21
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A Contribution to the Study of the Oxidation Potential of the Berkelium (III)-(IV) Couple in Various Media C. MUSIKAS and R. BERGER Department de Chimie, Services de Chimie des Combustibles Irradies, Section d'Etudes Chimiques et Radioactives, Commisariat a l'Energie Atomique, Centre d'Etudes Nucléaires, Fontenay aux Roses, France
Indirect determinations of the formal oxidation potential of Bk(IV)—Bk(III) couple in sulfuric and nitric acids have been made by tracer measurement. From the Bk(IV)/Bk(III) ratios and the corresponding Ce(IV)/Ce(III) ratios at equilibrium conditions one can calculate the oxidation potential of the Bk(IV)-Bk(III) couple. The Bk(IV)/Bk(III) ratio can be determined by extracting Bk(IV) by an appropriate organic solvent. The formal oxidation potentials of the Bk(IV)Bk(III) couple in 1N and 0.5N sulfuric acid were found to be 1.42 and 1.44 volts using trilaurylmethylammonium sulfate in carbon tetrachloride as a solvent. In 6N nitric acid the oxidation potential of the couple was found to be 1.56 volts by using 0.18M tributylphosphate. Whereas, in 1N to 2N nitric acid berkelium was not oxidized by cerium(IV).
/ ~ \ x i d a t i o n of b e r k e l i u m to t h e tetravalent state w a s d e m o n s t r a t e d i n 1950 b y T h o m p s o n , C u n n i n g h a m , a n d S e a b o r g
(7).
Using
eerie
i o d a t e as a t e t r a v a l e n t species c a r r i e r f o r tracer experiments, t h e y f o u n d that i n 8N H N 0
3
m e d i u m t h e f o r m a l o x i d a t i o n potentials of t h e C e ( I V ) -
C e ( I I I ) a n d t h e B k ( I V ) - B k ( I I I ) couples w e r e n e a r l y t h e same. I n t h e same y e a r Jones a n d C u n n i n g h a m c o n t i n u e d these e x p e r i ments (2)
a n d f o u n d t h a t the c e r i u m a n d t h e b e r k e l i u m a d s o r p t i o n o n
z i r c o n i u m p h e n y l a r s o n a t e c a r r i e r w e r e s i m i l a r regardless of t h e o x i d i z i n g agent ( b i c h r o m a t e , c h l o r a t e , h y p o c h l o r i t e , or b r o m a t e ) , or t h e m e d i u m ( I N n i t r i c a c i d , 1 M l i t h i u m p e r e h l o r a t e - p e r e h l o r i c a c i d at h y d r o g e n i o n 296
Fields and Moeller; Lanthanide/Actinide Chemistry Advances in Chemistry; American Chemical Society: Washington, DC, 1967.
21.
MusiKAs
A N D
Oxidation
B E R G E R
concentrations f r o m 0 . 1 N to I N ) .
297
Potential
F r o m these experiments t h e y
con-
c l u d e d t h a t the o x i d a t i o n p o t e n t i a l of the B k ( I V ) - B k ( I I I ) c o u p l e d i d not differ b y m o r e t h a n 60 m v . f r o m that of the C e ( I V ) - C e ( I I I )
couple.
I n o r d e r to c o m p l e t e these experiments w e u n d e r t o o k tracer l e v e l measurements of the f o r m a l o x i d a t i o n p o t e n t i a l of the B k ( I V ) - B k ( I I I ) c o u p l e i n n i t r i c a c i d a n d s u l f u r i c a c i d solutions, u s i n g the
Ce(IV)-
C e ( I I I ) c o u p l e as a m e d i a t o r . T h e tetravalent species w e r e extracted b y Downloaded by UNIV OF CALIFORNIA SAN DIEGO on March 18, 2016 | http://pubs.acs.org Publication Date: June 1, 1967 | doi: 10.1021/ba-1967-0071.ch021
o r g a n i c solvents. A s i m i l a r m e t h o d was u s e d b y M a t s u u r a a n d H a i s s i n s k y i n 1958
(4)
a n d b y H a i s s i n s k y a n d P l u c h e t i n 1962 ( I ) for d e t e r m i n i n g the f o r m a l o x i d a t i o n potentials of
the P o ( V I ) - P o ( I V )
a n d the
Pa(V)-Pa(IV)
couples r e s p e c t i v e l y . W e took a d v a n t a g e of the p r o p e r t y of different solvents to extract selectively the tetravalent a c t i n i d e a n d l a n t h a n i d e elements. t h e m are sufficiently stable i n the presence of o x i d i z i n g agents. the o r g a n o n i t r o g e n a n d o r g a n o p h o s p h o r u s
Some
of
Among
compounds we used were t r i -
l a u r y l m e t h y l a m m o n i u m ( T L M A ) salts a n d t r i b u t y l p h o s p h a t e ( T B P ) i n carbon tetrachloride.
