A reaction mixture of 4.00 mL of 0.00200 M SCN and 5.00 mL of 0.00200 M Fe^3+ is diluted to 10.00 mL with 0.1 M HNO3 to form the blood-red FeNCS^2+ complex. The equilibrium molar concentration of the FeNCS^2+ determined from a calibration curve, is 1.5 x 10^-4 mol/L. Calculate, in sequence each of the following quantities in the aqueous solution to determine the equilibrium constant for the reaction.
Fe^3+(aq) + SCN-(aq)<-------->FeNCS2+(aq)
a. moles of FeNCS^2+ that form in reacting equilibrium
b. moles of Fe3+ that react to form the FeNCS^2+ at equilibrium
c. moles of SCN- that react to form the FeNCS^2+ at equilibrium
d. moles of Fe^3+ initially placed in the reaction system
e. moles of SCN- initially placed in the reaction system
f. moles of Fe^3+ (unreacted) at equilibrium
EQUATION:
mol Fe^3+ equilibrium = mol Fe^3+ initial - mol Fe^3+ reacted
g. moles of SCN- (unreacted) at equilibrium
EQUATION:
mol SCN- equilibrium = mol SCN- initial - mol SCN- reacted
h. molar concentration of Fe^3+ (unreacted) at equilibrium
i. molar concentration of SCN- (unreacted) at equilibrium
j. molar concentration of FeNCS^2+ at equilibrium
k. Kc= ([FeNCS^2+]) / ([Fe^3+][SCN-])