conjugate acids

Moderators: Chem_Mod, Chem_Admin

Madelyn Cearlock
Posts: 72
Joined: Fri Sep 28, 2018 12:19 am

conjugate acids

Postby Madelyn Cearlock » Mon Dec 03, 2018 8:24 pm

Can someone help me write the formula for the conjugate acids of CH3NH2 and methylamine

Emma Scholes 1L
Posts: 62
Joined: Fri Sep 28, 2018 12:18 am

Re: conjugate acids

Postby Emma Scholes 1L » Mon Dec 03, 2018 8:27 pm

The formula of the conjugate acid is CH3NH3+. You just add an H+.

Sydney Aurelio_Dis4B
Posts: 30
Joined: Fri Sep 28, 2018 12:28 am

Re: conjugate acids

Postby Sydney Aurelio_Dis4B » Mon Dec 03, 2018 10:58 pm

Whenever you need to determine the conjugate acid of a base you add one H+. This is because conjugate acids accept an H+ from the conjugate base. Therefore it would be CH3NH3+.

Angel Chen 2k
Posts: 59
Joined: Fri Sep 28, 2018 12:20 am

Re: conjugate acids

Postby Angel Chen 2k » Mon Dec 03, 2018 11:23 pm

I want to explain this point more generally. Since a Lowey-Bronsted acid is a proton donor, the acid gives out a proton (normally H+) to become a conjugated base. On the other hand, as a proton acceptor, the base received the proton to become a conjugated acid. In summary:
1. If you want to find the Bronsted acid and base as well as their conjugated acid or base, you need to figure out the movement of the proton (H+).
2. As what we learned in reaction equilibrium, the reaction is a dynamic equilibrium. For this reason, the conjugated acid and base can also act as reactants to react in reverse direction.
3. The strength of acid and base reminds the direction of reaction because they determine the reaction equilibrium together.

Hope this helps!

Return to “Conjugate Acids & Bases”

Who is online

Users browsing this forum: No registered users and 1 guest