Which of the following solutions of strong electrolytes contains the largest number of ions per liter?

• A. 0.10 M CaCl2
• B. 0.10 M KNO3
• C. 0.10 M NaCl
• D. 0.10 M Na2SO4

Answer: (A)

Verified step by step guidance

1. Identify that all given substances are strong electrolytes, meaning they completely dissociate into their ions in solution.
2. Write the dissociation equations for each electrolyte to determine the total number of ions produced per formula unit: - CaCl\_2 \rightarrow Ca^{2+} + 2Cl^{-} (3 ions total) - KNO\_3 \rightarrow K^{+} + NO\_3^{-} (2 ions total) - NaCl \rightarrow Na^{+} + Cl^{-} (2 ions total) - Na\_2SO\_4 \rightarrow 2Na^{+} + SO\_4^{2-} (3 ions total)
3. Since all solutions have the same molarity (0.10 M), calculate the total ion concentration by multiplying the molarity by the number of ions produced per formula unit for each electrolyte.
4. Compare the total ion concentrations calculated for each solution to determine which has the largest number of ions per liter.
5. Conclude that the solution with the highest total ion concentration corresponds to the electrolyte that produces the greatest number of ions per formula unit multiplied by its molarity.