Principle of the Method T h e f o r m a l o x i d a t i o n p o t e n t i a l of the B k ( I V ) - B k ( I I I ) c o u p l e c a n b e deduced
f r o m N e r n s t s l a w i f the d i s t r i b u t i o n e q u i l i b r i a b e t w e e n
aqueous phase a n d the n o n m i s c i b l e o r g a n i c phase is r e a c h e d .
the
This can
be w r i t t e n as: E
i
EU
_ -
F f
Ef
ce
+ M [Ce(IV)] + - p - log [
C
e
(
m
)
L
a
X
[Bk(III)]. (IV)]
[ B k
e
m ( 1 )
i n w h i c h the concentrations are aqueous concentrations after extraction. T h e different terms of E q u a t i o n 1 w e r e o b t a i n e d as f o l l o w s — E f , f o r m a l p o t e n t i a l of the C e ( I V ) - C e ( I I I ) c o u p l e i n the m e d i u m , w a s taken from publications; [ C e ( I V ) ] and [ C e ( I V ) ] have been measured b y direct absorption spectrophotometry; [ C e ( I I I ) ] was c a l c u l a t e d b y difference b e t w e e n t o t a l c e r i u m , t i t r a t e d b y p o t e n t i o m e t r y , a n d t e t r a v a l e n t c e r i u m ; [ B k ( I V ) ] was c a l c u l a t e d f r o m the solvent b e t a c o u n t i n g , a l l o w i n g for the m e a s u r e d d i s t r i b u t i o n coefficient of B k ( I V ) ; [ B k ( I I I ) ] was d e t e r m i n e d b y s u b t r a c t i n g the [ B k ( I V ) ] v a l u e f r o m the aqueous c o u n t i n g ; i n a l l cases [ C e ( I I I ) ] a n d [ B k ( I I I ) ] w e r e f o u n d to b e negligible. Ce
a
0
f f
a
a
a
0
0
T o t a l oxidation a n d extraction e q u i l i b r i u m were verified b y p l o t t i n g : [Bk(IV)]
w
[Ce ( I V ) ] q
a
- W i n n : ° i^mm: a n d c h e c k i n g to see that the slope of the straight l i n e w a s close to 1. l
o
g
m
l o g l
Fields and Moeller; Lanthanide/Actinide Chemistry Advances in Chemistry; American Chemical Society: Washington, DC, 1967.
298
LANTHANIDE /ACTINIDE
CHEMISTRY
Preliminary Experiments T o d e t e r m i n e t h e aqueous a n d o r g a n i c concentrations of t h e tetrav a l e n t c e r i u m a n d b e r k e l i u m w i t h sufficient a c c u r a c y , i t w a s necessary % initial. Cerium (IV)
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100 0.05 M TLMA sulfate . C C U 90 H
A
80
0.1 M
704
60
0,08M
50
TLA
1h
Figure 1.
Reduction
TLMA-HNOs.CCU
sulfate.CCU
• Time hours 3h
2h
rate of cerium(IV)
in various organic solvents
% initial Cerium (IV)
1N H2S04
100 1N
H 2 S O 4 - I N HNOs
1N HCUK
8 Time hours
Figure 2.
Reduction
rate of cerium(IV)
in various aqueous media
Fields and Moeller; Lanthanide/Actinide Chemistry Advances in Chemistry; American Chemical Society: Washington, DC, 1967.
21.
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Optical
MusrxAs
Oxidation
Potential
299
density
Figure 3.
Optical
A N D B E R G E R
A:1N
H z S O J » non electrolysed
Β · 1N
Ht SOùt
electrolysed
(used
for
dilutions)
Effect of the electrolytic oxidation of sulfuric acid on Beers lines at 380 mμ for cerium(IV)
density
straight
A : 1N HeSOt aqueous Β : 0.18 M T B P - CCI 4
A
C:
Figure 4.
0.05M
TLMA sulfate. C C U .
