Question

For each test tube solution enter the initial concentration of Fe+ and SCNthe equilibrium concentration of FeSCN2: into the ICE table given. Complete entries for the rest of the table and calculate the K value for each of the tables. The values of K should be confined to a narrow range to reflect constancy. Comment on the quality of your work in this regard and calculate the average K. • Standard Solution: 5.00 mL of 0.200M Fe(NO3)3 : 1.00 mL of 0.00200 M KSCN; and 4.00 mL of 1.00 M HNO3. (0.200 M) (5.00 mL) = Total volume of the mixture is _ 10 mL Concentration of Fe(NO3)3 is (Use M;V;= M/V) Concentration of KSCN is (Use M;V; = MVO) Concentration of [FeSCN2) is (Use limiting reactant theory and equation) Fe +2 (aq) + (SCN) (aq) (FeSCN)+2 (aq) Since (Fe+3) >>(SCN) in the solution, essentially all (SCN) has been converted to (FeSCN2). according to the Le Chatelier's Principle. Thus the equilibrium concentration of (FeSCN+2) is equal to the initial (SCN) concentration which is calculated as: 0.00200 M x 1.0 mL/10.00 mL = 2.0 x 10-4 M ice table Standard Sample: Absorbance of standard solution FeSCN2+1 is Plot a linear graph of concentration of (FeSCN"{x-axis) vs. Absorbance {y-axis) with line

What's the concentration of [FeSCN2+] using limiting reactant theory and equation?

Answer 1

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