Strong And Weak Electrolytes Quiz
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What are the most familiar electrolytes?
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Acids
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Bases
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Salts
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All of the above
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What are strong and weak electrolytes? What is the difference between the two terms? Can you tell if a given electrolyte is weak or strong? Attempt this quiz below and see what you know about electrolytes. Here, we will not tell you anything about electrolytes as it's time to check your knowledge regarding these substances. Let's see how much a See morescore you will get on this chemistry quiz. Start playing the quiz, then!
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- 2.
Substances whose solutions conduct electricity are called
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Electrolytes
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Biomolecules
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Polymers
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All of the above
Correct Answer
A. ElectrolytesExplanation
Electrolytes are substances that, when dissolved in water or melted, produce ions that can conduct electricity. These ions are responsible for carrying electric current through the solution. Biomolecules and polymers are not typically known for their ability to conduct electricity, so they are not considered electrolytes. Therefore, the correct answer is electrolytes.Rate this question:
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- 3.
Is H2SO3 a strong or weak electrolyte?
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Strong
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Weak
Correct Answer
A. WeakExplanation
H2SO3 is a weak electrolyte because it only partially dissociates into ions when dissolved in water. Weak electrolytes conduct electricity to a lesser extent compared to strong electrolytes, which completely dissociate into ions.Rate this question:
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- 4.
What is the difference between a strong and a weak electrolyte?
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A strong electrolyte does not completely dissociate in solution, whereas a weak electrolyte does.
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A strong electrolyte completely dissociates in solution, whereas a weak electrolyte does not.
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Both are the same.
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None of the above
Correct Answer
A. A strong electrolyte completely dissociates in solution, whereas a weak electrolyte does not.Explanation
A strong electrolyte is a substance that completely dissociates into ions when dissolved in a solution, meaning that it breaks apart into its constituent ions. This results in a high concentration of ions in the solution, allowing for efficient conduction of electricity. On the other hand, a weak electrolyte only partially dissociates in solution, meaning that only a fraction of the substance breaks apart into ions. This results in a lower concentration of ions in the solution, leading to less efficient conduction of electricity. Therefore, the correct answer is that a strong electrolyte completely dissociates in solution, whereas a weak electrolyte does not.Rate this question:
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- 5.
Strong acids, strong bases, and ionic salts are strong electrolytes.
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True
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False
Correct Answer
A. TrueExplanation
Strong acids, strong bases, and ionic salts are considered strong electrolytes because they completely dissociate into ions when dissolved in water. This means that they conduct electricity very effectively, as the presence of ions allows for the flow of electric current. In contrast, weak acids, weak bases, and covalent compounds do not dissociate completely in water and are considered weak electrolytes or non-electrolytes. Therefore, the statement that strong acids, strong bases, and ionic salts are strong electrolytes is true.Rate this question:
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- 6.
What are examples of weak electrolytes?
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Acetic acid
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Ammonia
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Phosphoric acid
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All of the above
Correct Answer
A. All of the aboveExplanation
All of the given options, acetic acid, ammonia, and phosphoric acid, are examples of weak electrolytes. Weak electrolytes are substances that partially dissociate into ions when dissolved in water, resulting in a weak electrical conductivity. These substances do not completely break apart into ions like strong electrolytes, but only a fraction of the molecules dissociate. Acetic acid, ammonia, and phosphoric acid all exhibit this behavior, making them weak electrolytes.Rate this question:
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- 7.
Dissociation and dissolution are the same things.
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True
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False
Correct Answer
A. FalseExplanation
Dissociation and dissolution are not the same things. Dissociation refers to the separation of ions in a compound when it is dissolved in a solvent, while dissolution refers to the process of a solid substance dissolving in a liquid solvent. Although both involve the separation of components, dissociation specifically refers to the separation of ions, whereas dissolution is a broader term that encompasses the dissolution of any substance in a solvent. Therefore, the statement that dissociation and dissolution are the same things is false.Rate this question:
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- 8.
What makes acetic acid a weak electrolyte?
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The small amount of water
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The small amount of product (ethanoate)
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A large amount of methane
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All of the above
Correct Answer
A. The small amount of product (ethanoate)Explanation
Acetic acid is a weak electrolyte because it only partially ionizes in water, producing a small amount of ethanoate ions. Weak electrolytes only conduct electricity to a limited extent, as they only produce a small number of ions when dissolved in water. The small amount of product (ethanoate) formed from the ionization process is what makes acetic acid a weak electrolyte.Rate this question:
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- 9.
Most compounds that contain __________ are weak electrolytes.
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Oxygen
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Hydrogen
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Nitrogen
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All of the above
Correct Answer
A. NitrogenExplanation
Most compounds that contain nitrogen are weak electrolytes because nitrogen is a nonmetal and tends to form covalent bonds with other elements. Covalent compounds do not dissociate into ions when dissolved in water, which is necessary for a substance to conduct electricity. Therefore, compounds containing nitrogen are not able to conduct electricity effectively, making them weak electrolytes.Rate this question:
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- 10.
What is/are true regarding nonelectrolytes?
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These do not break into ions in water.
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Most carbon compounds, such as sugars, are nonelectrolytes.
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Both A and B
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None of the above
Correct Answer
A. Both A and BExplanation
Both A and B are true regarding nonelectrolytes. Nonelectrolytes do not break into ions in water, and most carbon compounds, such as sugars, are nonelectrolytes.Rate this question:
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Current Version
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Mar 05, 2024Quiz Edited by
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Expert Reviewed by
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Dec 09, 2022Quiz Created by
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