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Chapter 16: Problem 58

Which of the following \(\mathrm{pH}\) values indicate an acidic solution at \(25^{\circ} \mathrm{C}\) ? Which are basic and which are neutral? a. \(12.9\) b. \(8.9\) c. \(5.1\) d. \(1.6\)

Short Answer

Expert verified
a is basic, b is basic, c and d are acidic. No neutral solutions.

Step by step solution

01

Understanding pH Scale

The pH scale ranges from 0 to 14, where a pH of 7 is considered neutral, pH less than 7 is acidic, and pH greater than 7 is basic (alkaline). At \(25^{\circ} \mathrm{C}\), neutral solutions have a pH of exactly 7.0.
02

Identifying Acidic Values

Solutions with a pH less than 7 are acidic. Thus, if the pH is less than 7, we classify it as acidic.
03

Identifying Basic Values

Solutions with a pH greater than 7 are basic. If the pH is more than 7, the solution is classified as basic.
04

Identifying Neutral Value

If a solution's pH is exactly 7, it is classified as neutral.
05

Answering the Exercise

a. \(12.9\) is basic because it is greater than 7. b. \(8.9\) is basic because it is greater than 7. c. \(5.1\) is acidic because it is less than 7. d. \(1.6\) is acidic because it is less than 7. None of the given pH values are exactly 7, so there is no neutral solution here.

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Key Concepts

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

Acidic Solutions
When we talk about acidic solutions, we're referring to solutions that possess a pH level less than 7. These solutions are characterized by a higher concentration of hydrogen ions (H鈦�) compared to hydroxide ions (OH鈦�).

In daily life, many substances are acidic. For example, lemon juice and vinegar both have a low pH value. Some key points about acidic solutions include:

  • pH less than 7
  • Higher concentration of H鈦� ions
  • Tastes sour
  • Can conduct electricity
In the original exercise, the pH values of 5.1 and 1.6 indicate acidic solutions. This is because both values are below 7. Remember, the lower the pH value, the more acidic the solution. A strong acid like battery acid can have a pH level very close to 0, which makes it highly corrosive.
Basic Solutions
Basic solutions, also known as alkaline solutions, are characterized by having a pH level greater than 7. These solutions have more hydroxide ions (OH鈦�) than hydrogen ions (H鈦�).

Many household cleaning products are basic due to this higher pH value, which helps them break down oils and fats. Let's break down the essential features of basic solutions:

  • pH greater than 7
  • Higher concentration of OH鈦� ions
  • Tastes bitter and feels slippery
  • Can also conduct electricity
In the provided exercise, the values 12.9 and 8.9 are examples of basic solutions, as they are both above the neutral pH of 7. A typical strong base, like lye, can have a pH approaching 14, making it just as aggressive as strong acids, but in the opposite way.
Neutral Solutions
The concept of a neutral solution is simple yet important. Neutral solutions have a pH level of exactly 7. This balance occurs when the concentration of hydrogen ions (H鈦�) equals the concentration of hydroxide ions (OH鈦�).

Pure water is the most classic example of a neutral solution. Here are some characteristics:

  • pH exactly 7
  • Equal concentration of H鈦� and OH鈦� ions
  • Generally tasteless
The original exercise didn't present any pH values of exactly 7, which means no neutral solutions were listed. It's good to know that, in real-world conditions, factors such as temperature and contamination can slightly shift the pH of water, but the neutral pH definition still holds true in theoretical contexts.

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Most popular questions from this chapter

List the following compounds in order of increasing acid strength: \(\mathrm{HBr}, \mathrm{H}_{2} \mathrm{Se}, \mathrm{H}_{2} \mathrm{~S}\).

Give two important factors that determine the strength of an acid. How does an increase in each factor affect the acid strength?

For the following reactions, label each species as an acid or a base. Indicate the species that are conjugates of one another. a. \(\mathrm{HSO}_{4}^{-}+\mathrm{NH}_{3} \rightleftharpoons \mathrm{SO}_{4}^{2-}+\mathrm{NH}_{4}^{+}\) b. \(\mathrm{HPO}_{4}^{2-}+\mathrm{NH}_{4}^{+} \rightleftharpoons \mathrm{H}_{2} \mathrm{PO}_{4}^{-}+\mathrm{NH}_{3}\) c. \(\mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{3+}+\mathrm{H}_{2} \mathrm{O} \rightleftharpoons \mathrm{Al}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{OH}^{2+}+\mathrm{H}_{3} \mathrm{O}^{+}\) d. \(\mathrm{SO}_{3}^{2-}+\mathrm{NH}_{4}^{+} \rightleftharpoons \mathrm{HSO}_{3}^{-}+\mathrm{NH}_{3}\)

Some lemon juice has a hydronium-ion concentration of \(5.0 \times 10^{-3} M .\) What is the \(\mathrm{pH}\) of the lemon juice?

Give the conjugate acid to each of the following species regarded as bases. a. \(\mathrm{HS}^{-}\) b. \(\mathrm{NH}_{2}^{-}\) c. \(\mathrm{BrO}_{2}^{-}\) d. \(\mathrm{N}_{2} \mathrm{H}_{4}\)
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