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Mechanism and Rate of Butyl Phosphinate Formation from
Reaction of Phosphinic Acid (Cyanex 272) and Tributyl
Phosphate
K.R. Barnard*
CSIRO Process Science and Engineering / Parker Centre / CSIRO Minerals Down Under National Research
Flagship, PO Box 7229, Karawara, WA 6152, Australia.
and D.W. Shiers
Abstract
An impurity species, butyl bis(2,4,4-trimethylpentyl)phosphinate (‘butyl
phosphinate’), has recently been identified in the Murrin Murrin solvent extraction (SX)
circuits. The present work established that this species is formed via direct reaction
between tributyl phosphate (TBP) and the phosphinic acid extractant found in Cyanex
272 and that the reaction is first order relative to the concentration of each reactant. The
observations are consistent with the reaction progressing via a bimolecular nucleophilic
substitution (SN2) mechanism whereby nucleophilic attack of substrate TBP by the
phosphinic acid anion occurs, resulting in cleavage of the C-O bond and ejection of
dibutyl phosphate anion.
The butyl phosphinate formation rate has been determined under synthetic extract,
strip and aqueous-free conditions, the latter at temperatures between 40 and 75°C. In
the absence of an aqueous phase, the rate coefficient was found to be 0.43 ± 0.02 M-1
* Email address: [email protected] . Phone 61-8-9334 8071. Fax 61-8-9334 8001.
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per annum (95 % confidence interval) at 70°C with an activation energy of 122 kJ/mol.
Based on the present data and historical SX plant operating information, a model to
estimate annual butyl phosphinate generation and its build-up in the Murrin Murrin SX
circuits over the last decade was developed. The estimated accrued level of 31 g/L butyl
phosphinate by June 2009 is comparable to the measured 32-35 g/L.
Keywords: Cyanex 272; bis(2,4,4-trimethylpentyl)phosphinic acid; butyl
phosphinate; butyl bis(2,4,4-trimethylpentyl)phosphinate; tributyl phosphate; TBP;
Murrin Murrin.
1. Introduction
Cyanex 272 is a commercial solvent extraction (SX) reagent used to separate cobalt
from nickel in sulphate media (Flett, 2004). The active component is bis(2,4,4-
trimethylpentyl)phosphinic acid (‘phosphinic acid’), which is present at about 85 % in
Cyanex 272, with tris(2,4,4-trimethylpentyl)phosphine oxide (‘phosphine oxide’) being
the major impurity. This phosphinic acid is also present as the active component in the
alternative SX reagents Ionquest 290 and LIX 272.
The first known product arising from chemical degradation of Cyanex 272 has
recently been reported (Barnard, 2010). The species is the butyl ester of phosphinic
acid, namely butyl bis(2,4,4-trimethylpentyl)phosphinate (‘butyl phosphinate’, Figure
1). It was identified in organic samples from the zinc and cobalt SX circuits in Minara
Resources’ Western Australia-based Murrin Murrin (Murrin) nickel laterite operation.
The organic in these two circuits is essentially equivalent and can be interchanged. The
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degradation product was assigned as butyl phosphinate after both its isolation and
spectroscopic characterisation from the Murrin organic, and its synthesis from the parent
phosphinic acid via a chloride intermediate.
This recently-identified species had been observed to be growing in the Murrin SX
circuits over the prior 10 years. This is undesirable from a commercial operating
perspective as besides indicating a loss of valuable extractant it could potentially have
adverse effects on the process such as increased acid (and thus aqueous) entrainment in
the organic phase.
The Murrin zinc and cobalt SX circuits in which this species formed both used a
combination of Cyanex 272 and tributyl phosphate (TBP) in Shellsol 2046 diluent. As
butyl phosphinate was not observed in several commercial Cyanex 272-containing
systems where TBP was absent, it was concluded that the impurity was most likely
formed in the plant organic by reaction (either directly or indirectly) of a component of
Cyanex 272 (phosphinic acid or phosphine oxide impurity) with TBP (Barnard, 2010).
Generation of butyl phosphinate from the phosphine oxide impurity was considered very
unlikely as it would require cleavage of a chemically stable P-C bond and direct
replacement of that with the butoxy group. A more likely path was via reaction of the
phosphinic acid hydroxy group. On this basis, two possible mechanisms were proposed,
namely direct reaction between TBP and phosphinic acid, or a two-step process
involving hydrolysis of TBP liberating a butoxy group which subsequently reacted with
the phosphinic acid.
