Determine the concentration of the cation and anion in each...

Determine the concentration of the cation and anion in each aqueous solution. (Assume complete dissociation of each compound.)
(a) $0.12 \mathrm{M} \mathrm{Na}_{2} \mathrm{SO}_{4}$
(b) $0.25 \mathrm{M} \mathrm{K}_{2} \mathrm{CO}_{3}$
(c) $0.11 \mathrm{M} \mathrm{RbBr}$

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Key Concepts

Stoichiometry of Ionic Dissociation

This involves the quantitative relationships between the compound and its ions based on its chemical formula. The stoichiometric coefficients indicate the number of each type of ion produced from one formula unit, which is crucial for determining individual ion concentrations in the solution.

Ion Concentration Calculations

Calculating ion concentrations in aqueous solutions requires multiplying the molarity of the compound by the number of ions yielded per formula unit. This calculation stems from complete dissociation and ensures that the total number of moles of each ion is accurately reflected based on the compound's stoichiometry.

Complete Dissociation

This concept assumes that when an ionic compound is dissolved in water, it breaks apart fully into its constituent ions. There are no undissociated molecules remaining in the solution, thereby allowing the concentration of each ion to be directly related to the formula of the compound.

Molarity

Molarity is a measure of concentration expressed as the number of moles of solute per liter of solution. It is essential in calculating the final concentrations of ions in a solution after the compound dissociates.

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