How can you determine Bronsted-lowry acids and bases?

2 Answers
reudhreghs
Apr 9, 2016

Bronsted-Lowry acids drop #H^+# ions. Bases pick them up again.

Explanation:

Bronsted-Lowry acids are molecules that lose #H^+# ions. Bases are those that pick them up again.

For example,

#H_2O + HCl -> H_3O^+ + Cl^-#.

In this reaction, hydrochloric acid loses #H^+#, so it is a Bronsted-Lowry acid, while water picks up the #H^+#, so it is a Bronsted-Lowry base.

Because #Cl^-# would now accept #H^+# ions, it is called a conjugate base. In the same way, #H_3O^+# would give up the hydrogen ion and so is a conjugate acid.

Conjugate, here, simply means made or rendered.

David Drayer
Aug 14, 2016

A Bronsted acid produces a hydrogen ion # H+# in a reaction While a Bronsted base absorbs a hydrogen ion # H+# in a reaction.

Explanation:

Water #H2O# can be considered to be both a Bronsted acid and a Bronsted base.

2 #H2O# ==== #H3O+# + OH-

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