Answered

Discover answers to your questions with Westonci.ca, the leading Q&A platform that connects you with knowledgeable experts. Join our platform to connect with experts ready to provide accurate answers to your questions in various fields. Explore comprehensive solutions to your questions from knowledgeable professionals across various fields on our platform.

What is the pH of a solution that contains 0.0011 moles of KOH in 393 mL of solution?

Sagot :

samueladesida43

The pH of a solution that contains 0.0011 moles of KOH in 393 mL of solution is 2.56. Details about pH can be found below.

How to calculate pH?

The pH of a solution can be calculated using the following expression:

pH = - log [H3O+]

However, the hydrogen concentration of the KOH solution can be calculated as follows:

concentration = 0.0011 mol ÷ 0.393 L

concentration = 2.798 × 10-³M

The pH of KOH = - log [2.798 × 10-³M]

pH = 2.56

Therefore, the pH of a solution that contains 0.0011 moles of KOH in 393 mL of solution is 2.56.

Learn more about pH at: https://brainly.com/question/15289741

#SPJ1

We hope our answers were helpful. Return anytime for more information and answers to any other questions you may have. Thanks for stopping by. We strive to provide the best answers for all your questions. See you again soon. We're dedicated to helping you find the answers you need at Westonci.ca. Don't hesitate to return for more.