Absorption of cerium(IV) at 380 m μ in various media
to find a solvent i n w h i c h the d i s t r i b u t i o n coefficients of these t w o tetra v a l e n t species b e t w e e n the solvent a n d the chosen aqueous m e d i u m w a s i n the r a n g e 0.1 to 10. I n a d d i t i o n the o x i d a t i o n rate of the solvent b y the t e t r a v a l e n t elements s h o u l d be sufficiently l o w . F o r s u l f u r i c a c i d solutions, t r i l a u r y l m e t h y l a m m o n i u m sulfate i n c a r b o n t e t r a c h l o r i d e w a s p r e f e r r e d to t r i l a u r y l a m i n e sulfate because i t is less sensitive to o x i d a t i o n b y c e r i u m ( I V ) ( F i g u r e 1 ). I n the case of n i t r i c a c i d , t r i b u t y l p h o s p h a t e
Fields and Moeller; Lanthanide/Actinide Chemistry Advances in Chemistry; American Chemical Society: Washington, DC, 1967.
300
LANTHANIDE /ACTINIDE
CHEMISTRY
i n c a r b o n t e t r a c h l o r i d e gives h i g h e r d i s t r i b u t i o n coefficients for b e r k e l i u m t h a n t r i l a u r y l m e t h y l a m m o n i u m n i t r a t e i n the same d i l u e n t . B e c a u s e the r e d u c t i o n rate of c e r i u m ( I V )
i n these solvents is not
n e g l i g i b l e , i t is necessary to take samples for b e t a c o u n t i n g a n d spectrophotometry? analysis at the same t i m e . T h e c o n c e n t r a t i o n of c e r i u m ( I V ) w a s d e t e r m i n e d b y d i r e c t a b s o r p t i o n s p e c t r o p h o t o m e t r y at 380 m/x, b o t h i n aqueous a n d i n o r g a n i c solutions. T h i s w a v e l e n g t h was chosen i n o r d e r
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to a v o i d a n y i n t e r f e r e n c e b y the reagents. I n s u l f u r i c a c i d , t e t r a v a l e n t c e r i u m is m o r e stable t h a n i n the other a q u e o u s solutions ( F i g u r e 2 ) .
F o r this reason I N H S 0 2
the m e d i u m for s p e c t r o p h o t o m e t r i c measurements.
4
was chosen as
N e v e r t h e l e s s i t was
necessary to o x i d i z e e l e c t r o l y t i c a l l y a l l the reagents b e f o r e the spectrop h o t o m e t r i c measurements.
T h i s is i l l u s t r a t e d b y F i g u r e 3 i n w h i c h the
o p t i c a l densities vs. the c e r i u m ( I V ) concentrations are p l o t t e d . T h e v e r i f i c a t i o n of L a m b e r Beer's l a w is s h o w n i n F i g u r e 4.
Organic
solutions of c e r i u m w e r e p r e p a r e d b y e x t r a c t i n g c e r i u m ( I V ) f r o m t i t r a t e d a q u e o u s solutions a n d s t a n d a r d i z e d b y b e t a c o u n t i n g of
1 4 1
C e tracer.
S t a n d a r d i z a t i o n curves w e r e p l o t t e d f r o m three values for f u r t h e r spect r o p h o t o m e t r i c d e t e r m i n a t i o n s of c e r i u m ( I V ) . T h e b e r k e l i u m ( I V ) e x t r a c t i o n coefficients h a v e b e e n d e t e r m i n e d b y s t r i p p i n g solvents p r e v i o u s l y l o a d e d w i t h t e t r a v a l e n t c e r i u m a n d b e r k e l i u m i n the presence of s o d i u m b i s m u t h a t e .
Sodium bismuthate
has
b e e n f o u n d to be a n efficient o x i d i z i n g agent for t r i v a l e n t c e r i u m . B e c a u s e of its s m a l l s o l u b i l i t y i t does not affect the d i s t r i b u t i o n coefficients
of
tetravalent cerium.
by
These two properties have been demonstrated
c o m p a r i n g the d i s t r i b u t i o n coefficients of c e r i u m ( I V ) m e a s u r e d b y spect r o p h o t o m e t r y w i t h those of c e r i u m o x i d i z e d b y s o d i u m b i s m u t h a t e a n d m e a s u r e d b y b e t a c o u n t i n g of the
1 4 3
c e r i u m isotope tracer. T h e d a t a are
s u m m a r i z e d i n T a b l e I a n d i n d i c a t e no r e a l difference i n the d i s t r i b u t i o n coefficients
of c e r i u m o b t a i n e d b y these t w o m e t h o d s
when using tri-
l a u r y l m e t h y l a m m o n i u m s a l t s - c a r b o n t e t r a c h l o r i d e as solvent. Table I.
