CHEMISTRY

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A STUDENT STUDYING THE FE+3- HSCN equilibrium put into a test tube 10.00ml of 2.00 x 10-3 M Fe(NO3)3 with 10.0 mL of 2.00 x 10-3 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 1.00x10-4M.

1.-CALCULATE THE INITIAL MOLARITY OF THE FE+3 AFTER DILUTION BUT BEFORE REACTION OCCURRED.
2.- CALCULTE THE INITIAL MOLARITY OF HSCN AFTER DILUTION.
3.- CALCULATE THE FE+3 WHICH REMAINED UNREACTED IN SOLUTION.
4.- CALCULATE THE HSCN MOLARITY WHICH REMAINED UNREACTED IN SOLUTION.
5.- CALCULATE THE VALUE FOR KC FOR THE REACTION.

I HOPE YOU CAN DO THIS HELP PLEASE IM LOST

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