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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+.

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+.

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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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 as sucrose (CH..n..) and mathonal (CH.OD de nnt fa ct Determination of FeSCN²* at equilibrium 3. Label four clean 10.00 mL volumetric flasks #1-4. Using pipets, carefully prepare the four couilibrium solutions described in Table 2 below. Transfer 5.00 mL of the 2.00 X 10-³ M iron nitrate solution (record the exact molarity shown) to a 10 mL volumetric flask. Add the appropriate volume of your freshly prepared HSCN stock solution directly to the volumetric flask. Dilute to the mark with 0.5 M nitric acid. Mix the solutions thoroughly. Measure the absorbance of each solution at the wavelength of maximum absorbance, 447 nm, in the spectrophotometer. 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 in Part B. 1- D. 138 20. asI 3- 0.397 4= 0.481 Table 2. Equilibrium Solutions Solution No. 2.00 X 10-3 M Fe(NO3)3 2.00 X 10-3 M HSCN 0.5 M HNO3 1 5.00 mL 5.00 mL 1.00 mL Dilute to the 2.00 mL 3.00 mL 4.00 mL 3 5.00 mL mark! 4 5.00 mL Calculations: Plan to work on these calculations in lab and organize your results in the tables that follow. Standard Solutions 1. Calculate the molarity of HSCN for each solution using MIV1 = M2V2. noiulo M1 = 2.00x10-3 M HSCN V2 = 25.00 mL Vị is given in Table 1 Find M2 for each. Answers will have 3 significant figures. 4.00x 10 M &00 x 10-5 144x10 2.00x106% Solution 1: Solution 2: -4 Solution 3: Solution 4: 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+. 1- 2x10-4M 2-4x 104 M 3-6x 10-4 M 4s 4=8x104M
Transcribed Image Text:NaCl and HNO, contain ions and thus conduct electricity. Solutions of nonelectrolytes such as sucrose (CH..n..) and mathonal (CH.OD de nnt fa ct Determination of FeSCN²* at equilibrium 3. Label four clean 10.00 mL volumetric flasks #1-4. Using pipets, carefully prepare the four couilibrium solutions described in Table 2 below. Transfer 5.00 mL of the 2.00 X 10-³ M iron nitrate solution (record the exact molarity shown) to a 10 mL volumetric flask. Add the appropriate volume of your freshly prepared HSCN stock solution directly to the volumetric flask. Dilute to the mark with 0.5 M nitric acid. Mix the solutions thoroughly. Measure the absorbance of each solution at the wavelength of maximum absorbance, 447 nm, in the spectrophotometer. 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 in Part B. 1- D. 138 20. asI 3- 0.397 4= 0.481 Table 2. Equilibrium Solutions Solution No. 2.00 X 10-3 M Fe(NO3)3 2.00 X 10-3 M HSCN 0.5 M HNO3 1 5.00 mL 5.00 mL 1.00 mL Dilute to the 2.00 mL 3.00 mL 4.00 mL 3 5.00 mL mark! 4 5.00 mL Calculations: Plan to work on these calculations in lab and organize your results in the tables that follow. Standard Solutions 1. Calculate the molarity of HSCN for each solution using MIV1 = M2V2. noiulo M1 = 2.00x10-3 M HSCN V2 = 25.00 mL Vị is given in Table 1 Find M2 for each. Answers will have 3 significant figures. 4.00x 10 M &00 x 10-5 144x10 2.00x106% Solution 1: Solution 2: -4 Solution 3: Solution 4: 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+. 1- 2x10-4M 2-4x 104 M 3-6x 10-4 M 4s 4=8x104M
A solution is a homogeneous mixture. A solution consists of a solvent, the substance in which something is dissolved, and one or more solutes the substance(s) dissolved in the solvent. In this chapter 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 as NaCl and HNO, contain ions and thus conduct electricity. Solutions of nonelectrolytes such as sucrose (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 stron electrolyte exists in produces only a sm an an Ionic compound: ions. Soluble alcohol are after 2 Fipette 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 beaker Procedure: 1. Preparation of the HSCN stock solution: マー35 meledocis carefully to be sure you are measuring out the correct solution and the corect molarity! 