Effect of Sodium Bismuthate on the Distribution Coefficients of Cerium (IV) E° a
Organic 0.05M TLMA-Sulfate
Spectrophotometric Determination of Ce(IV)
Aqueous 0.5N H S 0 2
0.1M TLMA-Sulfate
IN H S0
0.1M T L M A - H N O ; ,
I N HNO
0.1M TLMA-HNO3
6N H N O 3
2
4
; î
4
Ce(IV) Beta Counting of Ce (-bNaBiOs) ni
7.7
7.4
2.6
2.7
110
78
200
240
Fields and Moeller; Lanthanide/Actinide Chemistry Advances in Chemistry; American Chemical Society: Washington, DC, 1967.
21.
MusiKAS
Oxidation
A N D BERGER
301
Potential
Table II. 0.1M Trilaurylmethylammonium Nitrate—Carbon Tetrachlo ride Extraction of Cerium and Berkelium from N i t r i c A c i d Solutions in the Presence of Sodium Bismuthate
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Aqueous IN IN IN 4N 4N 6N 6N 8N ΙΟΝ
HN0 HNO3 HNO3 HNO3 HNO3 HNO3 HNO3 HNO3 HNO3
E° a
3
+
1.5M A l ( N O )
H
+
1.5M A 1 ( N 0 ) ,
s
3
H
1 1 65 12 20 6 9 3.6 2
110 110 100 100 100 100 100
3
(without N a B i O ) + 1.5M A 1 ( N 0 )
% of Initial Bk Extracted
Ce(IV)
3
C e ( I V ) initial aqueous concentration = 6.0 X 1 0 " M E ° C e (III) < 0.005 when [ H N O 3 ] < 6 N 3
a
Experimental
Apparatus. T h e f o l l o w i n g apparatus was u t i l i z e d for this s t u d y : a P R T 2000 t y p e potentiostat ( T a c u s s e l ) for the electrolysis; a G r a p h i s p e c t r a l spectrophotometer ( J o u a n ) for the a b s o r p t i o n measurements; a T S 6 t y p e m i l l i v o l t m e t e r ( T a c u s s e l ) for p o t e n t i o m e t r i c analysis; a 2?r w i n d o w l e s s flow gas counter ( S . A . I . P . ) for m e a s u r i n g the soft b e t a f r o m B k ; a n d a b e l l t y p e G e i g e r counter for C e and C e beta counting. 2 4 9
1 4 1
1 4 4
Reagents. B E R K E L I U M . A n a m o u n t of 5μ C i of b e r k e l i u m 249 was s u p p l i e d b y E u r a t o m . Its p u r i t y was c h e c k e d b y a l p h a a n d b e t a c o u n t i n g a n d b y a l p h a a n d g a m m a s p e c t r o g r a p h y . T h e y i e l d of soft b e t a was greater t h a n 9 8 % . T h e s a m p l e was d i s s o l v e d i n 6 N n i t r i c a c i d , a n d the c o n v e r s i o n to s u l f u r i c a c i d m e d i u m was m a d e b y f u m i n g d o w n one a l i q u o t three times a n d d i s s o l v i n g the r e s i d u e i n the a p p r o p r i a t e s o l u t i o n . C E R I U M . C e r i u m 141 a n d 144 isotopes w e r e s u p p l i e d b y the " D é p a r t e m e n t des Radioéléments" of Saclay. C e r o u s n i t r a t e solutions w e r e p r e p a r e d b y d i s s o l v i n g the reagent ( P r o l a b o N o . 2 2 5 8 5 ) . C e r i c n i t r a t e was o b t a i n e d b y e l e c t r o l y t i c o x i d a t i o n of the p r e v i o u s s o l u t i o n i n a c e l l w i t h s e p a r a t e d c o m p a r t m e n t s . C e r i c sulfate a n d f e r r o a m m o n i u m sulfate solutions w e r e p r e p a r e d f r o m the g u a r a n t e e d reagent ( M e r c k N o . 