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Chapter 9: Problem 14

Which of the following is/are correct? I. NaF is an electrolyte. II. Glucose is a nonelectrolyte. III. \(\mathrm{CH}_3 \mathrm{OH}\) is a weak electrolyte. IV. \(\mathrm{CH}_3 \mathrm{CH}_2 \mathrm{COOH}\) is a weak electrolyte. A. I, III, and IV only B. I and II only C. II, and IV only D. I, II, and IV only

Short Answer

Expert verified
D. I, II, and IV only

Step by step solution

01

Understand Electrolytes

Electrolytes are substances that dissociate into ions in solution, making the solution capable of conducting electricity. Strong electrolytes dissociate completely, while weak electrolytes dissociate partially.
02

Classify NaF as Electrolyte or Nonelectrolyte

Sodium fluoride (NaF) is an ionic compound that dissociates completely in water, which makes it an electrolyte. Thus, statement I is correct.
03

Classify Glucose as Electrolyte or Nonelectrolyte

Glucose (C6H12O6) is a covalent compound that does not dissociate into ions in solution. It is a nonelectrolyte. Thus, statement II is correct.
04

Examine \(\text{CH}_3 \text{OH}\) as Strong, Weak Electrolyte or Nonelectrolyte

Methanol (CH3OH) is a covalent compound and does not dissociate into ions significantly in water. It is considered a nonelectrolyte, so statement III is incorrect.
05

Evaluate \(\text{CH}_3 \text{CH}_2 \text{COOH}\) as Strong, Weak Electrolyte or Nonelectrolyte

Propanoic acid (CH3CH2COOH) is a weak acid and only partially dissociates in water, making it a weak electrolyte. Thus, statement IV is correct.
06

Determine Correct Statements

From the analysis, statements I, II, and IV are correct. Therefore, the correct answer is D.

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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 break apart into their respective positive and negative ions in solution. Because these ions freely move and carry electric charge, solutions of strong electrolytes conduct electricity very well. Examples of strong electrolytes include:
  • Sodium chloride (NaCl)
  • Potassium nitrate (KNO3)
  • Hydrochloric acid (HCl)
In the case of sodium fluoride (NaF) mentioned in the exercise, it is an ionic compound and dissociates completely in water to form sodium (Na鈦�) and fluoride ions (F鈦�). Thus, NaF is a strong electrolyte.
Weak Electrolytes
Weak electrolytes are substances that only partially dissociate into ions in water. This means a significant portion of the substance remains in its original form, with only a small fraction turning into ions. As a result, solutions of weak electrolytes do not conduct electricity as well as strong electrolytes. Common examples include:
  • Acetic acid (CH3COOH)
  • Ammonium hydroxide (NH4OH)
  • Propanoic acid (CH3CH2COOH)
In the given exercise, propanoic acid is a weak electrolyte because only a small percentage of the molecules dissociate into ions (CH3CH2COO鈦� and H鈦�) when dissolved in water.
Nonelectrolytes
Nonelectrolytes are substances that do not dissociate into ions at all in solution. They remain intact as molecules, and therefore, their solutions do not conduct electricity. These are typically covalent compounds. Examples include:
  • Glucose (C6H12O6)
  • Ethanol (C2H5OH)
  • Methanol (CH3OH)
According to the exercise, glucose is classified as a nonelectrolyte because it does not form ions in solution. Similarly, methanol (CH3OH) is also categorized as a nonelectrolyte, contrary to the incorrect classification in the exercise.
Dissociation of Ionic Compounds
The process of dissociation involves the splitting of an ionic compound into its constituent ions when dissolved in water. This property of ionic compounds is what enables the solution to conduct electricity. The degree of dissociation determines whether an electrolyte is strong or weak. For strong electrolytes, dissociation is complete, while for weak electrolytes, it is only partial. For instance:
In the case of NaF, the dissociation equation in water is:
\[ \text{NaF} \rightarrow \text{Na}^+ + \text{F}^- \] This complete dissociation characterizes strong electrolytes. On the other hand, weak electrolytes like propanoic acid (\text{CH3CH2COOH}) dissociate as follows:
\[ \text{CH3CH2COOH} \rightleftharpoons \text{CH3CH2COO}^- + \text{H}^+ \] Here, the double arrow indicates that the dissociation is not complete, illustrating the behavior of weak electrolytes.

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Most popular questions from this chapter

Lead is a dangerous element that exists in the environment in large quantities due to man-made pollution. Lead poisoning has many symptoms, including mental retardation in children. If a body of water is polluted with lead ions at \(30 \mathrm{ppb}\) (parts per billion), what is the concentration of lead in molarity? (Density of water is \(1 \mathrm{~g} / \mathrm{mL}\), ppb equals grams per \(10^9\) grams of solution.) A. \(6.2 \times 10^{-7} \mathrm{M} \mathrm{Pb}^{2+}\) B. \(1.4 \times 10^{-10} \mathrm{M} \mathrm{Pb}^{2+}\) C. \(1.4 \times 10^{-7} \mathrm{M} \mathrm{Pb}^{2+}\) D. \(6.2 \times 10^{-6} \mathrm{M} \mathrm{Pb}^{2+}\)

Which of the following combinations of liquids would be expected to have a vapor pressure higher than the vapor pressure that would be predicted by Raoult's law? A. Ethanol and hexane B. Acetone and water C. Isopropanol and methanol D. Nitric acid and water

Which phase of solvent and solute, respectively, can form a solution? I. Solid solvent, gaseous solute II. Solid solvent, solid solute III. Gaseous solvent, gaseous solute A. I and II only B. II and III only C. I and III only D. I, II, and III

Detergents are compounds that are dissolved in water. However, they are also able to dissolve hydrophobic stains, such as oil and grease in clothing and other fabrics. How are these compounds able to fulfill both hydrophilic and hydrophobic functions? A. They contain a hydrophobic core molecule encased in a hydrophilic shell. B. They can ionize into two parts; one part is ionic, and the other part is hydrophobic. C. They have two states; in water they are ionic, and in hydrophobic solvents they form nonpolar ring structures. D. They have two functionally distinct parts; one side is a hydrophobic chain, and the other end is polar and ionic.

A \(0.01 \mathrm{M}\) solution of a nonelectrolyte has an osmotic pressure of \(15.0 \mathrm{~mm} \mathrm{Hg}\). What is the osmotic pressure of a \(0.02 \mathrm{M}\) solution of \(\mathrm{Mg}\left(\mathrm{NO}_3\right)_2\) ? The temperature of both solutions is the same. A. \(7.5 \mathrm{~mm} \mathrm{Hg}\) B. \(30 \mathrm{~mm} \mathrm{Hg}\) C. \(45 \mathrm{~mm} \mathrm{Hg}\) D. \(90 \mathrm{~mm} \mathrm{Hg}\)
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