Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 15: Problem 163

If \(\mathrm{CI}^{-}\) is the conjugate base of \(\mathrm{HCl}\), why isn't an aqueous solution of \(\mathrm{NaCl}\) acidic?

Short Answer

Expert verified
An aqueous solution of NaCl isn't acidic because the dissociated ions, Na+ and Cl-, do not significantly affect the concentration of hydronium ions (\(\mathrm{H_3O^+}\)). Cl- is a weak base as the conjugate base of a strong acid (HCl), and Na+ is a weak acid as the conjugate acid of a strong base (NaOH). Both have a low tendency to either accept or donate protons, and therefore, do not make the solution acidic.

Step by step solution

01

Understanding conjugate acids and bases

A conjugate acid-base pair consists of two species that differ by one proton (H+). In this case, HCl is the acid, and Cl- is its conjugate base.
02

Analyzing the dissociation of NaCl in water

When NaCl is dissolved in water, it dissociates into its constituent ions: Na+ and Cl-. The equation for this process is: \[ \mathrm{NaCl} \rightarrow \mathrm{Na}^+ + \mathrm{Cl}^- \]
03

Understanding the role of Cl- ions

Since Cl- is the conjugate base of a strong acid (HCl), it is a weak base, almost inert. It has a very low tendency to accept protons (H+) from water, and so it doesn't significantly affect the concentration of hydronium ions (\(\mathrm{H_3O^+}\)). Therefore, it doesn't make the solution acidic.
04

Understanding the role of Na+ ions

Na+ is the conjugate acid of a strong base (NaOH). It is a weak acid, also almost inert, and has a very low tendency to donate protons (H+) to water. It doesn't have a significant effect on the concentration of hydronium ions (\(\mathrm{H_3O^+}\)) either, so it also doesn't make the solution acidic.
05

Conclusion

An aqueous solution of NaCl isn't acidic because the ions formed by the dissociation of NaCl, namely Na+ and Cl-, do not significantly affect the concentration of hydronium ions (\(\mathrm{H_3O^+}\)). The Cl- ion, as the conjugate base of a strong acid, is a weak base and does not have a high enough affinity for protons to have an effect on the acidity of the solution. Likewise, the Na+ ion, as the conjugate acid of a strong base, is a weak acid and therefore does not donate many protons to make the solution acidic.

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

The \(\mathrm{pH}\) of a solution is 4 . (a) What is the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration? (b) What is the \(\mathrm{OH}^{-}\) concentration? (c) Is this solution acidic or basic?

You mix \(500 \mathrm{~mL}\) of \(1.00 \mathrm{M} \mathrm{NaOCl}\) with \(500 \mathrm{~mL}\) of \(0.500 \mathrm{MHNO}_{3}\). Write an equation for the reaction that occurs. Besides water, what species are in the solution after reaction? Is this solution a buffer?

Is it possible to obtain water at \(25{ }^{\circ} \mathrm{C}\) that contains absolutely no ions of any sort? Explain.

Write a chemical equation for the reaction between each pair of reactants, using single or double arrows as appropriate: (a) \(\mathrm{HNO}_{3}\) and \(\mathrm{OH}^{-}\) (b) \(\mathrm{HF}\) and \(\mathrm{OH}^{-}\) (c) \(\mathrm{NH}_{3}\) and \(\mathrm{H}_{2} \mathrm{O}\) (d) \(\mathrm{HCO}_{3}^{-}\) and \(\mathrm{H}_{2} \mathrm{O}\)

Consider the following statement: "As the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration in an aqueous solution increases, the \(\mathrm{OH}^{-}\) concentration must decrease." (a) Why is this true? (b) Is there any way to stop the \(\mathrm{OH}^{-}\) concentration from decreasing as you increase the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration?
See all solutions

Recommended explanations on Chemistry Textbooks

Kinetics

Read Explanation

Physical Chemistry

Read Explanation

Chemistry Branches

Read Explanation

Making Measurements

Read Explanation

The Earths Atmosphere

Read Explanation

Chemical Reactions

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