3.0 mL of 0.02 M Fe(NO3)3 solution is mixed with 3.0 mL of 0.002 M NaNCS and diluted to the mark with HNO3 in 10 mL volumetric flask. The blood-red [Fe(NCS)]2+ ion that forms has an equilibrium molar concentration of 2.5*10-4 mol/L as determined from the calibration plot. Calculate the Kc for [Fe(NCS)]2+ formation. Assume the volumes are additive.

The for formation is .

Explanation:

Concentration of ferric ion =

Volume of ferric solution = 3.0 mL = 0.003 L

Moles of ferric ion  

1 mL = 0.001 L

Concentration of ion =

Volume of ion solution = 3.0 mL = 0.003 L

Moles of ion=

Volume of nitric acid solution = 10 mL = 0.010 L

After mixing all the solution the concentration of ferric ion and ion will change

Total volume of solution = 0.003 L + 0.003 L + 0.010 L = 0.016 L

Initial concentration of ferric ion before reaching equilibrium :

=

Initial concentration of ion before reaching equilibrium :

=

Initially:

0.00375 M    0.000375 M       0

At equilibrium :

(0.00375-x)   (0.000375-x)       x

Equilibrium concentration of

The expression of equilibrium constant for formation is given by :

The for formation is .

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