What is the molarity of NO₃^– in each solution? a. 0.150 M KNO₃ b. 0.150 M Ca(NO₃)₂ c. 0.150 M Al(NO₃)₃

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

For KNO_3, note that it dissociates into one K^+ ion and one NO_3^- ion.

For Ca(NO_3)_2, note that it dissociates into one Ca^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.

Multiply the molarity of each compound by the number of nitrate ions produced to find the molarity of NO_3^- in each solution.

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주요 개념

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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, KNO3 dissociates into K+ and NO3–, while Ca(NO3)2 dissociates into Ca2+ and two NO3– ions. Understanding how many ions are produced from each compound is essential for determining the molarity of the nitrate ion in each solution.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on their molar ratios. In this context, it helps in determining the number of moles of NO3– produced from each compound based on its formula and the initial molarity. This concept is vital for accurately calculating the concentration of nitrate ions in the solutions provided.

What is the molarity of NO3– in each solution? a. 0.150 M KNO3 b. 0.150 M Ca(NO3)2 c. 0.150 M Al(NO3)3