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Calculate the initial concentrations of each reactant ([Fe^3+] and [SCN^-]) in Reactions 1-4 using the relationship [tex]C_1V_1 = C_2V_2[/tex].

Since the same volume of [Fe^3+] was added to all four reactions, you only need to show one calculation for [Fe^3+]₀.

| RXN | 0.00200 M Fe(NO3)3 (ml) | 0.00200 M KSCN (ml) | H2O (ml) |
|-----|-------------------------|----------------------|-----------|
| 1 | 5.00 | 2.00 | 3.00 |
| 2 | 5.00 | 3.00 | 2.00 |
| 3 | 5.00 | 4.00 | 1.00 |
| 4 | 5.00 | 5.00 | 0.00 |

Answer :

Final answer:

The initial concentration of Fe³+ is determined using the formula C₁V₁ = C₂V₂. By substituting the given values and solving, we find the initial concentration for Fe³+ to be 1.00 x 10⁻³ M.

Explanation:

In order to calculate the initial concentrations of Fe³+ and SCN-, we can employ the relation C₁V₁ = C₂V₂ where C₁ and V₁ are initial concentrations and volumes, and C₂ and V₂ are final concentrations and volumes. The reaction we are focusing on is Fe³+ + SCN- = [Fe(SCN)]²+.

For the calculation of [Fe³+]i, we can use the provided data for Reaction 1 as an example. Given that the volume of Fe(NO3)3 is 5.00 ml and the concentration is 0.00200 M, we can compute as follows:

V₁ = 5.00 mL = 5.00 x 10⁻³ L (Convert the volume from ml to L)

C₁ = 0.00200 M

C₂ = C₁V₁ / V₂ = 0.00200 M * 5.00 x 10⁻³ L / 0.01 L = 1.00 x 10⁻³ M

Strictly speaking, for the four cases you mentioned, the total volume (V₂) is different each time due to the added volume of KSCN and water. Therefore, the initial concentration of Fe³+ would be slightly different for each reaction if specifically calculated.

Note: If the total volume is almost constant, or the volume of one component is much larger than the others, we often simplify by taking the initial concentration as the concentration after mixing.

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