Which of the following is a nonelectrolyte? Please state why or why not for each. Thanks
a) NaOH
b) HNO3
c) C2H6O (ethanol)
d) KF
e) CH3COOH (acetic acid)
The Correct Answer and Explanation is:
Certainly! Let’s analyze each option carefully to determine which is a nonelectrolyte, along with explanations for all choices.
The question: Which of the following is a nonelectrolyte?
Options:
a) NaOH
b) HNO3
c) C2H6O (ethanol)
d) KF
e) CH3COOH (acetic acid)
Definitions first:
- Electrolyte: A substance that dissociates into ions in water and conducts electricity.
- Strong electrolytes dissociate completely.
- Weak electrolytes dissociate partially.
- Nonelectrolyte: A substance that does not dissociate into ions in water and therefore does not conduct electricity.
Analysis of each:
a) NaOH (Sodium hydroxide)
- Type: Strong base, ionic compound.
- Behavior in water: Completely dissociates into Na⁺ and OH⁻ ions.
- Electrolyte or not?
Strong electrolyte. Because it fully dissociates and conducts electricity well.
b) HNO3 (Nitric acid)
- Type: Strong acid.
- Behavior in water: Completely dissociates into H⁺ and NO3⁻ ions.
- Electrolyte or not?
Strong electrolyte. Fully ionizes in solution and conducts electricity.
c) C2H6O (Ethanol)
- Type: Molecular compound (organic alcohol).
- Behavior in water: Does not dissociate into ions; it dissolves as intact molecules.
- Electrolyte or not?
Nonelectrolyte. Ethanol does not produce ions; it dissolves but doesn’t conduct electricity.
d) KF (Potassium fluoride)
- Type: Ionic compound.
- Behavior in water: Dissociates completely into K⁺ and F⁻ ions.
- Electrolyte or not?
Strong electrolyte. It dissociates completely and conducts electricity.
e) CH3COOH (Acetic acid)
- Type: Weak acid.
- Behavior in water: Partially ionizes into CH3COO⁻ and H⁺ ions.
- Electrolyte or not?
Weak electrolyte. Because it ionizes partially but still conducts some electricity.
Correct answer:
c) C2H6O (ethanol) is the nonelectrolyte.
Detailed explanation (300+ words):
Electrolytes are substances that dissociate into ions when dissolved in water, allowing the solution to conduct electricity. Strong electrolytes fully dissociate, producing a high concentration of ions. Weak electrolytes partially dissociate, resulting in fewer ions and weaker conductivity. Nonelectrolytes, on the other hand, dissolve in water but do not produce ions, so they do not conduct electricity.
Sodium hydroxide (NaOH) is a strong base and a classic example of a strong electrolyte. When dissolved in water, NaOH dissociates completely into sodium ions (Na⁺) and hydroxide ions (OH⁻). This complete ionization results in a highly conductive solution.
Similarly, nitric acid (HNO3) is a strong acid and fully ionizes into hydrogen ions (H⁺) and nitrate ions (NO3⁻) in water, making it a strong electrolyte.
Potassium fluoride (KF) is an ionic salt that dissolves in water to release potassium ions (K⁺) and fluoride ions (F⁻). This full dissociation also makes KF a strong electrolyte.
Acetic acid (CH3COOH), although an acid, is a weak electrolyte because it only partially dissociates in water into acetate ions (CH3COO⁻) and hydrogen ions (H⁺). This partial ionization produces fewer ions compared to strong electrolytes, but enough to allow some electrical conductivity.
In contrast, ethanol (C2H6O) is a molecular compound and does not dissociate into ions when dissolved in water. Instead, it remains as intact molecules. Because ions are necessary for conducting electricity in solutions, ethanol solutions do not conduct electricity, classifying ethanol as a nonelectrolyte.
Thus, ethanol stands out as the only nonelectrolyte among the options given, while all the others are either strong or weak electrolytes.