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Chapter 13: Problem 65

Can the \(\mathrm{pH}\) of an acid solution be greater than 7 ?

Short Answer

Expert verified
No, the pH of an acid solution cannot be greater than 7 because an acid by definition is a substance that increases the concentration of H+ ions when added to water, thus resulting in a pH less than 7.

Step by step solution

01

Understanding pH scale

The pH scale is a measure of the concentration of Hydrogen ions (H+) in solution, varying from 0 to 14. A pH of 7 is neutral, values less than 7 indicate acidity and more than 7 indicate basicity.
02

Classification of Solutions Based on pH

Acidic solutions have a higher concentration of H+ ions, hence they have pH less than 7. Basic (or alkaline) solutions, on the other hand, have pH greater than 7 due to a lower concentration of H+ ions or, equivalently, a higher concentration of hydroxide ions (OH-).
03

Determine the pH of Acidic Solution

Since we are discussing an acid solution, by definition, its pH should be less than 7. This is due to the concentration of H+ ions, which, by definition of an acid, should be high in an acidic solution, leading to a lower pH value.

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Key Concepts

These are the key concepts you need to understand to accurately answer the question.

Acidic Solutions
An acidic solution is characterized by a higher concentration of hydrogen ions compared to water. This increased concentration of \(H^+\) ions leads to a pH value that is less than 7.
The lower the pH value, the stronger the acidity of the solution.

Acidity is a measure of the presence of \(H^+\) ions in a solution. It helps determine how acidic or "sour" a solution is. For example, lemon juice, vinegar, and gastric acid are common examples of acidic substances.

When discussing the pH of an acidic solution, it is important to remember:
  • pH < 7: indicates an acidic solution.
  • The presence of high \(H^+\) ion concentration results in a lower pH.
  • The strength of an acid is related to how fully it dissociates or releases \(H^+\) ions in water.
Understanding these aspects is crucial when studying changes in pH of various solutions.
Basic Solutions
Basic solutions, also known as alkaline solutions, are on the opposite end of the pH scale from acidic solutions. They have a pH greater than 7, indicating a lower concentration of hydrogen ions. Instead, they often have a higher concentration of hydroxide ions (OH鈦�).

These solutions can neutralize acids and are characterized by their bitter taste and slippery feel, such as soapy water or baking soda in solution. Basic solutions are essential in many chemical reactions and everyday cleaning products.

Key points about basic solutions include:
  • pH > 7: indicates a basic (alkaline) solution.
  • A higher concentration of \(OH^-\) ions compared to \(H^+\) ions.
  • They often neutralize acidic solutions when mixed.
Basics solutions play a critical role in balancing pH levels in various environments and processes.
Hydrogen Ion Concentration
The concentration of hydrogen ions is a fundamental aspect when discussing the pH scale. It serves as the driving factor behind whether a solution is acidic, neutral, or basic.

In any aqueous solution, \(H^+\) ions can exist either on their own or as part of hydronium ions (H鈧僌鈦�). The pH scale is essentially a logarithmic measure based on the concentration of these ions. It is calculated using the formula:
\[pH = -\log[H^+]\]

The concentration of hydrogen ions \(H^+\) affects the solution's pH in the following ways:
  • High \(H^+\): Leads to a low pH, indicating an acidic solution.
  • Low \(H^+\): Results in a high pH, indicating a basic solution.
  • Neutral solutions (pure water) have approximately \(10^{-7} M\) of \(H^+\).
Understanding the dynamics of hydrogen ion concentration is crucial in predicting and explaining the behavior of various solutions.

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Most popular questions from this chapter

Which of the following, when added to water, form a buffered solution? (a) \(\mathrm{HOCl}\) and \(\mathrm{NaCl}\) (b) \(\mathrm{HNO}_{2}\) and \(\mathrm{KNO}_{2}\) (c) \(\mathrm{CH}_{3} \mathrm{NH}_{2}\) and \(\mathrm{CH}_{3} \mathrm{NH}_{3} \mathrm{Cl}\)

Why is \(\mathrm{NH}_{3}\) a base but \(\mathrm{CH}_{4}\) is not? Is it possible for \(\mathrm{CH}_{4}\) to act as a Bronsted-Lowry base?

What is the \(\mathrm{pH}\) range for acidic solutions? For basic solutions?

What is the role of a buffer system in human blood?

How is a buffered solution different from a weak acid or a weak base dissolved in water?
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