Chemistry 5 moles of Hydrogen Iodide dihydrate,

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To calculate the mass of 5 moles of Hydrogen Iodide dihydrate, the molar mass must include the mass of the additional 2H2O, as it contributes to the total weight. The concentration of a hydrate in water can be expressed in moles per liter, and dissolving 1 mole of the dihydrate in 1 liter results in a 1M solution, similar to anhydrous salts. While there are rare cases where the properties of hydrated solutions differ from their anhydrous counterparts, these can typically be overlooked in basic calculations. The discussion also touches on the convenience of abbreviating "mole" to "mol." Overall, understanding the molar mass and concentration of hydrates is essential for accurate chemical calculations.
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If I have 5 moles of Hydrogen Iodide dihydrate, for example, what is the mass? I knw that I have to tke the number of moles times the molar mass to find the mass but what is the molar mass of the compound I suggested? Do I hve to include the extra 2H2O part when finding the molar mass? Thanks for the help.
 
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DarylMBCP said:
If I have 5 moles of Hydrogen Iodide dihydrate, for example, what is the mass? I knw that I have to tke the number of moles times the molar mass to find the mass but what is the molar mass of the compound I suggested? Do I hve to include the extra 2H2O part when finding the molar mass?

Yup. The water's going to be there if you weight it, right?
 


DarylMBCP said:
If I have 5 moles of Hydrogen Iodide dihydrate, for example, what is the mass? I knw that I have to tke the number of moles times the molar mass to find the mass but what is the molar mass of the compound I suggested? Do I hve to include the extra 2H2O part when finding the molar mass? Thanks for the help.

Yes , an example of another hydrate is the hydrate of hydrogen phosphate , it's crystalline which is able to be isolated.
 


Ok, thanks guys. Btw, how do I find the number of moles of Hydrogen Iodide dihydrate in 1dm3 of aqueous solution if the concentration of Hydrogen Iodide dihydrate is 1mol/dm3? Is is even possible to have the concentration of a hydrate in water? Thanks for the help again.
 


If I dissolve 1 mole of substance in 1 liter of solution I have 1M solution. Doesn't matter if it was hydrate, dihydrate or something else. But as solution prepared by dissolving 1 mole of dhydrate is no different from the solution prepared by dissolving 1 mole of anhydrous salt (or 1 mole of decahydrate) - this 'hydrate' part is omitted.

There are probably very specific cases when such solutions will differ - for example it can be impossible to prepare concentrated solution of some substance using hydrated salt (too much water to get correct concentration). But these are rare cases, that can be safely ignored at first approach.
 


Borek do you know who came up with the idea to shorten the word mole to mol?I think it was a brilliant idea and a great time saver. :biggrin:
 


K, thnks for the help guys.
 

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