Calculate the initial concentration of Sun⁻ in an equilibrium solution prepared by mixing 5.00 mL of Scᵃn⁻ and 5.00 mL of Fe³⁺. The final volume is 10.00 mL.

Question

01-01-2025
Chemistry

High School

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Calculate the initial concentration of Sun⁻ in an equilibrium solution prepared by mixing 5.00 mL of Scᵃn⁻ and 5.00 mL of Fe³⁺. The final volume is 10.00 mL.

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monur5195 monur5195 · Answer 1 · 2024-10-14T16:26:46-04:00

To find the initial concentration of SCN- in the equilibrium solution, use an ICE table with provided data to calculate it as 0.014 M.

To calculate the initial concentration of SCN- in the equilibrium solution, we can use the concept of equilibrium concentrations and stoichiometry. We can set up an ICE table with the given information and use the equilibrium concentration of Fe(SCN)²+ to determine the initial concentration of SCN-. In this case, the initial concentration of SCN- in the sample is found to be 0.014 M. The question involves calculating the initial concentration of SCN- in an equilibrium solution by comparing it with the concentration of Fe(SCN)2+ obtained from the reaction kinetics data.

The question asks to calculate the initial concentration of the thiocyanate ion (SCN-) in a sample when mixed with iron (III) ion (Fe3+), given that the analysis under identical conditions gives an Fe(SCN)2+ concentration of 3.52 imes 10-2 M after 10 seconds. This is a typical equilibrium problem in chemistry that involves a complexation reaction between Fe3+ and SCN- to form Fe(SCN)2+. To find the initial concentration of SCN- before equilibrium, we compare this with a standard solution or external standards under pseudo-first-order conditions. Data such as the final concentrations and the reaction's kinetics are used to backtrack and determine the initial concentration of the reactants.