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Chapter 16: Problem 53

The following are solution concentrations. Indicate whether each solution is acidic, basic, or neutral. a. \(5 \times 10^{-6} \mathrm{M} \mathrm{H}_{3} \mathrm{O}^{+}\) b. \(5 \times 10^{-9} \mathrm{M} \mathrm{OH}^{-}\) c. \(1 \times 10^{-7} \mathrm{M} \mathrm{OH}^{-}\) d. \(2 \times 10^{-9} \mathrm{M} \mathrm{H}_{3} \mathrm{O}^{+}\)

Short Answer

Expert verified
a. Acidic, b. Acidic, c. Neutral, d. Basic.

Step by step solution

01

Identify Acidic, Basic, and Neutral Conditions

In aqueous solutions, a solution is considered acidic if the concentration of hydronium ions (\(\text{H}_3\text{O}^+\)) is greater than \(1 \times 10^{-7}\,\text{M}\), basic if the hydroxide ion concentration (\(\text{OH}^-\)) is greater than \(1 \times 10^{-7}\,\text{M}\), and neutral if both are approximately \(1 \times 10^{-7}\,\text{M}\).
02

Analyze Condition A

For condition a, the concentration of \(\text{H}_3\text{O}^+\) is \(5 \times 10^{-6}\,\text{M}\). Since this value is greater than \(1 \times 10^{-7}\,\text{M}\), the solution is acidic.
03

Analyze Condition B

For condition b, the concentration of \(\text{OH}^-\) is \(5 \times 10^{-9}\,\text{M}\). Since this is less than \(1 \times 10^{-7}\,\text{M}\), the solution is more acidic and is therefore considered acidic.
04

Analyze Condition C

For condition c, the concentration of \(\text{OH}^-\) is \(1 \times 10^{-7}\,\text{M}\). This matches the concentration for neutral solutions, thus the solution is neutral.
05

Analyze Condition D

For condition d, the concentration of \(\text{H}_3\text{O}^+\) is \(2 \times 10^{-9}\,\text{M}\). This is less than \(1 \times 10^{-7}\,\text{M}\), suggesting a basic solution.

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Key Concepts

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

Acidic Solutions
Acidic solutions are those that have a higher concentration of hydronium ions ( H2O ) . These solutions have a pH value of less than 7, indicating acidity. In a typical acidic situation, the concentration of hydronium ions ( H2O ) is greater than the hydroxide ions ( OH- ).

For example, if the concentration of hydronium ions exceeds 1 脳 10^{-7} M, the solution shifts toward an acidic state. The solution becomes more acidic as this concentration increases.
- Acids like lemon juice and vinegar in everyday life are common examples. - Acids tend to taste sour and can conduct electricity due to the presence of charge carriers.
Measuring acidity can be achieved using a pH scale where each unit represents a tenfold change in ion concentration. Therefore, a solution with a pH of 3 is ten times more acidic than a pH of 4.
Basic Solutions
Basic solutions, also known as alkaline solutions, have a lower concentration of hydronium ions compared to hydroxide ions, resulting in a pH greater than 7. Unlike acidic solutions, basic solutions feel slippery and taste bitter.

Such solutions occur when the concentration of hydroxide ions ( OH- ) is greater than 1 脳 10^{-7} M. In these cases, the solution has more hydroxide ions relative to hydronium ions.
- Examples include household ammonia and baking soda solution. - Bases can also act as electrolytes, which means they can conduct electricity.
The pH scale measures alkalinity, just as it does acidity. For example, a pH of 12 is strongly basic and signifies a lower concentration of hydronium ions. Remember, as pH increases, the acidity decreases, and the basicity increases.
Neutral Solutions
Neutral solutions have a balance between hydronium ( H3O+ ) and hydroxide ( OH- ) ions, both at concentrations of approximately 1 脳 10^{-7} M. In such cases, the solution is neither acidic nor basic, and the pH is precisely 7.

An easy example of a neutral solution is pure water. - Pure water is a great example of neutrality in nature. - It is crucial in biological systems, as many reactions occur optimally at a neutral pH.
In practical scenarios, if you imagine diluting an acid with a base until they reach a point where they precisely neutralize each other. This results in a solution that is neither acidic nor basic. The balance in ion concentration is key to neutrality.

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Most popular questions from this chapter

An antiseptic solution at \(25^{\circ} \mathrm{C}\) has a hydroxide-ion concentration of \(8.4 \times 10^{-5} M\). Is the solution acidic, neutral, or basic?

What is meant by the \(\mathrm{pH}\) of a solution? Describe two ways of measuring \(\mathrm{pH}\).

Pure liquid ammonia ionizes in a way similar to that of water. a. Write the equilibrium reaction of liquid ammonia. b. Will sodium amide, \(\mathrm{NaNH}_{2}\), be an acid or a base in liquid ammonia? Why? c. Ammonium chloride can be used to titrate sodium amide in liquid ammonia. Write the chemical equation for the titration of sodium amide with ammonium chloride in liquid ammonia.

A 1.00-L aqueous solution contained \(5.80 \mathrm{~g}\) of sodium hydroxide, \(\mathrm{NaOH}\). What was the \(\mathrm{pH}\) of the solution at \(25^{\circ} \mathrm{C}\) ?

Define an acid and a base according to the Lewis concept. Give a chemical equation to illustrate.
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