I’m not sure if I did question 2 right. Calculate the molar it you if FeSCN2+ NaCl and HNO, contain ions and thus conduct electricity. Solutions of nonelectrolytes such assucrose (CH..n..) and mathonal (CH.OD de nnt factDetermination of FeSCN²* at equilibrium3.Label four clean 10.00 mL volumetric flasks #1-4. Using pipets, carefully prepare the fourcouilibrium solutions described in Table 2 below. Transfer 5.00 mL of the 2.00 X 10-³ M ironnitrate solution (record the exact molarity shown) to a 10 mL volumetric flask. Add theappropriate volume of your freshly prepared HSCN stock solution directly to the volumetricflask. Dilute to the mark with 0.5 M nitric acid. Mix the solutions thoroughly. Measure theabsorbance of each solution at the wavelength of maximum absorbance, 447 nm, in thespectrophotometer. Use the same instrument you used in Part B.Note that the concentration of the Fe(NO.)a is 100 times less concentrated than that used inPart B.1- D. 13820. asI3- 0.3974= 0.481Table 2. Equilibrium SolutionsSolution No.2.00 X 10-3 M Fe(NO3)32.00 X 10-3 M HSCN0.5 M HNO315.00 mL5.00 mL1.00 mLDilute to the2.00 mL3.00 mL4.00 mL35.00 mLmark!45.00 mLCalculations: Plan to work on these calculations in lab and organize your results in the tablesthat follow.Standard Solutions1. Calculate the molarity of HSCN for each solution using MIV1 = M2V2.noiuloM1 = 2.00x10-3 M HSCNV2 = 25.00 mLVị is given in Table 1Find M2 for each. Answers will have 3 significant figures.4.00x 10 M&00 x 10-5144x102.00x106%Solution 1:Solution 2:-4Solution 3:Solution 4:2. Calculate the molarity of FeSCN²* in each of the standard solutions, assuming that the initialconcentration of HSCN is equivalent to the concentration of the complex, FeSCN²+.1- 2x10-4M2-4x 104 M3-6x 10-4 M 4s4=8x104M A solution is a homogeneous mixture. A solution consists of a solvent, the substance in whichsomething is dissolved, and one or more solutes the substance(s) dissolved in the solvent. In thischapter we will focus on aqueous solutions in which water is the dissolving medium, or solvent.Solutes come in two varieties: electrolytes and nonelectrolytes Solutions of electrolytes such asNaCl and HNO, contain ions and thus conduct electricity. Solutions of nonelectrolytes such assucrose (C12HO1) and methanol (CH,OH) do not form ions in solution and thus do not conduct.electricity. An electrc---m ha mither a strong electrolyte or a weak electrolyte. A stronelectrolyte exists inproduces only a sman anIonic compound:ions. Solublealcohol areafter 2Fipette 10.00 mL of the 0 01M KSCN (record the exact molarity shown on the stock bottle)clean 50.00 mL volumetric flaskt pilute to the mark with 0.5 M HNO3. Mix well.Transfer the prepared solution to a clean, dry, labeled beakerProcedure:1. Preparation of the HSCN stock solution:マー35meledocis carefully to be sure you are measuring out the correct solution and the corectmolarity!2. Preparation of the Beer's Law Calibration Plot for the FeSCN" Solutions:D.1x25complex ion. The absorbance of these solutions will be measured and a Beer's Law Calibrationplot will be constructed.Note: The concentration of the Fe(NO:)a is much, much greater than the HSCN concentration;this forces the equilibrium completely to the right. It can therefore be assumed, without seriouserror, that all the HSCN is converted to the complex jon. The number of moles of the complexion in each solution can be calculated from the number of moles of HSCN initially present ineach solution.Label four clean 25.00 mL volumetric flasks #1-4 Using pipets, carefully prepare the fourstandard solutions describedin fable I below. Transfer 5.00 mL of the 0.200 M iron nitratesolution to a 25 mL volumetric flask. Add the appropriate volume of your freshly preparedHSCN stock solution directly to the volumetric flask. Dilute to the mark with 0.5 M nitricacid. Mix the solution thoroughly. Measure the absorbance of each solution at the wavelengthof maximum absorbance, 447 nm, in the spectrophotometer. Use 0.5 M HNO3 for the referencesolvent.Table 1. Standard SolutionsSolution No.0.200 M Fe(N03)32.00 X 103 M HSCN0.5 M HNO3alnedy added5.00 mL0.50 mL1.00 mL1.80 mLnoedto15.00 mL5.00 mLDilute to themark!345.00 mL2.50 mLNote: The Fe(NO3)3 solution and the HSCN solution have been prepared using 0.50 M HNO3as the solvent. Since these original solutions are 0.50 M in nitric acid and all dilutions will bemade with 0.5 M nitric acid, then all resulting solutions will be 0.50 M in nitric acid.E 0. 1892.0.3763.0.6664.0.91244

