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Chapter 4: Problem 38

Classify each of the following aqueous solutions as a nonelectrolyte, weak electrolyte, or strong electrolyte: (a) \(\mathrm{PbCl}_{2}\), (b) \(\mathrm{N}\left(\mathrm{CH}_{3}\right)_{3}\), (c) \(\mathrm{CsOH}\) (d) \(\mathrm{H}_{2} \mathrm{~S}\), (e) \(\mathrm{CrCl}_{2}\) (f) \(\mathrm{Ni}\left(\mathrm{CH}_{3} \mathrm{COO}\right)_{2}\)

Short Answer

Expert verified
(a) Weak electrolyte, (b) Weak electrolyte, (c) Strong electrolyte, (d) Weak electrolyte, (e) Strong electrolyte, (f) Strong electrolyte.

Step by step solution

01

Understand Electrolytes

Electrolytes are substances that dissolve in water to produce ions, conducting electricity. Strong electrolytes dissociate completely into ions, weak electrolytes partially dissociate, and nonelectrolytes do not dissociate at all.
02

Analyzing Lead Chloride  (PbCl_2)

Lead chloride is a slightly soluble salt, meaning only a small amount dissolves and dissociates into ions in water. Thus, it is a weak electrolyte because of its limited ion formation.
03

Analyzing Trimethylamine  (N(CH_3)_3)

Trimethylamine is a weak base. When dissolved in water, it accepts a proton and partially ionizes, forming ions. Thus, it is classified as a weak electrolyte.
04

Analyzing Cesium Hydroxide  (CsOH)

Cesium hydroxide is a strong base and fully dissociates into cesium and hydroxide ions in water. Therefore, it is classified as a strong electrolyte.
05

Analyzing Hydrogen Sulfide  (H_2S)

Hydrogen sulfide is a weak acid that partially dissociates into hydrogen and sulfide ions in water, making it a weak electrolyte.
06

Analyzing Chromium (II) Chloride  (CrCl_2)

Chromium (II) chloride is a salt that dissociates completely in water, like many chlorides, so it is considered a strong electrolyte.
07

Analyzing Nickel (II) Acetate  (Ni(CH_3COO)_2)

Nickel (II) acetate dissociates in water to form nickel ions and acetate ions. As it dissociates completely, it is classified as a strong electrolyte.

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Key Concepts

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

Nonelectrolyte
When a substance dissolves in water but does not produce any ions, it is called a nonelectrolyte. Nonelectrolytes do not conduct electricity in aqueous solutions.
For instance, common household substances like sugar or urea dissolve in water, but they do not form ions.
  • In such solutions, the molecules stay together and do not separate into charged particles.
  • This means the solution does not carry an electrical current.
Understanding nonelectrolytes is important in distinguishing them from substances that can conduct electricity when dissolved in water.
Weak Electrolyte
Weak electrolytes are substances that only partially dissociate into ions when dissolved in water. This means they conduct electricity weakly.
When you dissolve a weak electrolyte in water, only a small fraction of its molecules split into ions. The rest remain intact.
  • Examples of weak electrolytes include acetic acid and ammonia.
  • In the given exercise, substances like \(\text{N(CH}_3\text{)}_3\) and \(\text{H}_2\text{S}\) fall into this category due to their limited ionization.
Knowing about weak electrolytes helps in understanding how different substances influence the conductivity of solutions.
Strong Electrolyte
Strong electrolytes completely dissociate into ions when they dissolve in water. This complete ionization allows the solution to conduct electricity very well.
Strong acids, strong bases, and most salts fall under this category.
  • Common examples include sodium chloride (NaCl) and sulfuric acid (\(\text{H}_2\text{SO}_4\)).
  • In the textbook exercise, \(\text{CsOH}\) and \(\text{CrCl}_2\) are strong electrolytes as they fully dissociate, producing a high concentration of ions.
Understanding strong electrolytes is crucial for predicting how substances will behave in water as they significantly affect the solution's electrical conductivity.
Aqueous Solutions
An aqueous solution is formed when a substance dissolves in water. The water serves as the solvent in these solutions.
Water's ability to dissolve a wide range of substances makes it a universal solvent. This is why so many chemical reactions take place in aqueous solutions.
  • When substances dissolve, they can either form a molecular solution or dissociate into ions.
  • The behavior of dissolved substances can vary greatly and is key to categorizing them as electrolytes or nonelectrolytes.
Aqueous solutions are a fundamental concept in chemistry, helping to understand how different substances interact with water and each other.
Dissociation
Dissociation is the process of a compound separating into its constituent ions when dissolved in water.
This process is crucial for understanding how substances behave in solution.
  • In strong electrolytes, dissociation occurs completely, resulting in free ions that conduct electricity well.
  • Weak electrolytes only partially dissociate, leading to a balance between intact molecules and ions in solution.
  • Nonelectrolytes do not dissociate at all when dissolved.
The degree of dissociation is a key criterion in classifying substances as strong, weak, or non-electrolytes, and it significantly influences the properties of the solution.

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Most popular questions from this chapter

You make 1.000 L of an aqueous solution that contains \(35.0 \mathrm{~g}\) of sucrose \(\left(\mathrm{C}_{12} \mathrm{H}_{22} \mathrm{O}_{11}\right),(\mathbf{a})\) What is the molarity of sucrose in this solution? (b) How many liters of water would you have to add to this solution to reduce the molarity you calculated in part (a) by a factor of two?

Pure acetic acid, known as glacial acetic acid, is a liquid with a density of \(1.049 \mathrm{~g} / \mathrm{mL}\) at \(25^{\circ} \mathrm{C}\). Calculate the molarity of a solution of acetic acid made by dissolving \(20.00 \mathrm{~mL}\) of glacial acetic acid at \(25^{\circ} \mathrm{C}\) in enough water to make \(250.0 \mathrm{~mL}\) of solution.

When carbon dioxide dissolves in water, it is in equilibrium with carbonic acid \(\mathrm{H}_{2} \mathrm{CO}_{3},\) which is a weak electrolyte. What solutes are present in aqueous solution of this compound? Write the chemical equation for the ionization of \(\mathrm{H}_{2} \mathrm{CO}_{3}\)

The average adult human male has a total blood volume of 5.0 \(\mathrm{L}\). If the concentration of sodium ion in this average individual is \(0.135 \mathrm{M},\) what is the mass of sodium ion circulating in the blood?

You are titrating an acidic solution with a basic one, and just realized you forgot to add the indicator that tells you when the equivalence point is reached. In this titration, the indicator turns blue at the equivalence point from an initially colorless solution. You quickly grab a bottle of indicator and add some to your titration beaker, and the whole solution turns dark blue. What do you do now?
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