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How does Bronsted-Lowry define acids and bases?
A Brønsted-Lowry acid is any substance (molecule or ion) that can donate a hydrogen ion (##H^(+)##).
A Brønsted-Lowry base is any species that can accept a hydrogen ion (##H^(+)##).
Basically, acids are proton donors and bases are proton acceptors.
Take the reaction below for example:
##HI + NH_3 rightleftharpoons NH_4^(+) + I^(-)##
Hydroiodic acid (##HI##) is the Brønsted-Lowry acid because it donates a hydrogen ion. Ammonia (##NH_3##) is the Brønsted-Lowry base because it accepts the hydrogen ion.
The Brønsted-Lowry theory also introduces the concept of conjugate acid-base pairs. A conjugate acid-base pair are two species that differ by a (##H^(+)##) ion.
Based on the reaction above, the ammonium ion (##NH_4^(+)##) is the conjugate acid of the base ammonia and the iodide ion ##(I^(-)##) is the conjugate base of hydroiodic acid.
Here's a tip to let you know which substance is the conjugate acid and which substance is the conjugate base:
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A conjugate base has one less (##H^(+)##) proton than the acid you started with.
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A conjugate acid has one more (##H^(+)##) proton than the base you started with.
Here's a general depiction of conjugate acid-base pairs:
##HA## represents an acid
##B## represents a base
##A^(-)## represents the conjugate base since this substance has one less proton than the acid, HA.
##HB^(+)## represents the conjugate acid since this substance has one more proton than the base, B.