Hydrolysis is a common degradation pathway for TBP used in the nuclear industry
(Tahraoui and Morris, 1995) and for alkyl phosphates in general (Bel’skii, 1977).
However, the butanol formed is relatively soluble in water (77 g/L), and possesses an
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octanol on water partition coefficient of 7.9 (i.e. log Pow of 0.9, Anon., 2005). Any
butanol generated via hydrolysis of TBP would therefore be lost relatively quickly from
the organic phase by dissolution into the aqueous phase, particularly under extract
conditions. Thus for this mechanism to occur, reaction of butanol with the phosphinic
acid would need to be rapid.
The present work aimed to identify the mechanism by which butyl phosphinate forms
and assess its rate of formation under various conditions and relate this back to the
known butyl phosphinate concentration in the Murrin system and their historical
operating conditions.
2. Experimental
Two major series of experiments were performed, the first primarily under aqueous-
free conditions to determine the mechanism and rate of butyl phosphinate formation, the
second to establish the effect of various aqueous solutions and metal loading levels on
the formation rate.
2.1 Series 1 tests (primarily aqueous-free)
A series of organic solutions containing differing concentrations of phosphinic acid
and trialkyl phosphate (TBP or tris-2-ethylhexylphosphate, TEHP) in Shellsol 2046
were prepared as summarised in Table 1. Cyanex 272, used as the source of phosphinic
acid, was obtained from Murrin which in turn had purchased it from Cytec Industries
Inc. Cyanex 272 was assumed to contain 85 % phosphinic acid (782 g/L or 2.69 M) as
listed on the supplied Material Safety Data Sheet. Pure phosphinic acid used in
experiment 9 was isolated from Cyanex 272 as described previously (Barnard, 2010).
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TBP was sourced from both Aldrich and Murrin and assumed to be 100 % pure. TEHP
and octadecane (added as an internal standard for subsequent gas chromatography
analysis) were purchased from Aldrich. Shellsol 2046 was supplied by Shell Chemical
Co. Quantification of butyl phosphinate was achieved using previously-synthesised
material (Barnard, 2010).
Relevant organic (60 mL) and the one organic/aqueous mixture (experiment 8, 30 mL
each) were placed in hexagonal glass jars (70 mm diameter x 75 mm height), covered
with a thin layer of PTFE/glass composite fabric (Fiberflon® 108.08), then sealed using
twist top lids and Teflon tape. All 70°C solutions were agitated at 200 r.p.m. using an
Innova 4000 incubator shaker maintained at 70 ± 2°C. This temperature, slightly above
that used routinely at Murrin (60°C), was employed to accelerate and thus more readily
monitor progression of the reaction. Experiments at other temperatures were performed
in duplicate in polyethylene glycol baths maintained at the appropriate temperature
(± 2°C) using IKA RCT Basic heater/stirrers with IKA ETS-D4 temperature controllers.
None of the non-70°C systems were agitated. Samples were taken intermittently
throughout the trial and stored at 4°C prior to gas chromatography (GC) analysis.
2.2 Series 2 tests (primarily aqueous-containing)
A second series of tests (Table 2) were undertaken primarily to assess the effect of
metal-free and metal-containing extract and strip aqueous solutions and the effect of
loaded metals (Co, Zn) on the rate of butyl phosphinate formation. The organic and
aqueous solutions used are listed in Table 2. Organic solutions contained 30 % v/v
Cyanex 272 (0.81 M phosphinic acid) and either 10 % v/v TBP (0.36 M) or 20 % v/v
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butanol (Aldrich, 2.18 M). Aqueous solutions were prepared using AR grade sulfuric
acid, technical grade metal sulphate salts and de-ionised water.
In systems with no metal extraction (experiments 24-39), relevant organic (60 mL)
and organic/aqueous mixtures (A:O 40 mL:40 mL) were prepared, mixed using the
Innova shaker maintained at 70 ± 2°C, sampled intermittently and stored for subsequent
GC analysis. For systems where metal extraction occurred (experiments 40-47), the
organic and aqueous solutions (40 mL each) were initially mixed at pH 5.0 to allow
metal loading to occur. Samples of the loaded organic solutions taken throughout the
trial were stripped (A:O 3:1, 100 g/L sulfuric acid, 50°C) before storage.
