Chemistry 9th Edition

Published by Cengage Learning
ISBN 10: 1133611095
ISBN 13: 978-1-13361-109-7

Chapter 14 - Acids and Bases - Exercises - Page 704: 59


The $HI$ concentration in this solution is equal to $3.2 \times 10^{-3}M$

Work Step by Step

Since $HI$ is a strong acid, $[H_3O^+] = [HI]_{initial}$ 1. Calculate the hydronium ion concentration in this solution: $[H_3O^+] = 10^{-pH}$ $[H_3O^+] = 10^{- 2.50}$ $[H_3O^+] = 3.2 \times 10^{- 3}M$ Therefore, $[HI]_{initial} = 3.2 \times 10^{-3}M$
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