What is the molarity of each ion in a solution prepared by...

What is the molarity of each ion in a solution prepared by dissolving 0.550 $\mathrm{g}$ of $\mathrm{Na}_{2} \mathrm{SO}_{4}, 1.188 \mathrm{g}$ of $\mathrm{Na}_{3} \mathrm{PO}_{4}$ , and 0.223 $\mathrm{g}$ of $\mathrm{Li}_{2} \mathrm{SO}_{4}$ in water and diluting to a volume of 100.00 $\mathrm{mL} ?$

Key Concepts

Stoichiometry of Ionic Dissociation

When an ionic compound dissolves in water, it dissociates into its constituent ions in a predictable stoichiometric ratio as determined by its chemical formula. Understanding this dissolution behavior is essential for determining the concentration of each ion in solution, as each compound produces a specific number of ions upon complete dissociation.

Mole Concept

The mole concept involves converting a given mass of a substance into moles using the substance’s molar mass. This conversion is a fundamental step in quantitative chemistry because it establishes the direct relationship between the mass of a substance and the number of particles or ions it contains.

Molarity

Molarity is defined as the number of moles of a solute per liter of solution. It is a central concept in solution chemistry that allows for the quantification of how concentrated a solution is. Molarity is crucial when calculating the concentrations of ions resulting from the dissolution of compounds in a solution.

Volume Conversion and Dilution

Volume conversion and dilution involve adjusting the calculated moles of solute to the actual volume of the solution prepared, typically expressed in liters. This step is necessary to convert a mole quantity into molarity, particularly when the final solution volume is provided in milliliters or another unit that must be converted to liters.

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