The initial and final day loaded organic samples (experiments 40-47) were separated
from the corresponding aqueous phase via filtering through Whatman 1PS filter paper
before being stripped (A:O 3:1, 100 g/L sulfuric acid, 50°C, 20 minutes). The resulting
aqueous strip solution was filtered through a 0.45 µm Supor membrane filter then
assayed by inductively coupled plasma-optical emission spectroscopy (ICP-OES) for
metal ion content.
2.3 Gas chromatography
GC analyses were performed using a Varian 3800 gas chromatograph equipped with
a flame ionisation detector (FID). The chromatograph was fitted with an SGE forte BP-
1 fused silica capillary column (30 m x 0.32 mm i.d., 0.5 µm film thickness). Helium
(1.5 ml/min) was used as the carrier gas. The injection and detector ports were held at
250°C and 270°C, respectively. After sample injection at 150°C where it was held for
one minute, the oven temperature was increased to 330°C at 30°C/min. A split ratio of
50 and 1.0 µL injection volume was used.
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Gas chromatography-mass spectrometry (GC-MS) analyses were performed using a
Saturn 2000 mass spectrometer (MS) as the detector. Acetonitrile-based chemical
ionisation (CI) and electon impact (EI) ionisation were used. Helium (1.0 ml/min) was
used as the carrier gas. The transfer line and trap temperatures were 170 and 150°C,
respectively. An AT-5MS column (Alltech, 30 m x 0.25 mm i.d., 0.25 µm film
thickness) was used. After sample injection at 100°C (injection port 270°C), the oven
temperature was increased to 340°C at 15°C/min.
To enable the ready elution of the phosphinic acid extractant, samples (100 µL) were
derivatised by dissolution in 1:1 dimethyl formamide:toluene (600 µL), adding N,O-
bis[trimethylsilyl]acetamide (BSA, 400 µL) and heating (80°C) for 0.5 hours.
Derivatisation was not required for butyl phosphinate detection.
3. Results and Discussion
3.1 Series 1 experiments: Butyl phosphinate generation at 70°C under aqueous-free
conditions
Prior to the commencement of this work, a scoping study undertaken to assess
whether butanol or TBP reacted with Cyanex 272 to generate butyl phosphinate
indicated it was the latter. Given this outcome which was subsequently confirmed-see
Section 3.2, the initial work focussed on Cyanex 272/TBP systems.
3.1.1 Effect of reagent concentration and mechanism of formation
GC traces highlighting the generation of butyl phosphinate in a 20-5-70C system (see
Table 1 for code description) with time are shown in Figure 2. The quantity of butyl
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phosphinate (expressed as g/L) formed throughout the trial in the different systems at
70°C (experiments 1-12) is summarised in Table 3. For all tests, a linear increase in
butyl phosphinate concentration with time was observed (Figure 3). For each
experiment, the rate of butyl phosphinate formation was determined by a line of best fit
passing through the origin. The resulting annualised values (expressed as both g/L and
mM) are summarised in Table 3.
Increasing the concentration of Cyanex 272 (phosphinic acid) from 2–20 % v/v
(0.054–0.54 M) whilst keeping the TBP concentration constant at 5.0 % v/v (0.18 M,
experiments 1-9) was found to result in a proportional increase in the rate of butyl
phosphinate generation (Figure 4). Although discussed further in Sections 3.1.2, 3.1.3
and 3.1.4, the results for experiments 4-9 (all 20-5-70C experiments but under slightly
different conditions) were found to give comparable results and thus are treated as
equivalent in the present analysis. Importantly, experiment 9 shows butyl phosphinate
formation is attributable to the presence of phosphinic acid in Cyanex 272 and not the
phosphine oxide or any other impurity (Section 3.1.2).
Increasing the concentration of TBP from 1-10 % v/v (0.036 – 0.36 M) whilst
keeping the Cyanex 272 concentration constant at 20 % v/v (0.54 M phosphinic acid,
experiments 4-12) was found to result in a proportional increase in the rate of butyl
phosphinate generation (Figure 4).
These results indicate that the rate of butyl phosphinate formation primarily under
aqueous-free conditions is dependent on the concentrations of both phosphinic acid and
TBP. This relationship can be expressed as a standard rate expression;
Butyl phosphinate formation rate = k [Phosphinic Acid ]x[TBP]y (1)
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Where k is equal to a rate coefficient that is responsive to the temperature of the
reaction.
