Homework Answers
The solution for question 5 has been given as follows with the calculation and explanation part and the formula used to convert Transmittance to Absorbance.
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c. Complete the table to summarize your results for the preparation of copper(II) sulfate solutions. volume...
Show the calculations of the absorbance using the measured values of %T c. Complete the table...
Show the calculations of the absorbance using the measured
values of %T
c. Complete the table to summarize your results for the preparation of copper(II) sulfate solutions. Table 12-3. Preparation of copper|11) sulfate solutions. Amount of Volume of the Volume of the Concentration Volume of (M) CUSO, SH,0 Final Solution Concentrated (ml) Solution (ml) Water (ml) 0.50 497g 20mL 20 m 0.20 20mL 8mL lamL 0.10 20mL 10no L 10mL 0.05 20mL 10m 10m 5. Show the measured values of...
- Creating Solutions of Standard Molarity Having the measured absorbance of the made solutions, calculate th...
- Creating Solutions of Standard Molarity Having the measured absorbance of the made solutions, calculate the ACTUAL concentration of each solution (HINT: Use the equation of the line of best fit ob- Lained from Excel: A mM + b solve the equation for molarity M in terms of the absorbance A: slope, m; and intercept with the vertical axis b. Show your work.) Table 12-5. Comparison between the theoretical and actual concentration of the made Cul solutions Absorbance Actual Concentration...
Table A. Preparation of Standard solutions of FeSCN2+ 1.0 M HNO3 0.002 M 0.200 M Solution...
Table A. Preparation of Standard solutions of FeSCN2+ 1.0 M HNO3 0.002 M 0.200 M Solution KSCN (mL) Fe(NO3)3 (mL) 0.5 5 [FeSCN2+] (mol/L)* 1 4.0x10^-5 Add 1.0 M 2 1.0 5 8.0x10^-5 HNO3 3 1.5 5 1.2x10^-10 4 2.0 5 1.6x10-4 to each to adjust the volume to 25 mL. 5 2.5 5 2.0x10-4 * Calculate the concentrations of FeSCN2+ in each beaker, assuming that all SCN-ions exist as FeSCN2+. In other words, [FeSCN2+] (in Soln 1) = [SCN-]...
need help with the calculatiobs the bottom picture is what i got performing the experiment C....
need help with the calculatiobs the bottom picture is what i
got performing the experiment
C. Concentration Cells If both cell compartments contain copper metal and copper sulfate, the standard potential is 0.000 V and the Nernst equation becomes: Ercan = 0.000 volts (com dilute) volts Prepare a new cell, which has the beaker with 40 ml of 0.10 M CuSO. (from Part B) and 40 mL 0.0010 M Cuso. (from Part B) in an adjacent second one. Place copper...
Please complete the folllowing table! 9 HCI Molarity: 0.208 11 Preparation of Test Solutions Volume of...
Please complete the folllowing table!
9 HCI Molarity: 0.208 11 Preparation of Test Solutions Volume of Solution (mL) 12 Temperature of Solution (C) 15 Analysis of Test Solutions initial Buret Reading Buret Final Reading Volume of HQ Added (mL) 7.2 13 16 13 0.9 Data Analysis .Temperature x) 0.00304 000317 000316 0.00331 0.0034 0.00357 3 Moles of HC Used (mol) 0.0002496 0.0001872 0.0001664 0.000416 0.0002808 0.0001248 0.000104 0.0000936 832E-05| 1、Be sure to check the balanced equation for the reaction between...
Laboratory goggles must be worn! A) Preparation of Solutions from Concentrated Solution In this part the...
Laboratory goggles must be worn! A) Preparation of Solutions from Concentrated Solution In this part the experiment you will prepare several dilute solutions from the more concentrated cobalt nitrate solution 1. Read the label on the provided cobalt nitrate solution and record the molarity accurately. su-olu 563/ 316.603:48 صلاح 2. 3. 4. Molarity of Ca(NO3)2 solution 182.95 g/mol Obtain a 25-ml buret. Examine its markings, the line that spans the entire circumference occur for each milliliter. The smaller lines indicate...