Question

I’m not sure if I did question 2 right. Calculate the molar it you if FeSCN2+ NaCl and HNO, contain ions and thus conduct electricity. Solutions of nonelectrolytes such assucrose (CH..n..) and mathonal (CH.OD de nnt factDetermination of FeSCN²* at equilibrium3.Label four clean 10.00 mL volumetric flasks #1-4. Using pipets, carefully prepare the fourcouilibrium solutions described in Table 2 below. Transfer 5.00 mL of the 2.00 X 10-³ M ironnitrate solution (record the exact molarity shown) to a 10 mL volumetric flask. Add theappropriate volume of your freshly prepared HSCN stock solution directly to the volumetricflask. Dilute to the mark with 0.5 M nitric acid. Mix the solutions thoroughly. Measure theabsorbance of each solution at the wavelength of maximum absorbance, 447 nm, in thespectrophotometer. Use the same instrument you used in Part B.Note that the concentration of the Fe(NO.)a is 100 times less concentrated than that used inPart B.1- D. 13820. asI3- 0.3974= 0.481Table 2. Equilibrium SolutionsSolution No.2.00 X 10-3 M Fe(NO3)32.00 X 10-3 M HSCN0.5 M HNO315.00 mL5.00 mL1.00 mLDilute to the2.00 mL3.00 mL4.00 mL35.00 mLmark!45.00 mLCalculations: Plan to work on these calculations in lab and organize your results in the tablesthat follow.Standard Solutions1. Calculate the molarity of HSCN for each solution using MIV1 = M2V2.noiuloM1 = 2.00x10-3 M HSCNV2 = 25.00 mLVị is given in Table 1Find M2 for each. Answers will have 3 significant figures.4.00x 10 M&00 x 10-5144x102.00x106%Solution 1:Solution 2:-4Solution 3:Solution 4:2. Calculate the molarity of FeSCN²* in each of the standard solutions, assuming that the initialconcentration of HSCN is equivalent to the concentration of the complex, FeSCN²+.1- 2x10-4M2-4x 104 M3-6x 10-4 M 4s4=8x104M A solution is a homogeneous mixture. A solution consists of a solvent, the substance in whichsomething is dissolved, and one or more solutes the substance(s) dissolved in the solvent. In thischapter we will focus on aqueous solutions in which water is the dissolving medium, or solvent.Solutes come in two varieties: electrolytes and nonelectrolytes Solutions of electrolytes such asNaCl and HNO, contain ions and thus conduct electricity. Solutions of nonelectrolytes such assucrose (C12HO1) and methanol (CH,OH) do not form ions in solution and thus do not conduct.electricity. An electrc---m ha mither a strong electrolyte or a weak electrolyte. A stronelectrolyte exists inproduces only a sman anIonic compound:ions. Solublealcohol areafter 2Fipette 10.00 mL of the 0 01M KSCN (record the exact molarity shown on the stock bottle)clean 50.00 mL volumetric flaskt pilute to the mark with 0.5 M HNO3. Mix well.Transfer the prepared solution to a clean, dry, labeled beakerProcedure:1. Preparation of the HSCN stock solution:マー35meledocis carefully to be sure you are measuring out the correct solution and the corectmolarity!2. Preparation of the Beer's Law Calibration Plot for the FeSCN&#34; Solutions:D.1x25complex ion. The absorbance of these solutions will be measured and a Beer's Law Calibrationplot will be constructed.Note: The concentration of the Fe(NO:)a is much, much greater than the HSCN concentration;this forces the equilibrium completely to the right. It can therefore be assumed, without seriouserror, that all the HSCN is converted to the complex jon. The number of moles of the complexion in each solution can be calculated from the number of moles of HSCN initially present ineach solution.Label four clean 25.00 mL volumetric flasks #1-4 Using pipets, carefully prepare the fourstandard solutions describedin fable I below. Transfer 5.00 mL of the 0.200 M iron nitratesolution to a 25 mL volumetric flask. Add the appropriate volume of your freshly preparedHSCN stock solution directly to the volumetric flask. Dilute to the mark with 0.5 M nitricacid. Mix the solution thoroughly. Measure the absorbance of each solution at the wavelengthof maximum absorbance, 447 nm, in the spectrophotometer. Use 0.5 M HNO3 for the referencesolvent.Table 1. Standard SolutionsSolution No.0.200 M Fe(N03)32.00 X 103 M HSCN0.5 M HNO3alnedy added5.00 mL0.50 mL1.00 mL1.80 mLnoedto15.00 mL5.00 mLDilute to themark!345.00 mL2.50 mLNote: The Fe(NO3)3 solution and the HSCN solution have been prepared using 0.50 M HNO3as the solvent. Since these original solutions are 0.50 M in nitric acid and all dilutions will bemade with 0.5 M nitric acid, then all resulting solutions will be 0.50 M in nitric acid.E 0. 1892.0.3763.0.6664.0.91244

Accepted Answer

Answered: Image /qna-images/answer/5c868849-c36d-45ef-b619-5a5e467f710f.jpg

2. Calculate the molarity of FESCN²* in each of the standard solutions, assuming that the initial concentration of HSCN is equivalent to the concentration of the complex, FeSCN2+.