2274 a n d N o . 3793). C e r o u s sulfate w a s o b t a i n e d s i m i l a r l y b y e l e c t r o l y t i c r e d u c t i o n . T R I L A U R Y L M E T H Y L A M M O N I U M SALTS. A s o l u t i o n of 0.1 M t r i l a u r y l m e t h y l a m m o n i u m c h l o r i d e i n c a r b o n t e t r a c h l o r i d e was p r e p a r e d for e a c h e x p e r i m e n t b y d i s s o l v i n g the reagent ( R h ô n e - P o u l e n c ) . T r i l a u r y l m e t h y l a m m o n i u m n i t r a t e a n d sulfate solutions w e r e o b t a i n e d b y m i x i n g f o u r times the p r e v i o u s o r g a n i c s o l u t i o n ( 3 v / v ) r e s p e c t i v e l y w i t h 4 N H N O 3 a n d 1 M N a S 0 . I n a d d i t i o n , the solvents w e r e p r e - e q u i l i b r a t e d b y m i x i n g t h e m t w i c e ( 3 v / v ) w i t h the c o r r e s p o n d i n g a c i d solutions. T R I B U T Y L P H O S P H A T E . T h e reagent t r i b u t y l p h o s p h a t e ( E a s t m a n K o d a k ) w a s p u r i f i e d b y s c r u b b i n g w i t h s o d i u m carbonate s o l u t i o n ( 5 % v / v ) a n d t h e n w i t h d i s t i l l e d w a t e r a n d b y d i s t i l l a t i o n in vacuo. 2
4
Fields and Moeller; Lanthanide/Actinide Chemistry Advances in Chemistry; American Chemical Society: Washington, DC, 1967.
302
L A N T H A N I D E / A C T I N I D E
M I S C E L L A N E O U S . T h e c a r b o n t e t r a c h l o r i d e a n d acids u s e d w e r e r e agents of g r a d e R P ( P r o l a b o ) . ( C C 1 N o . 22521, H N O N o . 20420, H S 0 N o . 20700). Procedure. A q u e o u s phases w e r e p r e p a r e d f r o m samples of cerium ( I V ) , cerium (III), berkelium, and acid and diluted by distilled w a t e r to the p r o p e r concentrations. S a m p l e s of c e r i u m w e r e c h o s e n i n o r d e r to o b t a i n different c e r i u m ( I V ) / c e r i u m ( I I I ) ratios. T h e solutions w e r e a l l o w e d to s t a n d for six hours to r e a c h the o x i d a t i o n e q u i l i b r i u m . A 2 cc. s a m p l e of the solvent was a d d e d to the same v o l u m e of aqueous s o l u t i o n a n d m i x e d for 15 m i n u t e s . A f t e r s e p a r a t i o n b y a c e n t r i f u g e , samples of b o t h phases w e r e t a k e n for the b e t a c o u n t i n g of b e r k e l i u m a n d the s p e c t r o p h o t o m e t r i c d e t e r m i n a t i o n of c e r i u m ( I V ) . I n a d d i t i o n , one a l i q u o t of the l o a d e d solvent was t a k e n for d e t e r m i n i n g the d i s t r i b u t i o n coefficient of b e r k e l i u m ( I V ) . 4
2
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C H E M I S T R Y
a
4
Results D a t a obtained with 0.1M and 0.05M tri-
Sulfuric A c i d Solutions.
