Acids and Base [ENDORSED]
Moderators: Chem_Mod, Chem_Admin
-
- Posts: 105
- Joined: Fri Sep 24, 2021 6:40 am
-
- Posts: 101
- Joined: Fri Sep 24, 2021 5:30 am
- Been upvoted: 1 time
Re: Acids and Base
Acids are able to donate an H+, or accept electrons, while bases can accept H+ or donate electrons. So, you would look at the chemical formula to determine whether a molecule is able to accept or donate either of these. For example, HF can donate an H+, turning it into its conjugate base, F-.
-
- Posts: 101
- Joined: Fri Sep 24, 2021 7:05 am
Re: Acids and Base
Adding on to the previous answer, depending on the definition you are using, acids and bases are defined differently. The Bronsted-Lowry definition is the one that says acids donate H+ ions and bases accept H+ ions. The Lewis definition says that acids accept lone pairs of electrons and bases donate lone pairs of electrons.
Re: Acids and Base
Depend on the situation, for if you want to have a Lewis acid/base and Bronsted acid/base . For Lewis acid/base, they are defined as lone pair acceptor or lone pair donor. For Bronsted acid/base, it gives off proton or accept a proton.
Hope this helps.
Hope this helps.
-
- Posts: 167
- Joined: Fri Sep 24, 2021 5:14 am
Re: Acids and Base [ENDORSED]
The proton donor is an acid while the proton acceptor is the base (for bronsted acids).
Return to “Bronsted Acids & Bases”
Who is online
Users browsing this forum: No registered users and 6 guests