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Chapter 15: Problem 1

How does a strong acid differ from a weak acid?

Short Answer

Expert verified
A strong acid differs from a weak acid by the degree of dissociation. Strong acids completely dissociate in solutions, donating all of their hydrogen (H+) ions, while weak acids only partly dissociate, releasing fewer hydrogen ions.

Step by step solution

01

Understanding Acids

An acid, according to Arrhenius, is a substance that releases hydrogen ions (H+) when dissolved in water. On the other hand, the Bronsted-Lowry definition of an acid is a proton (H+) donor. Acids play an essential role in many chemical reactions and biological processes.
02

Defining Strong Acids

A strong acid is one that completely dissociates into its ions in a solution. This means that all the acid molecules break apart and donate their hydrogen ions in water solution. Examples of strong acids are Hydrochloric acid (HCl), Sulfuric acid (H2SO4), and Nitric acid (HNO3).
03

Defining Weak Acids

A weak acid is one that only partially dissociates into its ions in a solution. Not all acid molecules break apart; only a small percentage donate their hydrogen ions in a water solution. Strong acids disassociate more readily and release more hydrogen ions than weak acids. Examples of weak acids are Acetic acid (CH3COOH), and Citric acid (C6H8O7).
04

Comparison

In conclusion, the primary difference between a strong acid and a weak acid lies in the degree of dissociation. While a strong acid completely dissociates and releases all its hydrogen ions in solution, a weak acid only partially dissociates, releasing fewer hydrogen ions in solution.

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Most popular questions from this chapter

Would the \(\mathrm{pH}\) at the equivalence point of a titration of a weak acid with a strong base be less than, equal to, or greater than 7.0\(?\)

Stomach acid contains \(\mathrm{HCl}\) , whose concentration is about 0.03 \(\mathrm{mol} / \mathrm{L} .\) What is the pH of stomach acid?

A solution has a pH of \(10.1 .\) Calculate the hydronium ion concentration and the hydroxide ion concentration.

An HNO \(_{3}\) solution has a pH of \(3.06 .\) What volume of 0.015 \(\mathrm{M}\) LiOH will be required to titrate 65.0 \(\mathrm{mL}\) of the HNO \(_{3}\) solution to reach the equivalence point?

Explain the difference between end point and equivalence point. Why is it important that both occur at approximately the same pH in a titration?
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