l a u r y l m e t h y l a m m o n i u m s u l f a t e - c a r b o n t e t r a c h l o r i d e for d e t e r m i n i n g the f o r m a l o x i d a t i o n p o t e n t i a l of the B k ( I V ) - B k ( I I I ) c o u p l e i n I N a n d 0 . 5 N H S0 2
4
is s u m m a r i z e d i n T a b l e I I I ; the c o r r e s p o n d i n g curves
i 0 g l
[Bk(IV)]. [Bk(III)]
°
hS
-
a
l 0 g ,
°
of:
[Ce(IV)]. [Ce(III)L
are p l o t t e d i n F i g u r e s 5 a n d 6. T h e slopes are 0.92, c a l c u l a t e d b y the least squares m e t h o d ( F i g u r e 5 ) a n d close to 1 ( F i g u r e 6 ) , g r a p h i c a l l y e s t i m a t e d , for I N a n d 0 . 5 N H S 0 , r e s p e c t i v e l y . 2
4
F r o m these d a t a i t appears that i n s u l f u r i c a c i d the f o r m a l o x i d a t i o n potentials
of
the
Ce(IV)-Ce(III) H S0 2
4
Bk(IV)-Bk(III)
couple
differ
from
those
of
the
c o u p l e b y 0.022 a n d 0.017 volts, r e s p e c t i v e l y i n I N
and 0.5N H S 0 2
4
m e d i a . A s s u m i n g the p u b l i s h e d values of
1.44
a n d 1.46 volts for the f o r m a l o x i d a t i o n potentials of the C e ( I V ) - C e ( I I I ) couple i n I N and 0.5N H S 0 2
4
respectively (3, 6 ) , we obtain
£/
B k
=
1.42 volts i n I N H S 0
£/
B k
=
1.44 volts i n 0 . 5 N H S 0
2
2
4
4
N i t r i c A c i d Solutions. T h e d a t a o b t a i n e d w i t h 0 . 1 8 M t r i b u t y l p h o s p h a t e - c a r b o n t e t r a c h l o r i d e are s u m m a r i z e d i n T a b l e I V . It is a p p a r e n t that i n 6 N H N 0
3
F/
B k
-
Efce =
- 0 . 0 2 3 volts
I n this case the slope of the s t r a i g h t l i n e r e p r e s e n t i n g [Bk(IV)]
e
,
[Ce(IV)]
t t
is e s t i m a t e d to b e 1.1 ( F i g u r e 7 ) .
Fields and Moeller; Lanthanide/Actinide Chemistry Advances in Chemistry; American Chemical Society: Washington, DC, 1967.
21.
MusiKAs
A N D
Oxidation
B E R G E R
B y accepting
1.58
303
Potential
volts as the f o r m a l o x i d a t i o n p o t e n t i a l of
the
Ce(IV)-Ce(III) couple (6) we obtain: E/
B k
== 1.56 volts i n 6 N
HN0
3
O n the other h a n d v e r y l i t t l e b e r k e l i u m is extracted b y t r i b u t y l p h o s p h a t e f r o m I N to 2 N H N 0
3
as s h o w n i n T a b l e I V . T h e d e t e r m i n a t i o n of the
f o r m a l o x i d a t i o n p o t e n t i a l of the B k ( I V ) - B k ( I I I ) c o u p l e i n this m e d i u m Downloaded by UNIV OF CALIFORNIA SAN DIEGO on March 18, 2016 | http://pubs.acs.org Publication Date: June 1, 1967 | doi: 10.1021/ba-1967-0071.ch021
is n o t r e l i a b l e . A s s u m i n g that a l l the b e r k e l i u m e x t r a c t e d is tetravalent a n d t h a t the d i s t r i b u t i o n coefficient of b e r k e l i u m ( I V ) is the same as that of c e r i u m ( I V ) , c a l c u l a t i o n shows that the difference b e t w e e n the f o r m a l o x i d a t i o n p o t e n t i a l of the t w o couples s h o u l d be greater t h a n + 0 . 0 8 volts. Table III. Trilaurylmethylammonium Sulfate—Carbon Tetrachloride Extraction of Cerium and Berkelium from Sulfuric A c i d Solutions Aqueous: I N H SO^ Solvent: 0.1 M TLMA
Aqueous: 0 . 5 N H SO^ Solvent: 0.05M TLMA
2
iCe(IVn
a
E° a
[Ce(Iim
Bk(IV)
a
2
Sulfate-CCl^
lCe(IVn
a
1.35 1.41 1.32 1.22 1.40 1.28 1.47 1.28 1.36 1.25 1.50 1.18 1.23 1.43
Bk(IV)
a
a
a
0.022 0.052 0.040 0.065 0.13 0.11 0.12 0.17 0.19 0.24 0.34 0.44 0.65 0.85
E°
iCe(III)}
[Bk(IIin
It
[Bk(IV)]
a
iBk(Iim
a
4.9 5.1 5.3 6.4 6.1 5.5
0.0087 0.014 0.036 0.08 0.085 0.1
0.035 0.08 0.15 0.21 0.24 0.31 0.44 0.48 0.6 0.75 0.65 0.85 1.10 1.35
Sulfate-CCl
0.02 0.038 0.065 0.13 0.15 0.17
E ° B k ( I I I ) < 0.005 i n a l l cases. a
Discussion I n I N to 2 N n i t r i c solutions, b e r k e l i u m was n o t extracted either i n T L M A nitrate or T B P , whereas c e r i u m was extracted. berkelium ( I V )
a l r e a d y extracted f r o m 6 N H N 0
3
F u r t h e r m o r e , the
i n t o T B P was
com-
p l e t e l y b a c k - e x t r a c t e d b y I N H N 0 , w h i l e c e r i u m was not s t r i p p e d as 3
m u c h . A s i m i l a r e x p e r i m e n t m a d e after a d d i n g s o d i u m b i s m u t h a t e p r o v e d t h a t aqueous c e r i u m was e n t i r e l y at the f o u r v a l e n c e state, w h i l e b e r k e l i u m s h o w e d a l o w d i s t r i b u t i o n coefficient s p o n d i n g m a i n l y to the t r i v a l e n t state.
