Which of the following statements is false? (a) An Arrhenius base increases the concentration of OH- in water. (b) A Brønsted-Lowry base is a proton acceptor. (c) Water can act as a Brønsted–Lowry acid. (d) Water can act as a Brønsted–Lowry base. (e) Any compound that contains an –OH group acts as a Brønsted-Lowry base.

검증된 단계별 안내

Identify the definitions of Arrhenius and Brønsted-Lowry acids and bases.

Recall that an Arrhenius base increases the concentration of OH^- ions in water.

Understand that a Brønsted-Lowry base is defined as a proton (H^+) acceptor.

Recognize that water (H2O) can act as both a Brønsted-Lowry acid (proton donor) and a Brønsted-Lowry base (proton acceptor).

Evaluate the statement that any compound with an –OH group acts as a Brønsted-Lowry base, and consider exceptions such as alcohols, which do not typically act as bases.

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Arrhenius Theory of Acids and Bases

The Arrhenius theory defines acids as substances that increase the concentration of hydrogen ions (H+) in aqueous solution, while bases increase the concentration of hydroxide ions (OH-). This theory is foundational in understanding the behavior of acids and bases in water, particularly in identifying how they dissociate and interact in solution.

Brønsted-Lowry Theory of Acids and Bases

The Brønsted-Lowry theory expands the definition of acids and bases beyond aqueous solutions. According to this theory, an acid is a proton donor and a base is a proton acceptor. This concept allows for a broader understanding of acid-base reactions, including those that occur in non-aqueous environments.

Amphoteric Substances

Amphoteric substances are those that can act as either an acid or a base depending on the context of the reaction. Water is a prime example, as it can donate a proton (acting as an acid) or accept a proton (acting as a base). Understanding this dual behavior is crucial for analyzing reactions involving water and other amphoteric compounds.