In chemistry, we learned that when we have a bronsted-lowry acid and base, the acid donates a proton to the base. However this conflicts with the knowledge that an acid an a base form a salt and water. When do you use each method?
Answers
Answer:
A Brønsted-Lowry acid is any species that is capable of donating a proton—\text{H}^+H
+
start text, H, end text, start superscript, plus, end superscript.
A Brønsted-Lowry base is any species that is capable of accepting a proton, which requires a lone pair of electrons to bond to the \text{H}^+H
+
start text, H, end text, start superscript, plus, end superscript.
Water is amphoteric, which means it can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base.
Strong acids and bases ionize completely in aqueous solution, while weak acids and bases ionize only partially.
The conjugate base of a Brønsted-Lowry acid is the species formed after an acid donates a proton. The conjugate acid of a Brønsted-Lowry base is the species formed after a base accepts a proton.
The two species in a conjugate acid-base pair have the same molecular formula except the acid has an extra \text H^+H
+
start text, H, end text, start superscript, plus, end superscript compared to the conjugate base