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------------------------------------------------ A student mixes 5.00 mL of 0.00200 M Fe(NO₃)₃ and 5.00 mL of 0.00200 M KSCN. What are the initial concentrations of [tex]$Fe^{3+}$[/tex] and [tex]$SCN^-$[/tex] in the reaction mixture? (Hint: Don’t forget to account for the dilution due to mixing!)

Initial concentrations of Fe3+ and ScN- after mixing are both reduced to 0.00100 M due to dilution when the total volume of the reaction mixture becomes 10.00 ml.

The subject of this question is related to the calculation of initial concentrations after the mixing of two solutions in Chemistry, specifically within the context of a reaction mixture and the consideration of dilution effects. The question requires an understanding of solution concentration, reaction stoichiometry, and the concept of dilution when solutions are mixed. To find the initial concentrations of Fe3+ and ScN- after mixing 5.00 ml of 0.00200 M Fe(NO3)3 with 5.00 ml of 0.00200 M KScN, we must account for the total volume of the reaction mixture, which is 10.00 ml. Since the volume doubles when the two solutions are mixed, the concentration of each species is halved:

Initial [Fe3+]: (0.00200 M) x (5.00 ml / 10.00 ml) = 0.00100 M

Initial [ScN-]: (0.00200 M) x (5.00 ml / 10.00 ml) = 0.00100 M