Chemistry 12th Edition

Published by McGraw-Hill Education
ISBN 10: 0078021510
ISBN 13: 978-0-07802-151-0

Chapter 15 - Acids and Bases - Questions & Problems - Page 712: 15.70


(a) $H_2SO_4$ is a stronger acid than $H_2SeO_4$ (b) $H_3PO_4$ is a stronger acid than $H_3AsO_4$

Work Step by Step

(a) 1. Identify the type of acid: $H_2SO_4$ and $H_2SeO_4$ are both oxoacids, and we are going to compare two oxoacids having different central atoms. 2. Compare the oxidation numbers of their central atoms: Since they both have 2 H and 4 O, their oxidation number is the same. 3. Compare their electronegativity; Sulfur is more electronegative than Selenium. The more electronegative the central atom, the stronger is the oxoacid. Thus: $H_2SO_4$ is stronger than $H_2SeO_4$ (b) 1. Following the same steps, we got: - Phosphorus is more electronegative than Arsenic. Therefore: $H_3PO_4$ is stronger than $H_3AsO_4$
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