Asked by cristy
A student weighs out a 14.0 g sample of Fe(NO3)2, transfers it to a 500 mL volumetric flask, adds enough water to dissolve it and then adds water to the 500 mL tic mark.
What is the molarity of iron(II) nitrate in the resulting solution?
What is the molarity of iron(II) nitrate in the resulting solution?
Answers
Answered by
Dr Russ
Calculate the molar mass of Fe(NO3)2 (F)
number of moles of Fe(NO3)2 = 14.0 g/F
If the number of moles were dissolved in 1 L the molarity would be
14.0/F mol L^-1
but this is in only 500 ml so the concentration is
(14.0 x 1000)/(F x 500)
i.e. twice the concentration if the final volume had been 1 L.
number of moles of Fe(NO3)2 = 14.0 g/F
If the number of moles were dissolved in 1 L the molarity would be
14.0/F mol L^-1
but this is in only 500 ml so the concentration is
(14.0 x 1000)/(F x 500)
i.e. twice the concentration if the final volume had been 1 L.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.