An aspirin tablet problem?

[mariaaa]

An aspirin tablet weighing 0.650 g has been analyzed and contains 68.2 % ASA (180.16 g/mol) by mass. A student dissolved
the tablet in hot NaOH and the cooled solution was diluted with DI water to the mark in a 250 mL volumetric flask. Exactly 3.00 mL
of the solution was pipetted into a 100 mL volumetric flask and diluted to the mark with FeCl3 solution.
The concentration of the diluted solution is
....
i dont know where to start..
helpp!!

[Alex]

1) What is 68.2% of .650g to get Grams of ASA in the tablet
2) convert grams of ASA to moles of ASA using the given molar mass
3) Molarity is moles/L, so take the number of moles you got in #2 and divide it by .250L to get the dilution for the first step
4) use M1V1=M2V2 and solve for M2 to find the concentration for the second dilution (M1=what you got in 3, V1=3.00ml (.00300L), V2=.100L).

This will give you the concentration of the final dilute solution

[SwayGirl]

[quote=Alex;11335]1) What is 68.2% of .650g to get Grams of ASA in the tablet
2) convert grams of ASA to moles of ASA using the given molar mass
3) Molarity is moles/L, so take the number of moles you got in #2 and divide it by .250L to get the dilution for the first step
4) use M1V1=M2V2 and solve for M2 to find the concentration for the second dilution (M1=what you got in 3, V1=3.00ml (.00300L), V2=.100L).

This will give you the concentration of the final dilute solution[/quote]


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