|
Solution 1 |
Solution 2 |
|
|
Toluene |
1.7 mL |
1.5 mL |
|
1,2-dicloroethane |
1.5mL |
3.0 mL |
|
p-xylene |
0 |
3.0 mL |
|
Total volume |
10 mL |
10 mL |
|
Concentration |
||
Tetrachloroethylene was used to bring both solutions to the total volume. What is the concentration for the three analytes in each solution?

Solution 1 Solution 2 Toluene 1.7 mL 1.5 mL 1,2-dicloroethane 1.5mL 3.0 mL p-xylene 0 3.0...
Pure solid NaH2PO4 is dissolved in distilled water, making 100.00 ml of solution. 10.00ml of this solution is diluted to 100.00 ml to prepare the original phosphate standard solution. Three working standard solutions are made from this by pipetting 0.8ml, 1.5ml and 3.0 ml of the original standard solution into 100.00 ml volumetric flasks. Acid and molybdate reagent are added and the solutions are diluted to 100.00 ml. You may assume that all these absorbance measurements have already been corrected...
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In the simulation below, you will be working with a 10.00 mL
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values used for table 2
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Experiment V. Equilibrium Constant Lab Report ( 50 pts) Calibration Curve 1. Record the absorbance for each of the standard solutions in the table below. Calculate the concentration of FeSCN)" in each of the standard solutions and record the values in the table below. Show a sample calculation (for A2) of your work in the space below the table. Solution Absorbance [Fe(SCN)" A-1 A-2 A-3 0.000 0.390 0.535...
1.
2.
Using the equation C1V1 = C2V2, calculate the volume (V1) of concentrated solution and the volume of water needed to dilute the following solutions: Concentration Volume (in mls) Concentration of Volume (in mls) of Volume (in mls) of diluted of desired available stock stock solution required of solvent solution desired solution (V2) solution (C1) to make the diluted required to (C2) solution (V1) achieve desired volume (V2-V1) 5 mg/ml 100 ml 1000 mg/ml 15% 10 ml 50% 0.250...
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