2. Preparation of the Beer's Law Calibration Plot for the FeSCN" Solutions: D.1x25 complex ion. The absorbance of these solutions will be measured and a Beer's Law Calibration plot 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 serious error, that all the HSCN is converted to the complex jon. The number of moles of the complex ion in each solution can be calculated from the number of moles of HSCN initially present in each solution. Label four clean 25.00 mL volumetric flasks #1-4 Using pipets, carefully prepare the four standard solutions describedin fable I below. Transfer 5.00 mL of the 0.200 M iron nitrate solution to a 25 mL volumetric flask. Add the appropriate volume of your freshly prepared HSCN stock solution directly to the volumetric flask. Dilute to the mark with 0.5 M nitric acid. Mix the solution thoroughly. Measure the absorbance of each solution at the wavelength of maximum absorbance, 447 nm, in the spectrophotometer. Use 0.5 M HNO3 for the reference solvent. Table 1. Standard Solutions Solution No. 0.200 M Fe(N03)3 2.00 X 103 M HSCN 0.5 M HNO3 alnedy added 5.00 mL 0.50 mL 1.00 mL 1.80 mL noed to 1 5.00 mL 5.00 mL Dilute to the mark! 3 4 5.00 mL 2.50 mL Note: The Fe(NO3)3 solution and the HSCN solution have been prepared using 0.50 M HNO3 as the solvent. Since these original solutions are 0.50 M in nitric acid and all dilutions will be made with 0.5 M nitric acid, then all resulting solutions will be 0.50 M in nitric acid. E 0. 189 2.0.376 3.0.666 4.0.912 44
Transcribed Image Text:A solution is a homogeneous mixture. A solution consists of a solvent, the substance in which something is dissolved, and one or more solutes the substance(s) dissolved in the solvent. In this chapter 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 as NaCl and HNO, contain ions and thus conduct electricity. Solutions of nonelectrolytes such as sucrose (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 stron electrolyte exists in produces only a sm an an Ionic compound: ions. Soluble alcohol are after 2 Fipette 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 beaker Procedure: 1. Preparation of the HSCN stock solution: マー35 meledocis carefully to be sure you are measuring out the correct solution and the corect molarity! 2. Preparation of the Beer's Law Calibration Plot for the FeSCN" Solutions: D.1x25 complex ion. The absorbance of these solutions will be measured and a Beer's Law Calibration plot 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 serious error, that all the HSCN is converted to the complex jon. The number of moles of the complex ion in each solution can be calculated from the number of moles of HSCN initially present in each solution. Label four clean 25.00 mL volumetric flasks #1-4 Using pipets, carefully prepare the four standard solutions describedin fable I below. Transfer 5.00 mL of the 0.200 M iron nitrate solution to a 25 mL volumetric flask. Add the appropriate volume of your freshly prepared HSCN stock solution directly to the volumetric flask. Dilute to the mark with 0.5 M nitric acid. Mix the solution thoroughly. Measure the absorbance of each solution at the wavelength of maximum absorbance, 447 nm, in the spectrophotometer. Use 0.5 M HNO3 for the reference solvent. Table 1. Standard Solutions Solution No. 0.200 M Fe(N03)3 2.00 X 103 M HSCN 0.5 M HNO3 alnedy added 5.00 mL 0.50 mL 1.00 mL 1.80 mL noed to 1 5.00 mL 5.00 mL Dilute to the mark! 3 4 5.00 mL 2.50 mL Note: The Fe(NO3)3 solution and the HSCN solution have been prepared using 0.50 M HNO3 as the solvent. Since these original solutions are 0.50 M in nitric acid and all dilutions will be made with 0.5 M nitric acid, then all resulting solutions will be 0.50 M in nitric acid. E 0. 189 2.0.376 3.0.666 4.0.912 44
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