What is the empirical formula of this compound help?

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The discussion revolves around determining the empirical formula of a hydrated compound with a specific percentage composition of sodium, sulfur, oxygen, and water. Participants express confusion over their calculations, particularly regarding the mole ratios of the elements. One user suggests that their formula, Na2S2O3 - 5H2O, may not accurately represent the compound due to discrepancies in mole counts. Another user shares a methodical approach to converting percentages to moles, emphasizing the importance of following a systematic process. Overall, the conversation highlights the challenges in deriving empirical formulas from percentage compositions.
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A hydrated substance was found to have the following percentage composition= Na 18.53%
S= 25.87%
O= 10.34%
H2O= 62.9%
What is the empirical formula of this compound?


what i got was Na2S2O3 - 5H2O
but I am confused cause Na and S are both 0.806 mols
 
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Perhaps, if you showed your work you might get more answers.
 
10.34/16 < 18.53/23 and 25.87/32, but you have more O atoms in your formula than Na and S. How is that? I got Na5S5O4*22H2O, but that's probably not right.
 
umm hmm i assumed 100 grams and then converted to mols
 
Use this cool poem.

Percent to mass
Mass to mole
Divide by small
Multiply 'til whole
Poem by "Joel S. Thompson"
 
MichaelXY said:
Use this cool poem.

Percent to mass
Mass to mole
Divide by small
Multiply 'til whole
Poem by "Joel S. Thompson"

That's pretty neat! I'll have to remember that.
 
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