Fundamentals J #1

Moderators: Chem_Mod, Chem_Admin

Posts: 37
Joined: Mon Jun 17, 2019 7:23 am

Fundamentals J #1

Postby hannabarlow1A » Wed Jul 24, 2019 8:57 am

For number #1 in section J, they ask to identify each compound as a Bronsted acid or base. NH3, HBr, KOH, H2SO3, and Ca(OH)2
I know that Bronsted acids are proton donors and bases are acceptors, but how do we identify that based on just their molecular formula? I feel like I am missing something obvious

Posts: 17479
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 391 times

Re: Fundamentals J #1

Postby Chem_Mod » Wed Jul 24, 2019 10:18 am

The Bronsted-Lowry definition of acids and bases focuses on the transfer of protons. A Bronsted acid is a proton donor and a Bronsted base is a proton acceptor. When identifying compounds as Bronsted acids or bases, we must take into account the solvent that we are dissolving the compound in. When NH3 dissolves in water, it acts as a Bronsted base and accepts a proton from H20 to form OH-.
NH3 (aq) + H20 (l) --> NH4+ (aq) + OH- (aq)
HBr is a strong acid and dissolves in water and dissociates 100% to produce protons. This solution will have a high concentration of protons.
HBr --> H+ (aq) + Br- (aq) OR HBr + H20 --> Br- + H30+

Return to “Bronsted Acids & Bases”

Who is online

Users browsing this forum: No registered users and 1 guest