Bases ______ H+ ions.

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Multiple Choice

Bases ______ H+ ions.

Explanation:
In this concept, bases are defined by proton transfer: a base accepts H+ ions. When a base encounters an acid, the acid donates a proton and the base takes it up, forming the conjugate acid of the base. This proton acceptance reduces the free H+ in solution, raising the pH. A common example is ammonia in water: NH3 accepts a proton to form NH4+, while water becomes OH−. This illustrates why the base is the proton acceptor. The other statements describe behaviors that aren’t the defining action of a base in Bronsted–Lowry terms—donating H+ would be an acid behavior, and while bases can participate in neutralization with acids, the key feature here is accepting H+.

In this concept, bases are defined by proton transfer: a base accepts H+ ions. When a base encounters an acid, the acid donates a proton and the base takes it up, forming the conjugate acid of the base. This proton acceptance reduces the free H+ in solution, raising the pH. A common example is ammonia in water: NH3 accepts a proton to form NH4+, while water becomes OH−. This illustrates why the base is the proton acceptor. The other statements describe behaviors that aren’t the defining action of a base in Bronsted–Lowry terms—donating H+ would be an acid behavior, and while bases can participate in neutralization with acids, the key feature here is accepting H+.

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