<meta http-equiv="refresh" content="1; url=/nojavascript/"> Bronsted-Lowry Acids/Bases | CK-12 Foundation
Dismiss
Skip Navigation
You are reading an older version of this FlexBook® textbook: From Vitamins to Baked Goods: Real Applications of Organic Chemistry Go to the latest version.

Bronsted-Lowry acids are “proton donors.” Hydrogen chloride (HCl) is an example of Bronsted-Lowry acids. When hydrogen chloride is added to water, the attraction between the positively-charged hydrogen ion in the hydrogen chloride and the negatively-charged oxygen in the water is strong enough that the hydrogen ion is removed. Hydrogen chloride is therefore called a “proton donor.”

In turn, Bronsted-Lowry bases are “proton acceptors.” They react with Bronsted-Lowry acids as the negatively-charged force that pulls protons from the acid. An example of a Bronsted-Lowry base is ammonium (NH3), which can gain a proton to form ammonia (NH4).

Image Attributions

Files can only be attached to the latest version of None

Reviews

Please wait...
Please wait...
Image Detail
Sizes: Medium | Original
 
CK.SCI.ENG.SE.1.Organic-Chemistry-Applications.2.3

Original text