Question

In: Chemistry

A solution was prepared by mixing 4.00mL of 2.00х10-3M Fe(NO3)3 and 3.00mL of 5.00х10-3M NaSCN and...

A solution was prepared by mixing 4.00mL of 2.00х10-3M Fe(NO3)3 and 3.00mL of 5.00х10-3M NaSCN and diluting the mixture with water to a total of 10.00mL. Use your average value of Kc to calculate the equilibrium concentration of FeSCN2+ in the mixture.

Average value of Kc is 787.3

Solutions

Expert Solution

Initial moles of [Fe(H2O)6]3+ = 0.014 L * 2*10-3 mol/L = 2.8*10-5 mol
Initial moles of NaSCN = 3*10-3 L * 5*10-3 mol/L = 15*10-6 mol
Make an ICE table,

  Kc = [FeSCN]2+ / [Fe3+] [SCN-] = X / [2*10-5 - X] [15*10-6 - X]
787.3 = X / [2*10-5 - X] [15*10-6 - X]
  787.3 = X / [ 3*10-10 - 2*10-5X - 15*10-6X + X2 ]
787.3 [X2 - 3.5*10-5X + 3*10-10] = X
787.3X2 - 0.027555X + 2.3619*10-7 = X
787.3X2 - 1.0275555X + 2.3619*10-7 = 0
   Solve the above quadratic expression,
   X = 2.2989*10-7 mol = FeSCN2+
Concentration of FeSCN2+ at equilibrium = 2.2989*10-7 mol / (0.014+3*10-3)L = 1.3523*10-5 mol/L
[FeSCN]2+ = 1.3523*10-5M at equilibrium


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