How do you solve this stoichiometry problem? Is it possible?

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SUMMARY

The discussion centers on a stoichiometry problem involving a compound containing chlorine, where 10.25g of the compound is diluted and 30mL of this solution is reacted with excess AgNO3 to yield 35.5g of AgCl. The calculated mass of chlorine in the solution is approximately 8.78g, leading to a mass percent of chlorine in the original compound of around 86%. However, participants agree that insufficient information regarding the dilution process prevents a definitive solution to the problem.

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10.25g of a compound, including chlorine is then diluted. So there is 10.25g in the original compound, which is then diluted. 30mL of that solution is combined with an excess of AgNO3 to create 35.5g of AgCl. What is the mass percent of chlorine in the original compound/sample.

I got 8.78g for the grams of the 30mL of solution. But I don't know how much it was diluted to. So I got 8.78/10.25→~86%

I don't understand how to solve this. I asked a teacher and he didn't know either, saying there wasn't enough information.
 
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This should land in the homework section.

But I agree with your teacher - there is not enough information, you need details about the dilution process.
 

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