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Chapter 9: Problem 11

The nature of the compound determines the form in which it exists in water. Rate the following solutes as strong electrolytes, weak electrolytes and nonelectrolytes in terms of their degree of ionization in water: a. vinegar b. \(\mathrm{K}_{2} \mathrm{CO}_{3}\) c. cellulose

Short Answer

Expert verified
Vinegar is a weak electrolyte, K鈧侰O鈧� is a strong electrolyte and cellulose is a nonelectrolyte.

Step by step solution

01

- Understand the Definitions

A strong electrolyte completely dissociates into ions in water. A weak electrolyte partially dissociates into ions in water and a nonelectrolyte does not dissociate into ions in water.
02

- Analyze Vinegar

Vinegar contains acetic acid (CH鈧僀OOH). Acetic acid is a weak acid, meaning it only partially ionizes in water. Therefore, vinegar is a weak electrolyte.
03

- Analyze K鈧侰O鈧�

Potassium carbonate (K鈧侰O鈧�) is an ionic compound that completely dissociates into potassium ions (K鈦�) and carbonate ions (CO鈧兟测伝) in water. Therefore, K鈧侰O鈧� is a strong electrolyte.
04

- Analyze Cellulose

Cellulose is a large polysaccharide, which is a type of carbohydrate. It does not dissociate into ions in water. Therefore, cellulose is a nonelectrolyte.

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Key Concepts

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

strong electrolytes
Strong electrolytes are substances that completely dissociate into ions when dissolved in water. This means they separate into their component ions. This full dissociation allows the solution to conduct electricity very well. Examples of strong electrolytes include:
- Potassium carbonate \(\text{{K}}_2\text{{CO}}_3\)
- Sodium chloride \(\text{{NaCl}}\)
- Hydrochloric acid \(\text{{HCl}}\)
weak electrolytes
Weak electrolytes only partially dissociate into ions in water. This partial dissociation means that only some molecules break apart into ions, while others remain intact. Because there are fewer ions, weak electrolyte solutions conduct electricity, but not as well as strong electrolyte solutions. Examples include:
- Acetic acid (present in vinegar) \(\text{{CH}}_3\text{{COOH}}\)
- Ammonia \(\text{{NH}}_3\)
- Hydrofluoric acid \(\text{{HF}}\)
nonelectrolytes
Nonelectrolytes are substances that do not dissociate into ions when dissolved in water. Their molecules remain intact, so nonelectrolyte solutions do not conduct electricity. These compounds typically include organic molecules that do not ionize. Examples of nonelectrolytes are:
- Cellulose
- Glucose \(\text{{C}}_6\text{{H}}_{12}\text{{O}}_6\)
- Ethanol \(\text{{C}}_2\text{{H}}_5\text{{OH}}\)
degree of ionization
The degree of ionization refers to the fraction of molecules that dissociate into ions in a solution. It is often represented as a percentage. For instance, if a substance is 100% ionized in water, it means all molecules break into ions, making it a strong electrolyte. Conversely, if only 10% of the molecules ionize, it is considered a weak electrolyte. Degree of ionization is an important concept when identifying whether a substance is a strong, weak, or non-electrolyte.
acetic acid
Acetic acid, with the chemical formula \(\text{{CH}}_3\text{{COOH}}\), is a common weak acid found in vinegar. In water, acetic acid only partially dissociates into ions \(\text{{CH}}_3\text{{COO}}^-\) and \(\text{{H}}^+\). This partial dissociation means that vinegar, which contains acetic acid, acts as a weak electrolyte. Therefore, it conducts electricity, but not as well as a strong electrolyte does.
potassium carbonate
Potassium carbonate, \(\text{{K}}_2\text{{CO}}_3\), is an ionic compound that consists of potassium ions \(\text{{K}}^+\) and carbonate ions \(\text{{CO}}_3^{2-}\). When dissolved in water, it fully dissociates into these ions, making it a strong electrolyte. This complete dissociation allows for excellent electrical conductivity in its aqueous solution.
cellulose
Cellulose is a complex carbohydrate or polysaccharide. It is made up of long chains of glucose molecules linked together. In water, cellulose does not dissociate or ionize; its molecules stay intact. This means it can be classified as a nonelectrolyte. Because there are no ions present, a solution of cellulose does not conduct electricity.

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Most popular questions from this chapter

A solution is prepared with \(5.0 \mathrm{~g}\) of \(\mathrm{HCl}\) and \(195.0 \mathrm{~g}\) of \(\mathrm{H}_{2} \mathrm{O}\). The HCl solution has a density of \(1.49 \mathrm{~g} / \mathrm{mL}\). (9.4) a. What is the mass percent \((\mathrm{m} / \mathrm{m})\) of the \(\mathrm{HCl}\) solution? b. What is the total volume, in milliliters, of the solution? c. What is the mass/volume percent (m/v) of the solution? d. What is the molarity of the solution?

What volume, in \(\mathrm{mL}\), of \(2.50 \mathrm{M}\) of sodium chloride solution is needed to obtain \(3.0 \mathrm{~g}\) of \(\mathrm{NaCl}\) by evaporation? (9.4)

For each of the following solutions, calculate the: a. grams of \(2.0 \%(\mathrm{~m} / \mathrm{m}) \mathrm{NaCl}\) solution that contains \(7.50 \mathrm{~g}\) of \(\mathrm{NaCl}\) b. milliliters of \(25 \%\) (m/v) NaF solution that contains \(4.0 \mathrm{~g}\) of NaF c. milliliters of \(8.0 \%\) (v/v) ethanol solution that contains \(20.0 \mathrm{~mL}\) of ethanol

What is the initial volume, in milliliters, needed to prepare each of the following diluted solutions? (9.5) a. \(250 \mathrm{~mL}\) of \(3.0 \%(\mathrm{~m} / \mathrm{v}) \mathrm{HCl}\) from \(10.0 \%(\mathrm{~m} / \mathrm{v}) \mathrm{HCl}\) b. \(500 . \mathrm{mL}\) of \(0.90 \%(\mathrm{~m} / \mathrm{v}) \mathrm{NaCl}\) from \(5.0 \%(\mathrm{~m} / \mathrm{v}) \mathrm{NaCl}\) c. \(350 . \mathrm{mL}\) of \(2.00 \mathrm{M} \mathrm{NaOH}\) from \(6.00 \mathrm{M} \mathrm{NaOH}\)

Determine the final volume, in milliliters, of each of the following: a. a \(1.5 \mathrm{M} \mathrm{HCl}\) solution prepared from \(20.0 \mathrm{~mL}\) of a \(6.0 \mathrm{M}\) HCl solution b. a \(2.0 \%\) (m/v) \(\mathrm{LiCl}\) solution prepared from \(50.0 \mathrm{~mL}\) of a \(10.0 \%(\mathrm{~m} / \mathrm{v}) \mathrm{LiCl}\) solution c. a \(0.500 \mathrm{M} \mathrm{H}_{3} \mathrm{PO}_{4}\) solution prepared from \(50.0 \mathrm{~mL}\) of a \(6.00 \mathrm{M} \mathrm{H}_{3} \mathrm{PO}_{4}\) solution d. a \(5.0 \%(\mathrm{~m} / \mathrm{v})\) glucose solution prepared from \(75 \mathrm{~mL}\) of a \(12 \%(\mathrm{~m} / \mathrm{v})\) glucose solution
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