Question J.5  [ENDORSED]

Moderators: Chem_Mod, Chem_Admin

Jason Muljadi 2C
Posts: 62
Joined: Thu Jul 27, 2017 3:01 am

Question J.5

Postby Jason Muljadi 2C » Sat Dec 02, 2017 9:56 pm

Complete the overall equation, and write the complete ionic equation and the net ionic equation for each of the following acid–base reactions. If the substance is a weak acid or base, leave it in its molecular form in the equations.

(b) (CH3)3N(aq) + HNO3(aq) -->


For B, why does it become (CH3)3NHNO3(aq) instead of (CH3)3NO3(aq) + HN(aq)?

Chem_Mod
Posts: 17947
Joined: Thu Aug 04, 2011 1:53 pm
Has upvoted: 406 times

Re: Question J.5  [ENDORSED]

Postby Chem_Mod » Sun Dec 03, 2017 2:00 pm

This is a proton transfer reaction forming (CH3)3NH+(aq) + NO3-(aq).

The reaction you propose is far more complicated and does not occur in aqueous solution.

Julia Meno 1D
Posts: 28
Joined: Fri Sep 29, 2017 7:04 am

Re: Question J.5

Postby Julia Meno 1D » Tue Dec 05, 2017 2:10 pm

Why is it, then, written as (CH3)3NHNO3 (aq) instead of (CH3)3NH+(aq) + NO3-(aq)?


Return to “Bronsted Acids & Bases”

Who is online

Users browsing this forum: No registered users and 1 guest