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Chapter 13: Problem 66

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

Short Answer

Expert verified
The pH range for acidic solutions is from 0 to 7 but not including 7. The pH range for basic solutions is from 7 to 14 but not including 7.

Step by step solution

01

Define the pH scale

The pH scale is a measure of how acidic or basic a substance is. It ranges from 0 to 14.
02

Identify the range for acidic solutions

On the pH scale, solutions that have a pH less than 7 are considered acidic. Therefore, the range for acidic solutions is \(0 < \mathrm{pH} < 7 \).
03

Identify the range for basic solutions

On the pH scale, solutions that have a pH greater than 7 are considered basic. Therefore, the range for basic solutions is \( 7 < \mathrm{pH} < 14 \).

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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 one where the concentration of hydrogen ions (H鈦�) is higher than in pure water. These solutions have a pH value that is less than 7. The pH scale ranges from 0 to 14, and an acidic solution falls in the range between 0 and just below 7. It's important to note that the lower the pH, the stronger the acidity of the solution.

Here are some key points about acidic solutions:
  • They generally taste sour (like vinegar or lemon juice).
  • They can conduct electricity as they release hydrogen ions in solution.
  • Examples include gastric acid and citrus fruits.
Understanding the nature of acidic solutions is essential in various fields such as chemistry, biology, and environmental science.
Basic Solutions
Basic solutions, also known as alkaline solutions, have a lower concentration of hydrogen ions than pure water, and instead contain more hydroxide ions (OH鈦�). These solutions have a pH greater than 7. As you move up the pH scale towards 14, the basicity of the solution increases. Basic solutions play a vital role in many industrial processes and daily life activities.

Consider these characteristics of basic solutions:
  • They often feel slippery to the touch (like soap).
  • Basic solutions usually have a bitter taste.
  • Common examples include baking soda and household ammonia.
Grasping the concept of basic solutions is crucial, especially for understanding chemical reactions and maintaining safe environments in various applications.
pH Range
The pH range is a scale used to specify how acidic or basic a water-based solution is. It spans from 0 to 14, with 7 being neutral鈥攑ure water is a perfect example of a neutral substance. The pH scale is logarithmic, meaning each whole number pH change represents a tenfold change in acidity or basicity.
  • pH less than 7 indicates acidity.
  • pH greater than 7 indicates basicity.
  • Each step down the scale signifies ten times more acidic, and up, ten times more basic.
Understanding the pH range is pivotal for tasks such as managing aquarium water, soil for agriculture, and maintaining proper levels in swimming pools and drinking water systems. By learning how to manipulate the pH, better control of chemical environments can be achieved.

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Most popular questions from this chapter

A buffer system used to maintain solution pH values around 12 to 13 is prepared by adding similar concentrations of \(\mathrm{Na}_{2} \mathrm{HPO}_{4}\) and \(\mathrm{Na}_{3} \mathrm{PO}_{4}\) to water. (a) Write a balanced equation showing the acid and conjugate base in equilibrium. Omit spectator ions. (b) Describe how this buffer system prevents large \(\mathrm{pH}\) changes when an acid is added.

What is the \(\mathrm{H}_{3} \mathrm{O}^{+}\)concentration in each of the following solutions? (a) lake water, \(\mathrm{pOH}=6.00\) (b) coffee, \(\mathrm{pOH}=8.90\) (c) borax, pOH \(=4.50\)

Can a solution have a pH less than 0 or greater than 14 ? Explain.

Write an equation that shows what happens when \(\mathrm{Ba}(\mathrm{OH})_{2}\) dissolves in water. What is the \(\mathrm{pH}\) of \(0.01 M\) \(\mathrm{Ba}(\mathrm{OH})_{2}\) ?

Which of the following are amphoteric species? (a) \(\mathrm{NH}_{4}{ }^{+}\) (b) \(\mathrm{HBO}_{3}{ }^{2-}\) (c) \(\mathrm{H}_{2} \mathrm{PO}_{4}^{-}\)
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