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Chapter 15: Problem 86

\text { What is the Arrhenius definition of a base? }

Short Answer

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According to the Arrhenius theory, a base is a substance that, when dissolved in water, increases the concentration of hydroxide ions (OH⁻) in the solution. An Arrhenius base contains an OH⁻ group within its structure and donates OH⁻ ions when dissolved in water, resulting in an increase in the pH of the solution.

Step by step solution

01

Arrhenius Definition of a Base

According to the Arrhenius theory, a base is a substance that, when dissolved in water, increases the concentration of hydroxide ions (OH⁻) in the solution.
02

Features of An Arrhenius Base

An Arrhenius base has the following features: 1. It contains an OH⁻ group within its structure. 2. It donates OH⁻ ions when dissolved in water. 3. It results in an increase in the pH of the solution as the hydroxide ion concentration increases. Some examples of Arrhenius bases are sodium hydroxide (NaOH), potassium hydroxide (KOH), and calcium hydroxide (Ca(OH)₂).

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Most popular questions from this chapter

What is the molar concentration of hydronium ion and hydroxide ion in pure water at \(25{ }^{\circ} \mathrm{C}\) ?

Solid ammonium chloride, \(\mathrm{NH}_{4} \mathrm{Cl}\), reacts with solid sodium hydroxide to produce ammonia gas, water, and sodium chloride, \(\mathrm{NaCl}\). (a) Write a balanced equation for this reaction. (b) According to the Bronsted-Lowry definition, which species is the acid and which species is the base? Explain.

Why is a pH of 7 equal to neutrality?

You mix \(500 \mathrm{~mL}\) of \(1.00 \mathrm{M} \mathrm{NaOCl}\) with \(500 \mathrm{~mL}\) of \(0.500 \mathrm{MHNO}_{3}\). Write an equation for the reaction that occurs. Besides water, what species are in the solution after reaction? Is this solution a buffer?

\(\mathrm{HClO}_{4}\) is a strong acid, and \(\mathrm{HClO}_{2}\) is a weak acid. If you had a \(1.0 \mathrm{M}\) solution of \(\mathrm{NaClO}_{4}\) and a \(1.0 \mathrm{M}\) solution of \(\mathrm{NaClO}_{2}\), which would have the higher pH? Explain.
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