( s m a l l e r t h a n 0.01)
corre-
T h i s result was c o n f i r m e d b y a
Fields and Moeller; Lanthanide/Actinide Chemistry Advances in Chemistry; American Chemical Society: Washington, DC, 1967.
304
LANTHANIDE
ACTINIDE
CHEMISTRY
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iBMlVJa |Bk
tracer e x p e r i m e n t , c a r r i e d o u t w i t h extracted from I N H N 0
3
2 4 i )
Bk and
into T L M A
1 4 4
C e isotopes. C e r i u m w a s
i n the presence of s o d i u m
bis-
m u t h a t e whereas b e r k e l i u m w a s not. T h e last t h r e e experiments
seem to c o n f i r m that t h e difference
in
b e h a v i o r b e t w e e n b e r k e l i u m a n d c e r i u m i n I N to 2 N n i t r i c a c i d solutions does n o t result f r o m a difference i n the r e a c t i o n rate. I t is m o r e p r o b a b l y c a u s e d b y the h i g h e r f o r m a l o x i d a t i o n p o t e n t i a l of t h e B k ( I V ) - B k ( I I I ) c o u p l e . A t s u c h a h i g h f o r m a l o x i d a t i o n p o t e n t i a l tetravalent b e r k e l i u m s h o u l d b e less stable t h a n tetravalent c e r i u m , even i f the difference
is
s m a l l e r t h a n the e s t i m a t e d v a l u e ( + 0 . 0 8 v o l t s ) . T h e s e results suggest that t h e s t a n d a r d potentials of the C e ( I V ) — C e ( I I I ) a n d the B k ( I V ) - B k ( I I I )
couples s h o u l d b e rather
Fields and Moeller; Lanthanide/Actinide Chemistry Advances in Chemistry; American Chemical Society: Washington, DC, 1967.
different.
21.
MUSiKAS
A N D
Oxidation
B E R G E R
305
Potential
Bk(IV)|a
Bk(lll)U
Downloaded by UNIV OF CALIFORNIA SAN DIEGO on March 18, 2016 | http://pubs.acs.org Publication Date: June 1, 1967 | doi: 10.1021/ba-1967-0071.ch021
h
/ /
+
•
/
/
/
10
/ >
/+ / /
+
/
/
/ /
/
+/
Sic pe 1
/
/ / /
10'
/
/
> •*
/
/
/
/
/ / /
/
10"'
/
/
/
/
10"
10"
10"
1
jCe(lV)ja ICe(ll|)|a
Figure 6.
Formal potential of the Bk(IV)-Bk(III)
couple in 0.5N
H SO, 2
t
T h e f a c t that i n c o m p l e x i n g m e d i u m the t w o couples h a v e close values c o u l d i m p l y t h a t the B k ( I V ) complexes
are m o r e t i g h t l y b o u n d t h a n
those of the C e ( I V ) . A l t h o u g h b e r k e l i u m ( I V ) was o b t a i n e d i n c o n c e n t r a t e d n i t r i c a c i d (4, 6),
it was n o t extracted i n T L M A n i t r a t e C C 1 whereas 4
w a s extracted. concentration lium (IV)
cerium(IV)
W h e n d e c r e a s i n g the a c i d i t y for the same n i t r a t e i o n [e.g., i n I N H N 0
was e x t r a c t e d
3
+
(Table II).
1.5M A 1 ( N 0 ) 3 solution], berke3
This phenomenum
c o u l d be
at-
t r i b u t e d to the c o m p e t i t i o n b e t w e e n the n i t r i c a c i d a n d the t e t r a v a l e n t b e r k e l i u m species w h i c h c o u l d b e extracted.
Fields and Moeller; Lanthanide/Actinide Chemistry Advances in Chemistry; American Chemical Society: Washington, DC, 1967.
