[Chem] Determining Masses from Concentration

AI Thread Summary
To determine the masses of magnesium chloride and sodium chloride in a 0.6118 g sample, the student adds 145 mL of 0.1006 M silver nitrate, resulting in 1.7272 g of silver chloride precipitate. The first step involves calculating the moles of silver nitrate used, which can be derived from its volume and molarity. The reaction products include silver chloride, magnesium chloride, and sodium chloride, and the stoichiometry of the reaction will help establish the relationship between the moles of silver chloride and the original components. By using the mass of silver chloride and the total mass of the sample, the individual masses of magnesium chloride and sodium chloride can be calculated. Understanding the stoichiometric ratios and the excess data provided is crucial for solving the problem effectively.
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Homework Statement


In lab, a student decides to analyze a 0.6118 g sample containing only magnesium chloride and sodium chloride. He does this by adding 145 milliliters of 0.1006 M silver nitrate. A precipitate, silver chloride, is formed, which has a mass of 1.7272 grams. Using this data, calculate the mass of each of the original sample's components.

Homework Equations



M = mol / L

MgCl_{2} + NaCl + AgNO_{3} ...?

The Attempt at a Solution



I'm not really sure where to start here; my instinct is to multiply the volume of the silver nitrate by its molarity to get the number of moles. But I'm not sure what to do next, and I don't know what the products of the reaction are, other than the silver chloride precipitate. And besides, how would I able to find out how much mass there is of the individual components in the original sample if the problem only gives the total mass of these two components? Can anyone help me out? (Thanks in advance! :))
 
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dt_ said:

Homework Statement


In lab, a student decides to analyze a 0.6118 g sample containing only magnesium chloride and sodium chloride. He does this by adding 145 milliliters of 0.1006 M silver nitrate. A precipitate, silver chloride, is formed, which has a mass of 1.7272 grams. Using this data, calculate the mass of each of the original sample's components.


Homework Equations



M = mol / L

MgCl_{2} + NaCl + AgNO_{3} ...?

The Attempt at a Solution



I'm not really sure where to start here; my instinct is to multiply the volume of the silver nitrate by its molarity to get the number of moles. But I'm not sure what to do next, and I don't know what the products of the reaction are, other than the silver chloride precipitate. And besides, how would I able to find out how much mass there is of the individual components in the original sample if the problem only gives the total mass of these two components? Can anyone help me out? (Thanks in advance! :))


Start by writing out the precipitation reaction. This will give you the ratio of moles of silver chloride to moles of magnesium chloride plus sodium chloride.
Do you know how to determine the number of moles of silver chloride produced with the given data?
Hint: more data is given to you than you need to answer this question. Which data is unnecessary?
 
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