What is the molarity of each ion in a solution prepared by dissolving 0.550 g of Na2SO4, 1.188 g of Na3PO4, and 0.223 g of Li2SO4 in water and diluting to a volume of 100.00 mL?

Molarity is a measure of concentration defined as the number of moles of solute per liter of solution. It is expressed in moles per liter (mol/L) and is crucial for understanding how much of a substance is present in a given volume of solution. To calculate molarity, one must first determine the number of moles of solute by dividing the mass of the solute by its molar mass, and then divide by the volume of the solution in liters.

Ionic compounds, such as Na2SO4 and Na3PO4, dissociate into their constituent ions when dissolved in water. This dissociation is essential for calculating the molarity of each ion in the solution. For example, Na2SO4 dissociates into 2 Na⁺ ions and 1 SO4²⁻ ion, while Na3PO4 dissociates into 3 Na⁺ ions and 1 PO4³⁻ ion. Understanding the stoichiometry of these dissociations allows for accurate calculations of ion concentrations.

When preparing a solution, the total volume after dilution is critical for determining the molarity of the ions. In this case, the final volume is given as 100.00 mL, which must be converted to liters (0.100 L) for molarity calculations. It is important to ensure that all solutes are accounted for in the final volume to accurately reflect the concentration of each ion in the solution.