7. The Absorption Spectrum of Cobalt(II) Chloride Procedure Getting Started 1. Your laboratory instructor may ask...
7. The Absorption Spectrum of Cobalt(II) Chloride Procedure Getting Started 1. Your laboratory instructor may ask that you work in groups rather than alone. 2. Obtain directions from your laboratory instructor for discarding the solutions that you will use in'! this experiment. 3. Obtain instructions for using your spectrophotometer. 4. Obtain your unknown. Making the Measurements 1. Mark each of 7 dry 18 x 150-mm test tubes with one of a series of identification numbers running from 1 to 7....
4. A volume of 30.0 mL of 0.10 M NH, (aq) is titrated with 0.20MCThe value of the base-dissociation (aq) constant, K, for HCO2 in water is 1.2 x 1010 at 25°C. a. (1 pt.) Write the ionic equation...
4. A volume of 30.0 mL of 0.10 M NH, (aq) is titrated with 0.20MCThe value of the base-dissociation (aq) constant, K, for HCO2 in water is 1.2 x 1010 at 25°C. a. (1 pt.) Write the ionic equation for the reaction of NH, (aq) with HCL(aq) (1 pt.) What is the volume of base added at the equivalence point? Show work or reasoning. b. (1 pt.) Will the pH of the equivalence point be higher than, lower than or...
help please? this was the only other information given REPORT SHEET Determination of the Solubility-Product Constant...
help please?
this was the only other information given
REPORT SHEET Determination of the Solubility-Product Constant for a Sparingly Soluble Salt EXPERIMENT 8 A. Preparation of a Calibration Curve Initial (Cro121 0.0024 M Absorbance 5 mL Volume of 0.0024 M K Cro Total volume 1. I mL 100 mL 2. 100ML 3. 10 mL 100ml 4. 15 mL 100 ML Molar extinction coefficient for [CrO2) [Cro,2) 2.4x100M 12x1044 2.4810M 3.6810M 0.04) 2037.37 0.85 1.13 2. 3. Average molar extinction coefficient...
just one example/demonstration! Data needed to be calculated is in highlighted in green boxes. And I...
just one example/demonstration!
Data needed to be calculated is in highlighted in green boxes.
And I highlighted in red an equation (not sure if thats what you
use to calculate it) And ignore the lab instructions on completeing
a graph!! I already know how to do that in excel, just curious how
Ln (relative rate) and 1/T in K^-1 is calculated by hand*
here is the rest of that lab leading up to the question as I
know its typically...
Show the calculations of the absorbance using the measured
values of %T
c. Complete the table to summarize your results for the preparation of copper(II) sulfate solutions. Table 12-3. Preparation of copper|11) sulfate solutions. Amount of Volume of the Volume of the Concentration Volume of (M) CUSO, SH,0 Final Solution Concentrated (ml) Solution (ml) Water (ml) 0.50 497g 20mL 20 m 0.20 20mL 8mL lamL 0.10 20mL 10no L 10mL 0.05 20mL 10m 10m 5. Show the measured values of...
- Creating Solutions of Standard Molarity Having the measured absorbance of the made solutions, calculate the ACTUAL concentration of each solution (HINT: Use the equation of the line of best fit ob- Lained from Excel: A mM + b solve the equation for molarity M in terms of the absorbance A: slope, m; and intercept with the vertical axis b. Show your work.) Table 12-5. Comparison between the theoretical and actual concentration of the made Cul solutions Absorbance Actual Concentration...
