chemistry
posted by Christina .
A STUDENT STUDYING THE FE+3 HSCN equilibrium put into a test tube 10.00ml of 2.00 x 103 M Fe(NO3)3 with 10.0 mL of 2.00 x 103 M HSCN.THE H+ in the resulting solution was manteined at 0.500.By spectrophotometric analysis of the equilibrium solution, the equilibrium concentration of FESCN+2 was found to be 1.00x104M.
1.CALCULATE THE INITIAL MOLARITY OF THE FE+3 AFTER DILUTION BUT BEFORE REACTION OCCURRED.ie, {Fe+}0
2. CALCULTE THE INITIAL MOLARITY OF HSCN AFTER DILUTION.
3. CALCULATE THE FE+3 WHICH REMAINED UNREACTED IN SOLUTION.ie, The equillibrium malarity of Fe +3
4. CALCULATE THE HSCN MOLARITY WHICH REMAINED UNREACTED IN SOLUTION.ie, The equilibrium molarity.
5. CALCULATE THE VALUE FOR KC FOR THE REACTION

1. Initial (Fe^3) = 2E3 x (10 mL/20 mL)= ?M
2. Initial HSCN = 2E3 x (10 mL/20 mL) = ?
3.
...........Fe^3+ + SCN^ ==> FeSCN^2+
initial...1E3.....1E3.......0
change.....x......x.........x
equil.......................1E4
So x = 1E4. Calculate (F3^^3+) and (SCN^) and from there plug into Kc expresion and solve for Kc.