306
LANTHANIDE/ACTINIDE CHEMISTRY
|Bk (iV)fa I B K (iu)|i
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•
Figure 7.
Formal potential of the Bk(IV)-Bk(III)
couple in 6N
HN0
3
T h e a c c u r a c y of the m e t h o d was c h e c k e d f r o m the d a t a p l o t t e d i n F i g u r e 5. C a l c u l a t i o n gives a m e a n v a l u e for F/
-
R k
F/ce =
0.023 volts
w i t h a s t a n d a r d d e v i a t i o n of: σ
== ± 0 . 0 0 9 volts
T h e scattering of the results d e p e n d s u p o n the soft b e t a c o u n t i n g of B k w h i c h is sensitive to the self a b s o r p t i o n of the source; the spectro p h o t o m e t r i c d e t e r m i n a t i o n of u n s t a b l e c e r i u m ( I V ) ; a n d the great n u m b e r of e x p e r i m e n t a l d e t e r m i n a t i o n s n e e d e d for c a l c u l a t i n g the p o t e n t i a l . 2 4 9
Fields and Moeller; Lanthanide/Actinide Chemistry Advances in Chemistry; American Chemical Society: Washington, DC, 1967.
21.
MUsiKAs
A N D
Oxidation
B E R G E R
307
Potential
Table IV. 0.18M T r i b u t y l Phosphate—Carbon Tetrachloride Extraction of Cerium and Berkelium from N i t r i c A c i d Solutions E° Ce(IV)
[CeflV;]. [Ce(lII))
0.2 0.2
2.7
—
—
a
Aqueous" IN H N 0 + C e ( I V ) I N H N 0 + Ce(IV) + C e (III) I N H N 0 + 1.5M A l ( N 0 ) + Ce(IV) + NaBi0 2 N H N 0 + Ce(IV) + NaBi0 2 N H N 0 + Ce(IV) + Ce (III) 6N H N 0 + Ce(IV) + Ce (III) - d ° - d ° - d ° 3
Downloaded by UNIV OF CALIFORNIA SAN DIEGO on March 18, 2016 | http://pubs.acs.org Publication Date: June 1, 1967 | doi: 10.1021/ba-1967-0071.ch021
3
3
3
a
InltidBk Extracted
E° Bk(IV) a
1 1
JBk(lV)] [Bk(III)]
a
a
0.05
a
0.02
a
70
3
3
3
1.9
2.5
3
a
3
1.9
0.55
3
8.9
0.034
1.3
8.4 8.1 8.4
0.065 0.4 0.465
1.2 1.25 1.05
e
0.055 0.16 1.0 1.6
E s t i m a t e d values assuming that only B k ( I V ) is extracted a n d that E ° B k ( I V ) = a
Ce(IV).
T o t a l c e r i u m i n i t i a l aqueous concentration = a l l cases. I n 6N H N O s E ° B k ( I I I ) < 0.005. b
c
3
6.0 X 1 0 " M . 3
E ° Ce (III) < a
E ° a
0.01 i n
a
Acknowledgments T h e authors w i s h to t h a n k A . Chesné for the h e l p f u l discussions a n d M . M a r t e a u for e x p e r i m e n t a l assistance. J . K o o i is g r a t e f u l l y a c k n o w l e d g e d for s u p p l y i n g b e r k e l i u m - 2 4 9 , thus e n c o u r a g i n g this w o r k .
Literature Cited (1) Haissinsky, M., Pluchet, E., J. Chim. Phys. 76, 608 (1962). (2) Jones, M. E., Cunningham, B. B., U. S. At. Energy Comm. AECD-2913 (1950). (3) Kunz, A. H., J. Am. Chem. Soc. 53, 98 (1931). (4) Matsuura, N., Haissinsky, M., J. Chim. Phys. 55, 475 (1958). (5) Peppard, D. F., Moline, S. W., Mason, G. W., J. Inorg. Nucl. Chem. 4, 344 (1957). (6) Smith, G. F., Getz, C. Α., Ind. Eng. Chem. Anal. 10, 191 (1938). (7) Thompson, S. G., Cunningham, Β. B., Seaborg, G. T., J. Am. Chem. Soc. 72, 2798 (1950). RECEIVED December 27,
1966.
Fields and Moeller; Lanthanide/Actinide Chemistry Advances in Chemistry; American Chemical Society: Washington, DC, 1967.