Question

conjugate acid-base pairs differ by which one of the following? a hydronium ion a proton a hydronium or hydroxide ion an electron a hydroxide ion an oxyanion which of the following solutions i

Answer 1

Conjugate acid-base pairs differ by a single proton. A conjugate acid has one more proton than its conjugate base, as in the pair of H2O and OH−. The strength of an acid or base can be compared to water and is influential in determining if a base will show basic behavior in an aqueous solution.

Step-by-step explanation:

Conjugate acid-base pairs differ by the presence or absence of a single proton (H+). A conjugate acid has one more proton than its corresponding base. For example, H2O (water) and OH− (hydroxide ion) form a conjugate acid-base pair; here, water is the conjugate acid as it has one more proton compared to the hydroxide ion, which is the conjugate base.

In the context of acid-base reactions, when a strong base reacts with water, it accepts protons from water to form the conjugate acid and hydroxide ion. Weaker bases than water may not show observable basic behavior in aqueous solution because their conjugate acids, which are stronger than water, would react to re-form the base. This concept helps us understand the relative strengths of acids and bases by comparing them to water, typically highlighted in acid-base pair charts, such as in Figures 10.2.2, 15.3.3, and 14.8.

Answer 2

Conjugate acid-base pairs differ by a proton. H₂O as the conjugate acid has one more proton than OH⁻, the conjugate base. Acid strength influences the formation of hydronium ions and observable behavior in aqueous solutions.

Step-by-step explanation:

The conjugate acid-base pairs differ by a proton (H+). When comparing such pairs, one member of the pair, the acid, has an extra proton in comparison to its counterpart, the base. For instance, in the pair H₂O and OH⁻, H₂O acts as the conjugate acid, possessing one more proton, while OH⁻ is the conjugate base, having one proton less. Exploring acid-base strength, compounds that are weaker acids than water show no observable acidic behavior in aqueous solution, and their conjugate bases are relatively strong. Conversely, species that are stronger acids than water are capable of transferring protons to water, resulting in varying degrees of ionization and the formation of hydronium ions in aqueous solution.