Final answer:
Molar conductivity is influenced by the dissociation of electrolytes in solution, with strong electrolytes showing higher conductivity. In an acidic solution, the solubility of salts can increase if the acid reacts with one of the salt's ions. Na2SO4 conducts better than NaCl due to more ions and higher charges involved.
Step-by-step explanation:
In the context of aqueous solutions with the same concentration, molar conductivity refers to the conductance of a solution containing one mole of electrolyte per liter of solution. The molar conductivity depends on the number of ions present and their charge. Strong electrolytes, which fully dissociate into ions, have higher molar conductivities than weak electrolytes, which only partially dissociate.
Regarding the provided options for compounds dissolved in a 0.01-M solution of HClO4, solubility can be affected by the presence of a strong acid due to the common ion effect and the pH changes it induces. Generally, the solubility of a slightly soluble salt could be greater in an acidic solution than in pure water if the acid reacts with one of the ions of the salt, essentially removing it from the equilibrium and pushing the reaction towards more dissolution.
Conductivity measurements are important as they give insights into the nature of ions in a solution. For example, Na2SO4 conducts better than NaCl at the same concentration because it contributes more ions to the solution, and the sulfate ion has a higher charge which affects the conductivity.