Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 15: Problem 62

Find \(\left[\mathrm{H}_{3} \mathrm{O}^{+}\right]\) in a solution of \(\mathrm{pH} 4\).

Short Answer

Expert verified
The concentration of \(\mathrm{H}_{3} \mathrm{O}^{+}\) ions in a solution with \(\mathrm{pH}\) 4 is \(10^{-4}\) M.

Step by step solution

01

Understanding pH and \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration

The \(\mathrm{pH}\) of a solution is defined as the negative logarithm (base 10) of the molar concentration of \(\mathrm{H}_{3} \mathrm{O}^{+}\) ions in the solution. So the formula that connects \(\mathrm{pH}\) and \(\mathrm{H}_{3} \mathrm{O}^{+}\) ions concentration (\(\mathrm{H+}\)) is: \[\mathrm{pH} = - \log [\mathrm{H+}]\]
02

Inverting operation

In order to find the concentration of \(\mathrm{H}_{3} \mathrm{O}^{+}\) ions for given a \(\mathrm{pH}\) value the inversion operation is done using the same formula. After rearranging the formula the \[\mathrm{H+} = 10^{-\mathrm{pH}}\]
03

Substitute pH value in the formula

Now we can substitute the \(\mathrm{pH}\) value of 4 into the equation to get the \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration. So, we have \[\mathrm{H+} = 10^{-4}\]

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

Name an indicator you might use to titrate ammonia with hydrochloric acid.

What is the pH of a solution whose \(\mathrm{H}_{3} \mathrm{O}^{+}\) concentration is \(1.9 \times 10^{-6} \mathrm{M} ?\)

Would the \(\mathrm{pH}\) at the equivalence point of a titration of a weak acid with a strong base be less than, equal to, or greater than 7.0\(?\)

Give the equation that relates pH to hydronium ion concentration.

What volume of 0.100 \(\mathrm{M} \mathrm{NaOH}\) is required to neutralize 25.00 \(\mathrm{mL}\) of 0.110 \(\mathrm{M} \mathrm{H}_{2} \mathrm{SO}_{4} ?\)
See all solutions

Recommended explanations on Chemistry Textbooks

Nuclear Chemistry

Read Explanation

Chemical Analysis

Read Explanation

Chemical Reactions

Read Explanation

Physical Chemistry

Read Explanation

Inorganic Chemistry

Read Explanation

Chemistry Branches

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