How many moles of sulfate ions are in 100 mL of a solution of 0.0020 M Fe2(SO4)3
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How many moles of sulfate ions are in 100 mL of a solution of 0.0020 M Fe2(SO4)3

[From: ] [author: ] [Date: 12-06-12] [Hit: ]
..0.0020 moles/L (0.0020M) x 100mL = 0.Fe2(SO4)3 is 2 parts Iron to 3 parts Sulfate,......
this is all i got so far
first i find the mole by 0.0020 M Fe2(SO4)3 *0.1L=0.0002 mole Fe2(SO4)3
then percent of (SO4) in Fe2(SO4)3 which 288/399.87=72.02%
find mole of SO4 0.0002 mole Fe2(SO4)3 *.7202=1.4*E-4
(this is still a wrong answer thought, ;(

-
Molarity x Volume = Moles
Ratio of Ion Moles to Total Moles x Number of Total Moles = Number of Ion Moles

So...

0.0020 moles/L (0.0020M) x 100mL = 0.0002 moles

Fe2(SO4)3 is 2 parts Iron to 3 parts Sulfate, or in other words, 3 parts Sulfate to 5 parts Total

3/5 x 0.0002 moles = 0.00012 = 1.2 x 10^-4 moles
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