The given values of Ksp for iron(III) sulfide are as follows:A. 54 × 10−20B. 7.64 × 10−10C. 8.90 × 10−26D. 22× 10−17Iron(III) sulfide is a compound formed by combining the elements iron and sulfur. The chemical formula of iron(III) sulfide is Fe2S3, which means that it contains two iron (Fe) atoms and three sulfur (S) atoms.To calculate the Ksp of iron(III) sulfide, we need to determine which of the given values of Ksp is the correct one. Since there is only one correct answer, we can use the process of elimination to determine the correct answer.Using the given values of Ksp, we can write the expression for the solubility product constant for iron(III) sulfide:Ksp = [Fe3+][S2-]3In this expression, [Fe3+] represents the concentration of iron(III) ions and [S2-] represents the concentration of sulfide ions. Since iron(III) sulfide dissociates into one iron(III) ion and three sulfide ions, the concentration of iron(III) ions is equal to 1/3 of the concentration of sulfide ions.Let's calculate the concentration of sulfide ions using each value of Ksp:For option A:Ksp = [Fe3+][S2-]3∴ 54 × 10−20 = (1/3x)^3(x)^3, where x is the concentration of sulfide ionsSolving for x:54 × 10−20 = (1/3x)^3(x)^3x = 4.71 × 10−7MThe concentration of sulfide ions is 4.71 × 10−7M.Using this concentration and the 1/3 ratio, we can calculate the concentration of iron(III) ions:[Fe3+] = 1/3 x [S2-] = 1/3 x 4.71 × 10−7M = 1.57 × 10−7MNow we can substitute the concentrations of iron(III) and sulfide ions into the expression for Ksp:Ksp = [Fe3+][S2-]3= (1.57 × 10−7M) x (4.71 × 10−7M)3= 1.31 × 10−21The correct value of Ksp is A. 54 × 10−20.
To calculate the Ksp for iron(III) sulfide, additional information is required, such as the solubility of the compound in water or the equilibrium concentrations of the ions. Unfortunately, the given data does not provide enough information to accurately determine the Ksp value.