In the second part of this experiment, a student makes a solution with initial concentrations of iron(III) and thiocyanate ions of 0.000900 M and 0.000600 M respectively. Using the Beer's Law plot produced in the first part of the lab, the student determines the equilibrium concentration of the thiocyanatoiron(III) complex (Fe(SCN)2+) to be 2.00 × 10−5 M.  What are the equilibrium concentrations of the two starting ions, and what is the value of the equilibrium constant?     [Fe3+] =  [SCN−] =   Kc =

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A: solution given as below:

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Q: Silver and ammonia may react to form Ag(NH3)2+ complex (​K​f = 1.66 x 10​7). A 500 mL of 0.20mol Ag+…

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Q: n the second part of this experiment, a student makes a solution with initial concentrations of…

A: Solution with initial concentrations of iron(III) =0.000900 M…

Q: For the aqueous [Ni(NH3 )6]2+ complex Kf=5.50 x 108 at 25C . Suppose equal volumes of 0.0024 M…

A: Given :  Kf = 5.50 x 108   Concentration of Ni(NO3)2 = 0.0024 M  Concentration of NH3 = 0.94 M

Q: A similar experiment as this lab is done as following: 0.456 g of solid AgCl is added a 25 mL…

A: Answer is explained below.

Q: Percent variance for Kc for Fe3+ + SCN- Fe(SCN)2+ = 110%, the average value for kc = 186 Percent…

A:

Q: Determine the molar solubility of AgI (Ksp = 8.50e-17) in 2.981 M S2O32- if the complex ion…

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Q: Co(NH,), complex K,= 1.58 × 10 at 25 °C. For the aqueous %3D Suppose equal volumes of 0.0028M…

A: As Equal volume are taken Concentration of Co(NO3)3 = 0.0028 M2 = [Co3+]Concentration of Co(NO3)3…

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Q: Sufficient sodium cyanide, NaCN, was added to 2.5x10^-2 M silver nitrate, AgNO3, to give a solution…

A: Given: Molarity of AgNO3 = 2.5×10-2 MMolarity of CN- ion = 0.193 MKf for Ag(CN)2- = 5.6×1018

Q: Sufficient sodium cyanide, NaCN, was added to 1.5 x 10-2 M silver nitrate, AgNO3, to give a solution…

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Q: For the aqueous Hg(NH,), complex K, =1.8 x 10" at 25 °C. !! Suppose equal volumes of 0.0042 M…

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A: The answer to the following question is-

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A: Since you have asked multiple question, we will solve the first question for you.If you want any…

Q: A solution in part C initially contains (4.06x10^-4) molar SCN and (2.960x10^-3) molar Fe3+. This…

A: Given the initial concentration values of the reactants: [SCN-(aq)]i = 4.06*10-4 M [Fe3+(aq)]i =…

Q: In the second part of this experiment, a student makes a solution with initial concentrations of…

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Q: Solid KSCN was added to a 2.25 M Co²* solution so that it was also initially 2.25 M SCN¯. These ions…

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Q: For the aqueous [Hg(NH3)4]²* complex K, = 1.91 × 10¹⁹ at 25 °C. Suppose equal volumes of 0.0062 M…

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Q: Write the balanced chemical equation associated with the formation constant, Kf , for each complex…

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Q: A similar experiment as this lab is done as following: 0.456 g of solid AgCl is added a 25 mL…

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Q: Sufficient sodium cyanide, NaCN, was added to 2.5 x 10 ² M silver nitrate, AgNO3, to give a solution…

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Q: A sample of SrF₂ (Ksp = 4.33 x 10¹9) is dissolved in 0.025 M AIF3 solution. Calculate: a. Solubility…

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Q: Compare the solubility of cobalt(II) carbonate in each of the following aqueous solutions:   Clear…

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Q: A similar experiment as this lab is done as following: 0.456 g of solid AgCl is added a 25 mL…

A: Answer is explained below.

Q: Silver and ammonia may react to form Ag(NH₃)₂⁺ complex (Kf = 1.66 x 107). A 500 mL of 10 mol Ag⁺ and…

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Q: The formation constant K; for the complex ion Zn(OH)4² is 2.8 x 1015. What is the concentration of…

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Q: A similar experiment as this lab is done as following: 0.456 g of solid AgCl is added a 25 mL…

A: Answer is explained below.

Q: A solution is prepared such that the initial concentration of A2+ is 1.50×10-3 Mand the initial…

A: Initial concentration of [A2+] = 1.50×10-3M  Initial concentration of X = 4.60×10-3M  Equilibrium…