Processing kodak motion picture films, module 3 analytical procedures
Processing kodak motion picture films, module 3 analytical procedures
Processing kodak motion picture films, module 3 analytical procedures
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APPENDIX B<br />
This appendix contains two assay <strong>procedures</strong> for Ferrous<br />
Ammonium Sulfate. The first procedure uses Potassium<br />
Dichromate; while the alternate procedure uses Potassium<br />
Permanganate titrant.<br />
Assay Procedure for Ferrous Ammonium<br />
Sulfate, Hexahydrate<br />
Reagents<br />
All reagents are ACS Reagent Grade unless otherwise stated.<br />
Potassium Dichromate, K2Cr2O7 , NIST Primary<br />
Standard, 136e, dried for 2 hours at 110°C<br />
Ferroin Indicator, 1,10-Phenanthroline Iron(II) Sulfate<br />
solution (0.025 M) [(C 12 H 8 N 2 ) 3 FeSO 4 ]<br />
Sulfuric Acid, concentrated, H 2 SO 4<br />
Ferrous Ammonium Sulfate-6-Hydrate,<br />
Fe(NH 4 ) 2 (SO 4 ) 2 6H 2 O<br />
Procedure<br />
1. Weigh 14.0 g of ferrous ammonium sulfate,<br />
hexahydrate to the nearest 0.0001 g and record the<br />
weight.<br />
2. Quantitatively transfer to a 200-mL volumetric flask<br />
and swirl the flask to dissolve the ferrous ammonium<br />
sulfate.<br />
3. Dilute the solution to the mark with reagent water.<br />
Invert the flask, 6-10 times, to thoroughly mix.<br />
4. Weigh 1.0 g of dried, potassium dichromate to the<br />
nearest 0.0001 g and record the weight.<br />
5. Quantitatively transfer to a 100-mL volumetric flask<br />
containing 50 mL of reagent water. Swirl the flask to<br />
dissolve the potassium dichromate.<br />
6. Dilute the solution to the mark with reagent water.<br />
Invert the flask, 6-10 times, to mix thoroughly.<br />
7. Fill a 50-mL buret with the ferrous ammonium sulfate<br />
solution (step 3, above).<br />
8. Add 20 mL concentrated sulfuric acid to a 150-mL<br />
beaker containing 25 mL of reagent water and a<br />
magnetic stirring bar.<br />
Caution<br />
Hot acid solution is formed.<br />
9. Pipet 15.0 mL of the potassium dichromate solution<br />
into the beaker.<br />
10. Add 2 drops of ferroin indicator to the beaker and<br />
place the beaker on a magnetic stirrer.<br />
11. Slowly add the ferrous ammonium sulfate solution<br />
from the buret to the beaker. The solution will change<br />
colors as the titrant is added, going from a green-blue<br />
color to a reddish-brown color. The point that<br />
produced the first reddish-brown color change is the<br />
end point.<br />
12. Record the volume of ferrous ammonium sulfate<br />
titrant consumed at the end point to the nearest<br />
0.05 mL.<br />
13. Repeat steps 7-12, two more times.<br />
Calculations<br />
N Potassium Dichromate<br />
where:<br />
N K 2 Cr 2 O 7 =<br />
N of Ferrous Ammonium Sulfate<br />
N Fe(NH4 ) 2 (SO4 ) 2<br />
where:<br />
= (mL K2Cr2O7 )(N K2Cr2O7 )<br />
mL Fe(NH4) 2(SO4) 2<br />
g/L, Iron(II) in Ferrous Ammonium Sulfate<br />
g/L, Iron(II) (actual)<br />
where:<br />
= N Fe(NH4 ) 2 (SO4 ) 2 x 55.85<br />
Theoretical wt of Ferrous in Solution<br />
Assay Percentage<br />
g wt of K2Cr2O7 1000<br />
x<br />
100 mL 294.2/6<br />
294.2/6 = the eq. wt of K2Cr2O7 g wt of K2Cr2O7 = recorded wt from step 4<br />
1000 = factor to convert equivalents to<br />
milliequivalents<br />
mL Fe(NH4 ) 2 (SO4 ) 2 =average * volume of the three titrations<br />
required to reach the end point color<br />
change<br />
mL K2Cr2O7 = 15.0 mL<br />
N K2Cr2O7 = normality calculated in N Potassium<br />
Dichromate<br />
* The average volume for the three titrations should not have a standard<br />
deviation (1s) greater than 0.50 mL.<br />
55.85 =<br />
gram-equivalent weight of Iron(II) in<br />
Fe(NH 4) 2(SO 4) 2 6H 2O<br />
g/L<br />
iron(II)<br />
where:<br />
= wt of Fe(NH4 ) 2 (SO4 ) 2 6H2O x 55.85 200 mL 391.85<br />
1000 mL<br />
x<br />
1L<br />
391.85 = molecular weight of ferrous<br />
ammonium sulfate, 6-hydrate<br />
55.85 = atomic weight of iron<br />
wt of Fe(NH4 ) 2 (SO4 ) 2 6H2O = weight recorded in step 1 of<br />
this procedure.<br />
1000 mL = factor to convert mL to L<br />
%Iron(II) =<br />
g/L Iron(II) (actual)<br />
g/L Iron(II) (theoretical)<br />
x 100<br />
<strong>Processing</strong> KODAK Motion Picture Films, Module 3, Analytical Procedures H24.03 5