Which of the following substances will produce a solution that does not conduct electricity when it dissolves in water? (LO 4.6) (a) NaOH (b) HNO3 (c) Na2SO4 (d) CH3OH

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Identify the nature of each substance: Determine if each substance is an electrolyte or a non-electrolyte.

Understand electrolytes: Electrolytes are substances that dissociate into ions in solution, allowing the solution to conduct electricity.

Analyze each option: (a) NaOH is a strong base and dissociates completely into Na+ and OH- ions. (b) HNO3 is a strong acid and dissociates completely into H+ and NO3- ions. (c) Na2SO4 is a salt and dissociates into 2 Na+ and SO4^2- ions.

Consider non-electrolytes: Non-electrolytes do not dissociate into ions in solution and therefore do not conduct electricity.

Evaluate option (d) CH3OH: Methanol (CH3OH) is a molecular compound that does not dissociate into ions in water, making it a non-electrolyte.

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Electrolytes

Electrolytes are substances that dissociate into ions when dissolved in water, allowing the solution to conduct electricity. Strong electrolytes, like NaOH and HNO3, completely ionize in solution, while weak electrolytes partially ionize. Understanding the nature of electrolytes is crucial for predicting whether a solution will conduct electricity.

Non-electrolytes

Non-electrolytes are substances that do not dissociate into ions in solution and therefore do not conduct electricity. An example is CH3OH (methanol), which dissolves in water but remains as neutral molecules. Recognizing non-electrolytes is essential for determining which substances will not produce conductive solutions.

Dissociation in Water

Dissociation in water refers to the process where ionic compounds break apart into their constituent ions when mixed with water. This process is key to understanding how different substances behave in aqueous solutions. For instance, Na2SO4 dissociates into Na+ and SO4^2- ions, contributing to electrical conductivity, while non-ionic compounds like CH3OH do not.