Suppose you have 5.00 g of powdered magnesium metal, 1.00 L of 2.00 M potassium nitrate solution, and 1.00 L of 2.00 M silver nitrate solution. d. What is the molarity of the Mg2+ ions in the resulting solution?

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Calculate the moles of magnesium (Mg) using its molar mass.

Write the balanced chemical equation for the reaction between magnesium and silver nitrate.

Determine the moles of Mg2+ ions produced from the reaction using stoichiometry.

Calculate the total volume of the resulting solution by adding the volumes of the potassium nitrate and silver nitrate solutions.

Find the molarity of Mg2+ ions by dividing the moles of Mg2+ by the total volume of the solution in liters.

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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). To calculate molarity, one must know the amount of solute in grams, convert it to moles using the molar mass, and then divide by the volume of the solution in liters.

Stoichiometry

Stoichiometry involves the calculation of reactants and products in chemical reactions based on balanced chemical equations. It allows us to determine the amount of products formed or reactants consumed in a reaction, which is essential for understanding how much magnesium will react with the nitrate solutions to produce Mg2+ ions.

Dissociation of Ionic Compounds

When ionic compounds dissolve in water, they dissociate into their constituent ions. For example, potassium nitrate (KNO3) and silver nitrate (AgNO3) dissociate into K+, NO3-, and Ag+ ions in solution. Understanding this dissociation is crucial for determining the concentration of Mg2+ ions after the reaction, as it affects the overall ion balance in the solution.

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