The linear response of butyl phosphinate generation to changes in both phosphinic
acid and TBP concentrations (Figure 4) indicate that the ‘x’ and ‘y’ coefficients in
equation 1 are both equal to one. This rate expression therefore simplifies to a second
order reaction:
Rate = k [Phosphinic Acid ] [TBP] (2)
Insertion of the relevant reagent concentrations and butyl phosphinate formation rate
into equation 2 allows the k value in each of the different experiments to be calculated.
The results for experiments 1-12, which are presented in Table 3, indicate an average k
value of 0.43 M-1 per annum at 70°C with a 95 % confidence interval of 0.02 M-1 per
annum.
The fact that the reaction occurs in the absence of an aqueous phase indicates that
degradation has the potential to occur throughout all stages of a process, i.e. mixing,
settling, storage. This reaction and its possible relevance to other SX systems
containing an acidic extractant and TBP is of interest.
3.1.2 Effect of pure phosphinic acid
In addition to phosphinic acid, Cyanex 272 contains impurities such as phosphine
oxide. In order to establish whether phosphinic acid or the phosphine oxide (or any
other impurity species) was reacting with TBP, a sample of pure phosphinic acid was
isolated as described previously (Barnard, 2010). Reaction of this pure phosphinic acid
with TBP under the 20-5-70C conditions (experiment 9) yielded the expected butyl
phosphinate product at a rate consistent with the other 20-5-70C experiments using ‘as
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supplied’ Cyanex 272. This result confirms phosphinic acid as the reactive species in
Cyanex 272 and that the presence of phosphine oxide impurity has no material effect on
the rate of reaction.
3.1.3 Effect of the presence of an aqueous acid solution
The rate of butyl phosphinate formation in the 20-5-70C system when in the presence
of a 100 g/L sulfuric acid aqueous phase was found to be 13.3 g/L per annum. This
result falls within the average rate of formation of 14.6 ± 1.5 g/L per annum (95 %
confidence interval) calculated for the five anhydrous 20-5-70C experiments. Based on
this single result there would seem to be no evidence to suggest that the presence of
such an aqueous phase affects the rate of butyl phosphinate formation. However,
additional results from subsequent experiments under both extract and strip conditions,
presented in Section 3.2, suggest otherwise.
3.1.4 Effect of different TBP sources
Of the four 20-5-70C experiments performed using Cyanex 272 under anhydrous
conditions, two were performed using Murrin TBP (experiments 6 and 7) and two were
performed using TBP sourced from Aldrich (experiments 4 and 5). The results
overlapped, confirming TBP and not an impurity specific to the Murrin-supplied reagent
is associated with the reaction.
3.1.5 Effect of a long chained alkyl phosphate
It was possible that phosphinic acid could react with trialkylphosphate species other
than TBP. If so, the reaction of TEHP (instead of TBP) with phosphinic acid might be
expected to result in an analogous 2-ethylhexyl phosphinate species. This reaction
(experiment 13) was undertaken using the same molar amount of TEHP (0.18 M) as was
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used in the TBP-containing 20-5-70C experiments. It resulted in the generation of a
small, phosphorus-containing peak growing with time in the GC trace at a retention time
comparable to or slightly higher than that seen for the butyl phosphinate species. GC-
MS analysis and inspection of the resulting chemical ionisation mass spectrum revealed
prominent ions at m/z 468 and 396, inconsistent with the molecular weight of 2-
ethylhexyl phosphinate (402.5). As hydrolysis of TEHP to di-2-ethylhexyl phosphoric
acid (DEHPA) was possible, a reference sample of DEHPA (molecular weight 322.42)
was derivatised and analysed. The resulting product was found to possess the same
retention time and mass spectrum as the species generated in the present work. The ion
at m/z 468 is assignable to doubly-derivatised DEHPA, whilst the ion at m/z 396
corresponded to the loss of one trimethylsilyl group. The product generated in the
present work is therefore assigned as DEHPA arising from hydrolysis of TEHP. The
inability of TEHP to react with phosphinic acid like TBP does is assumed to be
attributable to its increased steric bulk. This is discussed further in Section 3.3.
