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20.00 mL of 3.00E-3 M Fe(NO3)3 is mixed with 8.00 mL of 2.48E-3 M KSCN and...

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Chemistry

20.00 mL of 3.00E-3 M Fe(NO3)3 is mixed with 8.00 mL of 2.48E-3M KSCN and 12.00 mL of water. The equalibrium molarity of Fe(SCN)2+is found to be 6.82E-5 M. If the reaction proceeds as shown below,what is the equilibrium molarity of Fe3+ andSCN-?    Fe3+(aq) + 2 SCN-(aq) Fe(SCN)2+(aq)

I have the answers (they are correct according to my onlinehomework), but need to know how to get them. Thank you! The correctansweers are: Fe = 1.43E-3 SCN = 3.60E-4

Answer & Explanation Solved by verified expert
4.4 Ratings (866 Votes)
Answer Given FeNO33 300103 M volume 200 mL KSCN 248103 M volume 800 mL water volume 120 mL At equilibrium FeSCN22    See Answer
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