Calculating Moles of Water in BaCl2*H2O Hydrate - Step by Step Guide

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SUMMARY

The discussion focuses on calculating the number of moles of water in the hydrate BaCl2·H2O. Given a hydrate mass of 5 grams, a mass of lost water of 0.7 grams, and an anhydrous compound mass of 4.3 grams, the key calculation involves converting the mass of water to moles using the conversion factor of 1 mole of water per 18 grams. The conclusion is that the moles of water can be determined directly from the mass of lost water.

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  • Understanding of molar mass calculations
  • Familiarity with hydrates in chemistry
  • Knowledge of the concept of moles
  • Basic arithmetic skills for mass and mole conversions
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  • Learn about molar mass of common compounds, specifically BaCl2 and H2O
  • Study the concept of hydrates and their properties
  • Explore stoichiometry in chemical reactions
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Chemistry students, educators, and anyone interested in understanding the calculations involved in determining moles of water in hydrates.

crayzlilgurl
[SOLVED] A chem problem...help please

I don't know how to answer this question. I have to find the number of moles of water in the hydrate BaCL2*H2O. SOwwie i don't now how to make the 2 smaller. The mass of the hydrate is 5g, the Mass of lost
water is .7 grams and the anhydrous compound is 4.3 grams. Please help me. Thanks
 
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Originally posted by crayzlilgurl
I don't know how to answer this question. I have to find the number of moles of water in the hydrate BaCL2*H2O. SOwwie i don't now how to make the 2 smaller. The mass of the hydrate is 5g, the Mass of lost
water is .7 grams and the anhydrous compound is 4.3 grams. Please help me. Thanks

It's pretty easy. You know that there was 0.7 grams of water originally. You, should, also know that water is 1/18 moles per gram. I can't make it any easier for you than that without telling you the answer, and that wouldn't do you any good.
 
thanks...i noe wut to do it just all the numbers i was given confused the heck outta me...
 
i don't kow eitehr
 

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