For each compound (all water soluble), would you expect the resulting aqueous solution to conduct electrical current? a. RbBr b. Na₃OH c. C₁₂H₂₂O₁₁ d. MgSO₄

Key Concepts

Electrolytes

Electrolytes are substances that dissociate into ions when dissolved in water, allowing the solution to conduct electricity. Strong electrolytes, such as salts and strong bases, fully dissociate into ions, while weak electrolytes only partially dissociate. Understanding whether a compound is a strong or weak electrolyte is crucial for predicting its ability to conduct electrical current in solution.

Solubility of Ionic Compounds

Ionic compounds, such as RbBr and MgSO4, typically dissolve in water to form ions, which contribute to electrical conductivity. The solubility of these compounds in water is influenced by factors like lattice energy and hydration energy. Recognizing which ionic compounds are soluble helps determine if their aqueous solutions will conduct electricity.

Non-electrolytes

Non-electrolytes are substances that do not dissociate into ions in solution, thus failing to conduct electricity. An example is sucrose (C12H22O11), which dissolves in water but remains as intact molecules. Identifying non-electrolytes is essential for understanding which compounds will not contribute to electrical conductivity in an aqueous solution.