test tube mL Nickel standard ML 0.6 m H2SO4 blank 10.0 mL 2.0 mL 8.0 mL 2 4.0mL l6.0 mL 3 l6.0 mL 4.0 mL 4 8.0 mL 2.0 mL 10.0 mL 6-> fee board to the foft rmglme (10.0 mL) (62mg/mY20 mL) = M, (10.0mL) changes with TT
test tube mL Nickel standard ML 0.6 m H2SO4 blank 10.0 mL 2.0 mL 8.0 mL 2 4.0mL l6.0 mL 3 l6.0 mL 4.0 mL 4 8.0 mL 2.0 mL 10.0 mL 6-> fee board to the foft rmglme (10.0 mL) (62mg/mY20 mL) = M, (10.0mL) changes with TT
Chapter31: Introduction To Analytical Separations
Section: Chapter Questions
Problem 31.12QAP
Related questions
Question
Transcribed Image Text:test tube
mL Nickel standard
ML 0.6 m H2 S O4
blank
10.0 mL
2.0 mL
8.0mL
2
4.0mL
lo.0 mL
3
l6.0 mL
4.0 mL
4
8.0 mL
2.0 mL
10.0 mL
6> fee board to the left
rmglme
( ) = M, (10.0 mL)
62mg/mL)(20 mL)
Changes
with TT
Transcribed Image Text:218
Laboratory 17
Calculation of the Mole of Coordinated Ammonia Per Gram of Complex
The difference between the mole of HCl used to dissolve the complex and the mole of
NaOH used in the titration equals the mole of ammonia coordinated to Ni²+ in the complex.
Mole of coordinated ammonia:
4.2518
Mole of coordinated ammonia per gram of complex: . d504 mole NH,/g
Part III: Analysis of Nickel(11) in the Nickel Complex
Concentration of standard Ni2+ solution:le2
Mass of nickel complex used to prepare 50 mL of solution:
mg Ni2•/mL
Record all values in the table to three significant figures.
TEST TUBE
NUMBER
CONCENTRATION OF Ni2 IN mg/mL % TRANSMITTANCE
ABSORBANCE
12
1
0139
0, 232
3
e.323
0.410
D. 6 26
6
to be calculated
0323
Slope:
R2:
(Enter these values from the Regression Analysis computer program. 3 sig. figs. & use units)
Concentration of Ni2+ in solution of complex:
mg Ni2+/mL
Mass of Ni2+ in 50 mL of solution of complex:
g Ni2+
Number of mole of Ni2+ in dissolved sample:
mole Ni2+
(atomic weight of Ni = 58.71)
Number of mole of Ni2+ in 1.00 g of complex:
mole Ni2+/g
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