Discussion What would happen to your results (how would it effect the salt to wa

Question

Discussion What would happen to your results (how would it effect the salt to water ratio) if not all of the water was evaporated from your sample? What would happen to your results (how would it effect the salt to water ratio) if measureable oils and dirt were on the crucible (you touched the crucible after heating and before massing)? What would happen to your results (how would it effect the salt to water ratio) if some of the hydrate spattered out while heating. What happens if you bum off too much water? (Can you bum off water?) The chemical formula that you found above was magnesium oxide's empirical formula. What if you found the empirical formula of a compound made of hydrogen and oxygen as HO However, the molecular mass of the compound is 34.01 g/mol What would the molecular formula of this compound be?

Explanation / Answer

1) water would pose problem for salts, compounds like esters..where chances of hydrolysis is there.

an exception with stability in water would be acids. compounds would be unstable in water. because of the presence of water chances of unnecessary oxidation is also there.

2) oils and dirts woulnt hamper the product as such. but could alter our calculations , if the sample has to be used in a reaction later. spectroscopic confirmation of product would be incorrect for this dirts.

3) HYDRATE LOSS ON HEATING LEAD TO DECREASE IN WT OF THE SAMPLE.

it becomes atmost anhydrous.

4) water doesnt burn...you evapourate it off. if your sample is a considerable high melting solid / high boiling liquid heating off the water shouldnt cause any problem to the sample. if not then charring of sample is a chance..

(2) empirical formula is OH

molecular mass= 34.01g/mol

molecular formula is a multiple of empirical formula

OH= (1*1 +16*1)

= 17

EMPIRICAL FORMULA UNITS= 34.01/17 = 2

MOLECULAR FORMULA = 2 * OH = H2O2

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