3.1.6 Effect of dibutyl phosphate
Hydrolysis of TBP generates butanol and dibutyl phosphate. Although butanol does
not react with phosphinic acid (Section 3.2), another (very unlikely) possibility is
reaction between phosphinic acid and dibutyl phosphate. Two additional anhydrous
experiments were therefore undertaken by combining 20 % v/v Cyanex 272 (0.54 M)
with 7.9 % v/v dibutyl phosphate (0.36 M) and shaking for 12 days at 70°C. No butyl
phosphinate was formed.
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3.1.7 Effect of temperature on the rate of butyl phosphinate generation
The effect of temperature (40-75°C) on the rate of butyl phosphinate formation was
assessed using an organic solution containing 20 % Cyanex 272 (0.54 M) and 5.0 %
TBP (0.18 M, experiments 4-9 and 14-23). The quantity of butyl phosphinate formed
throughout the trial at the different temperatures is summarised in Table 4, along with
the resulting annualised rate of formation (in g/L and mM) and calculated rate
coefficient, k. As expected, increased butyl phosphinate formation was observed as the
operating temperature increased.
The activation energy (Ea) for butyl phosphinate formation under anhydrous
conditions can be determined from the available data by using the Arrhenius equation:
k = A exp(-Ea/RT) (3)
where k is the rate coefficient, R is the gas constant (8.314 J K-1 mol-1), T is
temperature (in Kelvin) and A, the pre-exponential factor, is the rate constant at infinite
temperature. Determination of Ea is most readily achieved by taking the logarithm of
each side of this equation which then becomes
ln(k) = ln (A) – (Ea/RT). (4)
This format is equivalent to a straight line equation y = mx +c, where x is (1/T) and
m (the gradient) equals - Ea/R. The Arrhenius plot based on the available data gave a
very good linear fit (Figure 5). From this plot, Ea was calculated to be 122 kJ/mol and
"A” is 1.57x1018 per annum. This can be used to readily assess the k value at other
operating temperatures under anhydrous conditions.
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3.2 Series 2 experiments: Effect of aqueous solutions and metal loading
The quantity of butyl phosphinate formed throughout the trial in the different systems
at 70°C is summarised in Table 5 along with the resulting annualised values (expressed
as both g/L and mM) and resulting rate coefficient, k.
Butyl phosphinate was not formed in any of the systems containing butanol
(experiments 24-29), confirming this alcohol is not associated with butyl phosphinate
formation.
The rate coefficients derived from the two anhydrous tests (experiments 30, 31) were
found to be comparable with the result of 0.43 ± 0.02 M-1 per annum (95 % confidence
interval) obtained previously under anhydrous conditions (Section 3.1.1), providing
confidence in the ability to compare the two series of results. Relative to the anhydrous
system, the presence of metal-free strip aqueous solution (20 g/L sulfuric acid) saw the
rate coefficient decrease to 0.33-0.35 M-1 per annum (experiments 32, 33), suggesting
dilute aqueous acid or water interferes with the reaction. The same rate coefficient was
obtained for tests done under strip conditions in the presence of 10 g/L each of Co, Ni
and Zn (experiments 34, 35), suggesting the presence of these uncomplexed metals play
no role in butyl phosphinate formation. Combined, these four results were found to
indicate a rate coefficient of 0.34 ± 0.02 M-1 per annum (95 % confidence interval) for
butyl phosphinate formation under strip conditions at 20 g/L sulfuric acid concentration.
In contrast, the single experiment performed previously in the presence of 100 g/L
sulfuric acid solution gave a higher result of 0.39 M-1 per annum (Section 3.1.3),
suggesting increased acidity leads to increased butyl phosphinate formation.
Confirmation of this possible trend would be of interest.
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Tests done under metal-free extract conditions (experiments 36, 37) and under
extract conditions in the presence of 10 g/L Ni (experiments 38, 39) saw comparable
results obtained, with rate coefficients in the range 0.32-0.37 M-1 per annum.
Combined, these four results were found to indicate a rate coefficient of 0.34 ± 0.04 M-1
per annum (95 % confidence interval) for butyl phosphinate formation under these
extract conditions at pH 5.0. This result is equivalent to that observed under strip
conditions using 20 g/L sulfuric acid, suggesting the rate of butyl phosphinate formation
is independent of acidity in that range. This implies the reduced reaction rate seen under
extract and strip conditions relative to the anhydrous system is due to the presence of the
aqueous phase.
