Question

Which of the following best explains the difference between a 0.1 molar aqueous solution of sodium sulfate and a 0.1 molar aqueous solution of sodium chloride in terms of their conductivity of electricity?

1) Sodium sulfate dissociates into more ions in solution than sodium chloride
2) Sodium sulfate has a higher molar mass than sodium chloride
3) Sodium sulfate has a higher boiling point than sodium chloride
4) Sodium sulfate has a higher solubility in water than sodium chloride

Answer 1

The 0.1 molar aqueous solution of sodium sulfate has greater conductivity than the sodium chloride solution because it dissociates into more ions with higher charges, leading to a greater ability to conduct electricity.

Step-by-step explanation:

The difference between a 0.1 molar aqueous solution of sodium sulfate (Na2SO4) and a 0.1 molar aqueous solution of sodium chloride (NaCl) in terms of their conductivity of electricity can be explained by the number and type of ions each compound dissociates into when dissolved in water.

Sodium sulfate is a 2:1 electrolyte, meaning it dissociates into two sodium ions (2Na+) and one sulfate ion (SO42-) for each formula unit. As a result, a solution of sodium sulfate will conduct better because it produces more ions and the sulfate ion carries twice the charge in comparison to the chloride ion (Cl-), which means conducting more electrical current.