In the context of the Bronsted-Lowry theory, acids and bases always come in pairs known as conjugate acid-base pairs. When an acid donates a proton, it forms its conjugate base. For instance, in the reaction between HCl and NaOH, hydrochloric acid (HCl) donates a proton to produce chloride ion (Cl^-), its conjugate base.
Likewise, when a base accepts a proton, it forms its conjugate acid. In the same reaction, the hydroxide ion (OH^-) from sodium hydroxide (NaOH) accepts a proton to form water (H2O), its conjugate acid.
- This relationship is crucial for understanding the direction of acid-base reactions.
- It helps predict the strength of acids and bases.
- It also provides insight into the reaction's mechanism and outcome.