The two Murrin SX circuits are used to sequentially extract zinc and cobalt from the
nickel rich, sulfate-based feed solution. Complexation of cobalt with phosphinic acid at
low (0.12 M) and high (0.28 M) concentrations (experiments 40-43) saw the rate of
butyl phosphinate formation increase from the metal-free rate of 0.34 M-1 per annum to
0.37 and 0.46 M-1 per annum, respectively. A plot of these results (Figure 6) suggests a
possible relationship exists between cobalt loading and butyl phosphinate rate
coefficient, although additional data is ideally required to confirm this. The rate
coefficient changing as a function of cobalt loading could be associated with the actual
amount of cobalt loaded, changes in complex structure / stoichiometry, or the ratio of
loaded cobalt to total phosphinic acid present in the organic phase. Further investigation
would also be required to clarify this matter.
Like cobalt, complexation of zinc with phosphinic acid at low (0.15 M)
concentrations (experiments 44, 45) saw no change in the butyl phosphinate rate
coefficient relative to the metal-free aqueous system (0.33 M-1 per annum), but
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increasing loading to 0.30 M (experiments 46, 47) saw a marked increase to 0.85 M-1
per annum.
It should be noted that all of these tests were performed under continual agitation
conditions and therefore are likely to be more representative of the rates expected under
mixing conditions. It is possible that the rate observed under non-mixing conditions
such as those prevailing in the settling stage of a commercial operation differ, with the
rates for stripped or partially loaded organic being more aligned to the results obtained
here under anhydrous conditions. This possibility ideally requires further investigation.
3.3 Mechanism of butyl phosphinate formation
The current results preclude butyl phosphinate formation via reaction of phosphinic
acid with any species arising from TBP hydrolysis. Instead, they demonstrate it is
formed via direct reaction between phosphinic acid and TBP, with the rate of formation
being first order relative to both TBP and phosphinic acid concentration and thus second
order overall.
Hydrolysis of alkyl phosphates proceeds through nucleophilic substitution arising
from attack of the P-O-C linkage by a nucleophile which can occur via two distinct
processes (Bel’skii, 1977 and references therein; Kocieński, 2005). The type 1 process
sees attack occur at the phosphorus atom leading to P-O bond cleavage, whereas the
type 2 processes progress via attack of the carbon substituent, leading to C-O bond
cleavage. Type 1 processes (P-O cleavage) can occur via three mechanisms, namely
addition-elimination, elimination-addition (e.g. hydrolysis of trialkyl phosphates under
basic conditions), and direct substitution. In all cases where such a reaction with a
trialkyl phosphate is successful, the nucleophile ends up being attached to the dialkyl
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phosphate with ejection of an alkoxy group. Type 2 processes (O-C cleavage) can
progress via two mechanisms: a bimolecular nucleophilic substitution (or SN2) reaction,
and a unimolecular nucleophilic substitution (or SN1) reaction. In both cases, the
phosphate acts as the leaving group.
Given a pKa of 5.22 (Zhang et al, 1995), some dissociation of phosphinic acid in the
organic matrix would be expected. The generation of butyl phosphinate even under
anhydrous conditions suggests phosphinic acid or, more likely, its anion can act as a
nucleophile. As such, reaction via any of the Type 1 processes to yield butyl
phosphinate can be discounted as it would instead result in the generation of a molecule
containing a P-O-P linkage. Such P-O-P-containing species could not form from either
of the Type 2 processes where phosphate acts as the leaving group. Instead, the alkyl
group excised from the trialkyl phosphate would end up attached to the attacking
nucleophile, in this case yielding butyl phosphinate. The second order nature of butyl
phosphinate formation as determined here is consistent with this reaction being assigned
as an SN2 reaction involving C-O cleavage (Figure 7).
Increasing the steric bulk of the substrate (alkyl phosphate in this case) results in
inhibition of SN2 reactions. The outcome obtained when TBP was replaced by the more
sterically bulky tris-2-ethylhexylphosphate is consistent with this expectation.
3.4 Implications for the Murrin site
It was previously determined that butyl phosphinate was present in the Murrin plant
organic solutions at 32-35 g/L in mid 2009 (Barnard, 2010). It was of interest to
estimate the annual amount of butyl phosphinate formed and cumulative concentration
present based on the data from the present work. In order to do this, Murrin kindly
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provided access to available relevant operating data over the past several years. The
results were then extrapolated to cover the period for which data was not readily
available. As such these calculations are only approximate.
