In: Chemistry
Table 1. Volumes of Solutions (mL) for Expirements 1 - 6.
Expirement | 0.20 M NaI | 0.20 M NaCl | 0.010 M Na2S2O3 | 2% Starch | 0.20 M K2SO4 |
0.20 M K2S2O8 |
1 | 2.00 | 2.00 | 2.00 | 1.00 | 2.00 | 2.00 |
2 | 2.00 | 2.00 | 2.00 | 1.00 | 0 | 4.00 |
3 | 4.00 | 0 | 2.00 | 1.00 | 2.00 | 2.00 |
4 (35˚C) | 2.00 | 2.00 | 2.00 | 1.00 | 2.00 | 2.00 |
5 (10˚C) | 2.00 | 2.00 | 2.00 | 1.00 | 2.00 | 2.00 |
6 (catalyst) | 2.00 | 2.00 | 2.00 | 1.00 | 2.00 | 2.00 |
Use the information from Table 1 to calculate the molarity of S2O82- and the molarity of I- in the test tubes for reactions 1 - 6. Hint: This is a dilution problem
Please show all work! Thank You.
Find the total volume of the solutions in test tube 1 = (2.00 + 2.00 + 2.00 + 1.00 + 2.00 + 2.00) mL = 11.0 mL.
Note that the final volume of the solutions is the same (=11.0 mL) in all the test tubes marked 2-6.
Work out the calculation for test tube 1 as a trial. Use the dilution equation.
M1*V1 = M2*V2 where V1 = volume of stock solution added; V2 = final volume of the solutions in all the test tubes (=11.0 mL); M1 = concentration of stock solution and M2 = concentration of the reagent in the final solution.
Start with S2O82- as shown below.
(2.00 mL)*(0.20 M) = (11.0 mL)*M2
===> M2 = (2.00*0.20 M)/(11.0) = 0.036 M (round off till the third decimal place.)
Next work with I- as shown below.
(2.00 mL)*(0.20 M) = (11.0 mL)*M2
===> M2 = (2.00*0.20 M)/(11.0) = 0.036 M (round off till the third decimal place.)
Treat the above two as sample calculations and work out the rest. Use the following data to present your data.
Experiment |
Vol. of 0.20 M K2S2O8 added (mL) |
Vol. of NaI added (mL) |
Concentration of S2O82- in the final solution (M) |
Concentration of I- in the final solution (M) |
1 |
2.00 |
2.00 |
0.036 |
0.036 |
2 |
4.00 |
2.00 |
0.073 |
0.036 |
3 |
2.00 |
4.00 |
0.036 |
0.073 |
4 |
2.00 |
2.00 |
0.036 |
0.036 |
5 |
2.00 |
2.00 |
0.036 |
0.036 |
6 |
2.00 |
2.00 |
0.036 |
0.036 |