathrm{HNO}_{3},\) nitric acid, if the concentrations of the solutions are as follows: (a) \(0.005 \mathrm{M},(\mathrm{b}) 0.05 \mathrm{M},(\mathrm{c}) 0.5 \mathrm{M},(\mathrm{d}) 5 \mathrm{M} ?\)

LiOH is a strong base. What is the pH of a 0.082 M LiOH solution?

To standardize a hydrochloric acid solution, it was used as titrant with a solid sample of sodium hydrogen carbonate, NaHCO \(_{3} .\) The sample had a mass of \(0.3967 \mathrm{g},\) and 41.77 \(\mathrm{mL}\) of acid was required to reach the equivalence point. Calculate the concentration of the standard solution.

What two buret readings need to be recorded in order to determine the volume of solution dispensed by the buret?
See all solutions

Recommended explanations on Chemistry Textbooks

Physical Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Chemical Reactions

Read Explanation

Making Measurements

Read Explanation

Kinetics

Read Explanation

Nuclear 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