Based on the present work, the key parameters affecting butyl phosphinate generation
are:
• Phosphinic acid (Cyanex 272) concentration.
• TBP concentration.
• Organic temperature.
• Aqueous strip acidity.
• Metal (Co, Zn) loading levels.
Based on the five years of analysed data, the following was concluded:
1. The average Cyanex 272 and TBP concentrations in the Murrin SX circuits
were about 21 % (0.54 M phosphinic acid) and 11 % (0.41 M), respectively.
2. The average organic temperature was 60°C for all of mixing, settling and
storage stages. The relatively short residence times in the storage tanks
between cycles meant the organic would not materially decrease in
temperature during that time.
3. Average zinc and cobalt loading levels and strip acidity in the relevant stages
and average residence time in the various stages of the Murrin circuit were
assessed. Rates during mixing and settling were assumed to differ as
discussed above. Specific parameters are not disclosed for confidentiality
reasons.
These conclusions were assumed to be valid over the entire life of the Murrin
operation. On the basis of points 2 and 3 above, the average rate coefficient was
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estimated to be 0.12 M-1 per annum and thus the annual rate of butyl phosphinate
formation calculated to be about 27 mM (9.5 g/L) per annum. Based on a 95 m3 organic
inventory, this equates to 2600 mole of butyl phosphinate being generated annually at a
reagent cost of approximately A$77,000 based on A$65/L for Cyanex 272 (965 L
consumed) and A$20/kg for TBP (690 L consumed). At the time of analysis in 2009
(Barnard, 2010), there was approximately A$250,000 of Cyanex 272 and TBP
associated with butyl phosphinate in the Murrin circuits.
Given the known level of butyl phosphinate in the circuit in 2009, it was of interest to
assess whether the calculated annual rate of formation would reasonably allow the
observed circuit concentration to be reached. Such a calculation requires the ongoing
rate of loss of butyl phosphinate from the circuit to also be known.
As the amount of Cyanex 272 added to the circuit per annum to compensate for
ongoing losses was known, it was originally intended to assume the percentage of butyl
phosphinate lost per annum matched that for Cyanex 272. However, two species are
readily detected in Cyanex 272 by GC analysis, namely the phosphinic acid extractant
and the phosphine oxide impurity. Although not reported, quantitative analysis of
Cyanex 272 phosphinic acid and the phosphine oxide impurity was undertaken at the
same time the butyl phosphinate in the Murrin circuit was quantified (Barnard, 2010). It
was noted that whereas the phosphinic acid was present at levels equating to about 20 %
v/v Cyanex 272, the phosphine oxide impurity was present at levels equating to about
28 % v/v Cyanex 272. That is, the more chemically inert nature of the phosphine oxide
impurity appears to slightly decrease its rate of loss from the Murrin circuit organic
relative to the phosphinic acid. (Although beyond the scope of the present analysis, it is
worth noting that any gradual increase of this phosphine oxide species with time could
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eventually have operating consequences in regard to increased acid entrainment, e.g.
Sarangi et al., 2006; Haghshenas et al., 2009). A salient example of this is the inability
of the phosphine oxide to form butyl phosphinate, unlike phosphinic acid. It was
therefore concluded that ongoing loss of butyl phosphinate from the Murrin circuit
would be best assessed relative to that determined for the phosphine oxide impurity in
Cyanex 272.
Based on the known average annual loss of phosphinic acid being about 40 % and the
ratio of phosphine oxide to phosphinic acid in the circuit organic being about 1.4 times
the ratio present in fresh Cyanex 272, it was estimated that phosphine oxide was being
lost from the circuit at about 28 % per annum. Combining the calculated rate of
formation with this estimated percent annual loss (both calculated using a monthly
interval, i.e. 0.79 g/L formed per month and 2.3 % lost per month) commencing from
June 1999 gave rise to an estimated value of 31 g/L butyl phosphinate in June 2009
(Table 6), comparable to the previously measured value of 32-35 g/L (Barnard, 2010).
This result suggests the developed model can reasonably explain the build-up of butyl
phosphinate in the Murrin plant. Unfortunately, no additional (historic) Murrin plant
samples were available for analysis to validate the present model.
