What is the process to calculate the mass of Na2CrO4 required to precipitate silver ions?

Question:

How can we determine the mass of Na2CrO4 needed to precipitate all of the silver ions from a solution of AgNO3?

Answer:

The process to calculate the mass of Na2CrO4 required to precipitate silver ions involves several steps. Let's break it down:

1. Write the balanced chemical equation for the reaction between Na2CrO4 and AgNO3:

2AgNO3 + Na2CrO4 → Ag2CrO4 + 2NaNO3

2. Calculate the number of moles of AgNO3 using the given volume and concentration. The formula to calculate moles is: Moles = Volume (in liters) × Concentration (in moles per liter).

3. Use the stoichiometry of the reaction to determine the number of moles of Na2CrO4 required. From the balanced equation, we can see that 2 moles of AgNO3 react with 1 mole of Na2CrO4.

4. Convert the moles of Na2CrO4 to grams using its molar mass. The molar mass of Na2CrO4 is 161.97 g/mol.

By following these steps, you can calculate the mass of Na2CrO4 needed to precipitate all of the silver ions from the solution of AgNO3. It's important to pay attention to the balanced chemical equation and use the molar masses of the compounds involved in the reaction.