A 5.0mL volume of 0.00200 M SCN- is mixed with5.0mL of 0.0200 M Fe^3+ to form th

Question

A 5.0mL volume of 0.00200 M SCN- is mixed with5.0mL of 0.0200 M Fe^3+ to form the blood-redFeNCS^2+ complex. The equilibrium molar concentration ofthe FeNCS^2+ determined from a calibration curve, is7.0x10^-4 mol/L. Calculate, in sequence, each of thefollowing quantities in the aqueous solution to determine theequilibrium constant for the reaction, Fe3+ (aq) + SCN- (aq) FeNCS2+ (aq) Given: moles of Fe^3+ (unreacted) at equilibriumare 9.3x10^-5 mol molesof SCN- (unreacted) at equilibrium are3.0x10^-6 mol Find: a. moles of Fe^3+ that react to form theFeNCS^2+ at equilibrium b. moles ofSCN- that react to form the FeNCS^2+ atequilibrium c. molar concentrationof Fe^3+ (unreacted) at equilibrium d. molar concentrationof SCN- (unreacted) at equilibrium

Explanation / Answer

A 5.0mL volume of 0.00200 M SCN- is mixed with5.0mL of 0.0200 M Fe^3+ to form th

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