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A mixture is made by combining 17.8 mL of 6.1×10−3 M KSCN, 9.6 mL of 9.5×10−2...

A mixture is made by combining 17.8 mL of 6.1×10−3 M KSCN, 9.6 mL of 9.5×10−2 M Fe(NO3)3, and 8 mL of 0.29 M HNO3. Calculate the concentration of Fe3+ in the solution.

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Answer #1

1mole of KSCN reacts with 1 mole of Fe(NO3)3 to form 1 mole of complex.

Remaining Fe3+ in solution = (9.5 x 10^-2 x 9.6 - 6.1 x 10-3 x 17.8)/(17.8+9.6+8)

                                             = 0.023 M is the required concentration  

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