Moderators: Chem_Mod, Chem_Admin

Posts: 106
Joined: Sat Aug 24, 2019 12:17 am


Postby Ami_Pant_4G » Sat Dec 07, 2019 9:15 pm

6C.19 Decide which acid in each of the following pairs is the stronger and explain why: (a) HF or HCl; (b) HClO or HClO2; (c) HBrO2 or HClO2; (d) HClO4 or H3PO4; (e) HNO3 or HNO2; (f) H2CO3 or H2GeO3.

Can someone please explain why HCl4 is stronger than H3PO4? thanks in advance

Posts: 107
Joined: Fri Aug 09, 2019 12:17 am

Re: 6C.19

Postby JChen_2I » Sat Dec 07, 2019 9:24 pm

HClO4 is a stronger acid than HPO4. The only differing atom between them is the chlorine and phosphorus. Chlorine is more electronegative so it will help to stabilize the negative charge that will be created after the molecule gives up a proton. Chlorine is able to pull electron density towards it and away from the oxygen that had the hydrogen and therefore stabilizes the overall molecule.

Posts: 101
Joined: Thu Jul 11, 2019 12:17 am

Re: 6C.19

Postby KSong_1J » Sat Dec 07, 2019 9:25 pm

When it comes to oxoacids with the same number off oxygens attached to the central atom, the greater the electronegativity of the central atom, the stronger the acid. This is due to the fact that a greater electronegativity means it's more electron withdrawing. Therefore, HClO4 is stronger than H3PO4 because chlorine has a higher electronegativity than phosphorus.

Return to “Bronsted Acids & Bases”

Who is online

Users browsing this forum: No registered users and 1 guest