Final answer:
When a neutral Brønsted-Lowry base accepts a proton, it forms a conjugate acid with a +1 charge. Ammonia becoming ammonium is a classic example of this acid-base behavior.
Step-by-step explanation:
When a Brønsted-Lowry base with no net charge accepts a proton (H+) in an acid-base reaction, the compound becomes the conjugate acid of that base. As the base gains a proton, its overall charge increases by one. Therefore, the charge on the conjugate acid that is formed will be +1.
For example, when ammonia (NH3), which is a neutral Brønsted-Lowry base, accepts a proton, it becomes the ammonium ion (NH4+), with a positive charge. This principle is a critical part of the Brønsted-Lowry acid-base theory, which focuses on proton transfer between acids and bases, resulting in the formation of conjugate acid-base pairs.