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Chapter 4: Problem 28

What are the characteristics of an acid-base neutralization reaction?

Short Answer

Expert verified
Acid-base neutralization reactions involve an acid and a base reacting to form a salt and water. They are characterized by: 1. Reactants are an acid and a base. 2. The hydrogen ions from the acid combine with the hydroxide ions from the base to form water. 3. A salt is formed from the positive ion from the base and the negative ion from the acid. 4. A change in pH towards neutrality. 5. The general form is: Acid + Base -> Salt + Water.

Step by step solution

01

Recognizing the Reactants

An acid-base neutralization reaction involves an acid and a base as the reactants. Acids are substances that donate protons or hydrogen ions, while bases are substances that accept protons or donate hydroxide ions.
02

Understanding the Reaction Process

During this type of reaction, the hydrogen ions from the acid react with the hydroxide ions from the base to form water, which is a neutral substance. This is why the reaction is called 'neutralization'.
03

Identifying the Products

The other product formed in a neutralization reaction is a salt. A salt is an ionic compound made up of the positive ion from the base and the negative ion from the acid. The type of salt produced varies based on the specific acid and base involved in the reaction.
04

Knowing the Indicators

One way to recognize a neutralization reaction is the change in pH. The pH of an acid is less than 7, the pH of a base is more than 7, and the pH of pure water (the result of an ideal neutralization reaction) is 7.
05

The General Reaction Form

Putting all this together, the general form of an acid-base neutralization reaction is: \[ Acid + Base \rightarrow Salt + Water \]

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Most popular questions from this chapter

Ammonium nitrate \(\left(\mathrm{NH}_{4} \mathrm{NO}_{3}\right)\) is one of the most important nitrogen-containing fertilizers. Its purity can be analyzed by titrating a solution of \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) with a standard \(\mathrm{NaOH}\) solution. In one experiment a \(0.2041-\mathrm{g}\) sample of industrially prepared \(\mathrm{NH}_{4} \mathrm{NO}_{3}\) required \(24.42 \mathrm{~mL}\) of \(0.1023 \mathrm{M} \mathrm{NaOH}\) for neutralization. (a) Write a net ionic equation for the reaction. (b) What is the percent purity of the sample?

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