Final answer:
Water is versatile as a Brønsted-Lowry acid or base, being able to donate or accept protons depending on the reaction conditions. It is suitable to protonate compounds in mechanisms like the hydration of alkenes.
Step-by-step explanation:
To determine if H₂O is a suitable reagent to protonate a compound, we must consider its ability to donate or accept a proton. Water can act in both ways under the right conditions. As a Brønsted-Lowry acid, water can donate a proton; as a Brønsted-Lowry base, it can accept one. In the hydration of alkenes, H₂O is a suitable reagent where it participates in the reaction mechanism as a nucleophile and as part of the proton transfer process. Furthermore, water plays a role as a base in the reaction with strong acids like HCl, wherein it accepts a proton, creating hydronium ions. These examples illustrate the dual role water can play depending on the reactants and the reaction environment.
H₂O can act as both a Brønsted-Lowry acid and a Brønsted-Lowry base under the right conditions. It can donate a proton, making it an acid, and it can accept a proton, making it a base. The reaction between HCl and water is an example of H₂O acting as a base, as it accepts a proton from the acid. Therefore, H₂O is a suitable reagent to protonate compounds.