How Do You Calculate Moles from Grams for BaCl2 *2H2O?

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SUMMARY

The discussion focuses on calculating the moles of BaCl2 * 2H2O from a mixture containing BaCl2 and BaCl2 * 2H2O. The experiment involves heating a 1.392g sample to obtain a mass of 1.087g after water loss, indicating the presence of water in the hydrate. The calculation of moles results in a value of 8.46507394x10-3, which requires clarification on the context of this figure. Participants emphasize the importance of showing work in calculations to receive assistance.

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  • Understanding of molar mass calculations, specifically for BaCl2 and BaCl2 * 2H2O.
  • Knowledge of the concept of hydrates and water of crystallization.
  • Familiarity with laboratory techniques for measuring mass before and after heating.
  • Basic principles of stoichiometry and weight percent calculations.
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  • Research the molar mass of BaCl2 * 2H2O for accurate calculations.
  • Learn about the process of determining weight percent in mixtures.
  • Study the principles of dehydration in hydrates and its impact on mass.
  • Explore stoichiometric calculations involving moles and mass conversions.
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Chemistry students, laboratory technicians, and educators involved in teaching analytical chemistry and stoichiometry concepts.

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If I have BaCl2 *2H2O how does that come to 8.46507394x10-3

Here is the question:
A common laboratory experiment involves the analysis of a mixture of BaCl2 and BaCl2 *2H2O. you are given a white powder that is a mixture of these compounds and are asked to determine the weight percent of each. you find that 1.392g of the mixture has a mass of 1.087g after heating it to drive off all of the water present.
 
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nieuport27 said:
If I have BaCl2 *2H2O how does that come to 8.46507394x10-3

In general - it doesn't, and what you wrote doesn't make sense. 8.46507394x10-3 of what? Cows? Marbles? mph? mpg? Stones per week?

Please note you have to show your attempts at solving the question to receive help. This is a forum policy.

A common laboratory experiment involves the analysis of a mixture of BaCl2 and BaCl2 *2H2O. you are given a white powder that is a mixture of these compounds and are asked to determine the weight percent of each. you find that 1.392g of the mixture has a mass of 1.087g after heating it to drive off all of the water present.

Hint: why did the sample get lighter?
 

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