Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 13: Problem 15

Can the \(\mathrm{pH}\) of a solution be negative? Explain.

Short Answer

Expert verified
Yes, the pH of a solution can be negative if the molar concentration of hydrogen ions \([H^+]\) is greater than 1, which can occur in extremely acidic solutions. This is because the pH is calculated as \[pH = -\log_{10} [H^+]\], and logarithm values become negative when their argument is greater than 1.

Step by step solution

01

Understanding pH

pH is a measure of the acidity of a solution, which represents the concentration of hydrogen ions (H+) in the solution. It is defined as the negative logarithm (base 10) of the molar concentration of hydrogen ions. Mathematically, it can be expressed as: \[ pH = -\log_{10} [H^+] \] where [H^+] is the molar concentration of hydrogen ions in the solution.
02

Calculating pH

To calculate the pH of a solution, we need to find the concentration of hydrogen ions. We can then plug it into the formula mentioned above. For example, consider a solution with [H^+] = 0.01 M (mol/L). The pH of the solution can be calculated as follows: \[ pH = -\log_{10} (0.01) = 2\] In this case, the pH of the solution is 2.
03

Can pH be negative?

The pH of a solution can be negative if the molar concentration of hydrogen ions [H^+] is greater than 1. This can occur in very acidic solutions. Mathematically speaking, logarithm values become negative when their argument (input) is greater than 1. For example, if the [H^+] > 1: \[ pH = -\log_{10}([H^+]) < 0\] In this case, the pH of the solution will indeed be negative.
04

Conclusion

Yes, the pH of a solution can be negative. This occurs when the molar concentration of hydrogen ions [H^+] in the solution is greater than 1. This is often seen in extremely acidic solutions.

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

Monochloroacetic acid, \(\mathrm{HC}_{2} \mathrm{H}_{2} \mathrm{ClO}_{2}\), is a skin irritant that is used in "chemical peels" intended to remove the top layer of dead skin from the face and ultimately improve the complexion. The value of \(K_{\mathrm{a}}\) for monochloroacetic acid is \(1.35 \times 10^{-3}\) Calculate the \(\mathrm{pH}\) of a \(0.10-M\) solution of monochloroacetic acid.

Determine \(\left[\mathrm{OH}^{-}\right],\left[\mathrm{H}^{+}\right],\) and the \(\mathrm{pH}\) of each of the following solutions. a. \(1.0 M\) KCl b. \(1.0 M \mathrm{KC}_{2} \mathrm{H}_{3} \mathrm{O}_{2}\)

A typical sample of vinegar has a pH of \(3.0 .\) Assuming that vinegar is only an aqueous solution of acetic acid \(\left(K_{a}=1.8 \times\right.\) \(10^{-5}\) ), calculate the concentration of acetic acid in vinegar.

Place the species in each of the following groups in order of increasing base strength. Give your reasoning in each case. a. \(\mathrm{IO}_{3}^{-}, \mathrm{BrO}_{3}^{-}\) b. \(\mathrm{NO}_{2}^{-}, \mathrm{NO}_{3}^{-}\) c. \(\mathrm{OCl}^{-}, \mathrm{OI}^{-}\)

Sodium azide (NaN, ) is sometimes added to water to kill bacteria. Calculate the concentration of all species in a \(0.010-M\) solution of \(\mathrm{NaN}_{3} .\) The \(K_{\mathrm{a}}\) value for hydrazoic acid \(\left(\mathrm{HN}_{3}\right)\) is \(1.9 \times 10^{-5}\)
See all solutions

Recommended explanations on Chemistry Textbooks

Making Measurements

Read Explanation

Chemical Reactions

Read Explanation

Nuclear Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Ionic and Molecular Compounds

Read Explanation

The Earths Atmosphere

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