What is the molarity of NO₃^– in each solution? a. 0.225 M NaNO₃ b. 0.225 M Mg(NO₃)₂ c. 0.225 M Al(NO₃)₃

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Identify the number of nitrate ions (NO_3^–) produced per formula unit of each compound.

For NaNO_3, note that it dissociates into one Na^+ ion and one NO_3^– ion.

For Mg(NO_3)_2, note that it dissociates into one Mg^2+ ion and two NO_3^– ions.

For Al(NO_3)_3, note that it dissociates into one Al^3+ ion and three NO_3^– ions.

Calculate the molarity of NO_3^– by multiplying the given molarity of each compound by the number of NO_3^– ions produced per formula unit.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Molarity

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 (M) and is crucial for understanding how much of a substance is present in a given volume of solution. In this question, calculating the molarity of NO3– requires knowing the total moles of nitrate ions contributed by each compound.

Dissociation of Ionic Compounds

Ionic compounds dissociate into their constituent ions when dissolved in water. For example, NaNO3 dissociates into Na+ and NO3–, while Mg(NO3)2 dissociates into Mg2+ and two NO3– ions. Understanding how many nitrate ions are produced from each compound is essential for determining the molarity of NO3– in the solutions provided.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced equations. In this context, it helps in determining the number of moles of NO3– produced from each compound based on their dissociation. This is vital for accurately calculating the molarity of the nitrate ion in each solution.

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