Log out Go to App
Go to App

Learning Materials

Features

Discover

Chapter 15: Problem 57

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

Short Answer

Expert verified
Without using a calculator, the pH cannot be calculated exactly, but with a calculator, the pH will approximately be 5.72.

Step by step solution

01

Understand the pH formula

The pH of a solution is given by the formula: \( pH = -\log[H_3O^{+}]\), where \([H_3O^{+}]\) represents the concentration of hydronium ions in the solution in molarity (M).
02

Substitute the given value into the pH formula

Substitute the provided value of \([H_3O^{+}]\) which is \(1.9 \times 10^{-6}\) into the formula: \( pH = -\log(1.9 \times 10^{-6})\).
03

Calculate the pH value

You calculate the pH using a calculator, remembering that log in this formula represents the decimal logarithm (base 10).

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 the hydronium ion concentration in a solution whose pH is 10.0\(?\)

A student passes an end point in a titration. Is it possible to add an additional measured amount of the unknown and continue the titration? Explain how this process might work. How would the answer for the calculation of the molar concentration of the unknown differ from the answer the student would have gotten if the titration had been performed properly?

Calculate the concentration of the \(\mathrm{H}_{3} \mathrm{O}^{+}\) and \(\mathrm{OH}^{-}\) ions in an aqueous solution of pH \(5.0 .\)

What is the hydroxide ion concentration in a solution of \(\mathrm{pH} 8.72 ?\)

Write an equation for the reaction between hydrocyanic acid, HCN, and water. Label the acid, base, conjugate acid, and conjugate base.
See all solutions

Recommended explanations on Chemistry Textbooks

Chemistry Branches

Read Explanation

Making Measurements

Read Explanation

Ionic and Molecular Compounds

Read Explanation

Organic Chemistry

Read Explanation

Physical Chemistry

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