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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

Acetic acid \(\left(\mathrm{CH}_{3} \mathrm{COOH}\right)\) is an important ingredient of vinegar. A sample of \(50.0 \mathrm{~mL}\) of a commercial vinegar is titrated against a \(1.00 \mathrm{M} \mathrm{NaOH}\) solution. What is the concentration (in \(M\) ) of acetic acid present in the vinegar if \(5.75 \mathrm{~mL}\) of the base were required for the titration?

Hydrogen halides (HF, HCl, HBr, HI) are highly reactive compounds that have many industrial and laboratory uses. (a) In the laboratory, HF and HCl can be generated by reacting \(\mathrm{CaF}_{2}\) and \(\mathrm{NaCl}\) with concentrated sulfuric acid. Write appropriate equations for the reactions. (Hint: These are not redox reactions.) (b) Why is it that HBr and HI cannot be prepared similarly, that is, by reacting \(\mathrm{NaBr}\) and \(\mathrm{NaI}\) with concentrated sulfuric acid? (Hint: \(\mathrm{H}_{2} \mathrm{SO}_{4}\) is a stronger oxidizing agent than both \(\mathrm{Br}_{2}\) and \(\mathrm{I}_{2} .\) ) (c) \(\mathrm{HBr}\) can be prepared by reacting phosphorus tribromide \(\left(\mathrm{PBr}_{3}\right)\) with water. Write an equation for this reaction.

This "cycle of copper" experiment is performed in some general chemistry laboratories. The series of reactions starts with copper and ends with metallic copper. The steps are: (1) A piece of copper wire of known mass is allowed to react with concentrated nitric acid [the products are copper(II) nitrate, nitrogen dioxide, and water]. (2) The copper(II) nitrate is treated with a sodium hydroxide solution to form copper(II) hydroxide precipitate. (3) On heating, copper(II) hydroxide decomposes to yield copper(II) oxide. (4) The copper(II) oxide is reacted with concentrated sulfuric acid to yield copper(II) sulfate. (5) Copper(II) sulfate is treated with an excess of zinc metal to form metallic copper. (6) The remaining zinc metal is removed by treatment with hydrochloric acid, and metallic copper is filtered, dried, and weighed. (a) Write a balanced equation for each step and classify the reactions. (b) Assuming that a student started with \(65.6 \mathrm{~g}\) of copper, calculate the theoretical yield at each step. (c) Considering the nature of the steps, comment on why it is possible to recover most of the copper used at the start.

(a) Without referring to Figure 4.10 , give the oxidation numbers of the alkali and alkaline earth metals in their compounds. (b) Give the highest oxidation numbers that the Groups \(3 \mathrm{~A}-7 \mathrm{~A}\) elements can have.

Someone spilled concentrated sulfuric acid on the floor of a chemistry laboratory. To neutralize the acid, would it be preferable to pour concentrated sodium hydroxide solution or spray solid sodium bicarbonate over the acid? Explain your choice and the chemical basis for the action
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