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Ch.16 - Acid-Base Equilibria
Chapter 16, Problem 14

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.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

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.
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Arrhenius Acids and Bases

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.
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Bronsted-Lowry Acid-Base Theory

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.
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