Table A. Preparation of Standard solutions of FeSCN2+ 1.0 M HNO3 0.002 M 0.200 M Solution KSCN (mL) Fe(NO3)3 (mL) 0.5 5 [FeSCN2+] (mol/L)* 1 4.0x10^-5 Add 1.0 M 2 1.0 5 8.0x10^-5 HNO3 3 1.5 5 1.2x10^-10 4 2.0 5 1.6x10-4 to each to adjust the volume to 25 mL. 5 2.5 5 2.0x10-4 * Calculate the concentrations of FeSCN2+ in each beaker, assuming that all SCN-ions exist as FeSCN2+. In other words, [FeSCN2+] (in Soln 1) = [SCN-]...
need help with the calculatiobs the bottom picture is what i
got performing the experiment
C. Concentration Cells If both cell compartments contain copper metal and copper sulfate, the standard potential is 0.000 V and the Nernst equation becomes: Ercan = 0.000 volts (com dilute) volts Prepare a new cell, which has the beaker with 40 ml of 0.10 M CuSO. (from Part B) and 40 mL 0.0010 M Cuso. (from Part B) in an adjacent second one. Place copper...
Please complete the folllowing table!
9 HCI Molarity: 0.208 11 Preparation of Test Solutions Volume of Solution (mL) 12 Temperature of Solution (C) 15 Analysis of Test Solutions initial Buret Reading Buret Final Reading Volume of HQ Added (mL) 7.2 13 16 13 0.9 Data Analysis .Temperature x) 0.00304 000317 000316 0.00331 0.0034 0.00357 3 Moles of HC Used (mol) 0.0002496 0.0001872 0.0001664 0.000416 0.0002808 0.0001248 0.000104 0.0000936 832E-05| 1、Be sure to check the balanced equation for the reaction between...
Laboratory goggles must be worn! A) Preparation of Solutions from Concentrated Solution In this part the experiment you will prepare several dilute solutions from the more concentrated cobalt nitrate solution 1. Read the label on the provided cobalt nitrate solution and record the molarity accurately. su-olu 563/ 316.603:48 صلاح 2. 3. 4. Molarity of Ca(NO3)2 solution 182.95 g/mol Obtain a 25-ml buret. Examine its markings, the line that spans the entire circumference occur for each milliliter. The smaller lines indicate...
7. The Absorption Spectrum of Cobalt(II) Chloride Procedure Getting Started 1. Your laboratory instructor may ask that you work in groups rather than alone. 2. Obtain directions from your laboratory instructor for discarding the solutions that you will use in'! this experiment. 3. Obtain instructions for using your spectrophotometer. 4. Obtain your unknown. Making the Measurements 1. Mark each of 7 dry 18 x 150-mm test tubes with one of a series of identification numbers running from 1 to 7....
4. A volume of 30.0 mL of 0.10 M NH, (aq) is titrated with 0.20MCThe value of the base-dissociation (aq) constant, K, for HCO2 in water is 1.2 x 1010 at 25°C. a. (1 pt.) Write the ionic equation for the reaction of NH, (aq) with HCL(aq) (1 pt.) What is the volume of base added at the equivalence point? Show work or reasoning. b. (1 pt.) Will the pH of the equivalence point be higher than, lower than or...
help please?
this was the only other information given
REPORT SHEET Determination of the Solubility-Product Constant for a Sparingly Soluble Salt EXPERIMENT 8 A. Preparation of a Calibration Curve Initial (Cro121 0.0024 M Absorbance 5 mL Volume of 0.0024 M K Cro Total volume 1. I mL 100 mL 2. 100ML 3. 10 mL 100ml 4. 15 mL 100 ML Molar extinction coefficient for [CrO2) [Cro,2) 2.4x100M 12x1044 2.4810M 3.6810M 0.04) 2037.37 0.85 1.13 2. 3. Average molar extinction coefficient...
just one example/demonstration!
Data needed to be calculated is in highlighted in green boxes.
And I highlighted in red an equation (not sure if thats what you
use to calculate it) And ignore the lab instructions on completeing
a graph!! I already know how to do that in excel, just curious how
Ln (relative rate) and 1/T in K^-1 is calculated by hand*
here is the rest of that lab leading up to the question as I
know its typically...
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