This model is sensitive to operating temperature. Increasing the average operating
temperature from 60°C to 62°C increases the rate of formation to 12.4 g/L per annum,
resulting in a calculated accrued butyl phosphinate level of 41 g/L by June 2009.
Conversely, decreasing the operating temperature to 58°C decreases the rate of
formation to 7.3 g/L per annum and calculated accrued level of 24 g/L.
It should be noted that this analysis using the phosphine oxide species as a reference
material was possible due to only Cyanex 272 being added to the circuit over the
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relevant timeframe. Substitution to an alternative reagent with a different phosphine
oxide concentration such as Ionquest 290 (phosphine oxide impurity < 5 % cf. about
15 % in Cyanex 272) during the timeframe examined would have made analysis based
on phosphine oxide concentration problematic.
4. Summary and conclusion
The impurity species butyl bis(2,4,4-trimethylpentyl)phosphinate (‘butyl
phosphinate’) has recently been identified in a commercial SX plant using Cyanex 272
and TBP. The present work has established that this species is formed via direct
reaction between phosphinic acid (the extractant in Cyanex 272) and TBP, with the rate
of formation being first order relative to both TBP and phosphinic acid concentration.
The observations are consistent with nucleophilic attack of TBP by the phosphinic acid
anion resulting in cleavage of the C-O bond and ejection of dibutyl phosphate anion via
a regular SN2 mechanism. Phosphinic acid was not observed to react with the more
sterically bulky phosphate species tris-2-ethylhexyl phosphate, an outcome consistent
with the proposed mechanism.
In the absence of an aqueous phase, the rate coefficient was found to be 0.43 ± 0.02
M-1 per annum (95 % confidence interval) at 70°C with an activation energy of
122 kJ/mol. The reaction occurring in the absence of an aqueous phase indicates that
degradation has the potential to occur throughout all stages of a process, i.e. mixing,
settling, storage. Agitation in the presence of an aqueous solution between pH 5.0 and
20 g/L sulfuric acid reduced the reaction rate relative to the anhydrous system by about
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20 % to 0.34 ± 0.02 M-1 per annum (95 % confidence interval) at 70°C, increasing to
0.39 M-1 per annum with 100 g/L sulfuric acid.
Complexation of 0.28 M cobalt saw an increase in the rate of formation to 0.46 M-1
per annum. Complexation of 0.15 M Zn had no effect on the rate, although increasing
loading to 0.30 M saw the rate increase markedly to 0.86 M-1 per annum. That the rate
coefficient appears to change as a function of metal loading could be associated with the
amount of metal loaded, complex structure / stoichiometry, or the ratio of loaded metal
to total phosphinic acid present in the organic phase. Further investigation would be
required to clarify this matter.
Based on the current results and historical SX plant operating information, the rate of
butyl phosphinate formation at the Murrin plant was calculated to be about 27 mM (9.5
g/L) per annum, equating to 2600 mole generated annually. Along with the estimated
annual rates of loss, this data was used to estimate butyl phosphinate build-up in the
Murrin circuit over the last decade. The estimated value of 31 g/L butyl phosphinate by
June 2009 is comparable to the measured 32-35 g/L.
Acknowledgements
Mr. John O’Callaghan and Dr. Sian Miller of Minara Resources are thanked for
providing information pertaining to the operation of the Murrin Murrin solvent
extraction circuits. The support of the Minerals Down Under National Flagship and
Parker CRC for Integrated Hydrometallurgy Solutions (established and supported under
the Australian Government’s Cooperative Research Centres Program) are gratefully
acknowledged.
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22
References
Anon., 2005. 1-butanol MSDS as found on International Programme of Chemical
Safety, http://www.inchem.org/documents/icsc/icsc/eics0111.htm, accessed 30 Sept.,
2010.
Barnard, K.R., 2010. Identification and characterisation of a Cyanex 272 degradation
product formed in the Murrin Murrin solvent extraction circuit, Hydrometallurgy, 103,
190-195.
Bel’skii, V.E., 1977. Kinetics of the hydrolysis of phosphate esters, Russ. Chem.
Rev., 46, 828-841.
Flett, D.S., 2004. Cobalt-Nickel separation in hydrometallurgy: A review, Chemistry
for Sustainable Development, 12, 81-91.
Haghshenas, D.F., Darvishi, D., Rafieipour, H., Alamdari, E.K., Salardini, A.A.,
2009. A comparison between TEHA and Cyanex 923 on the separation and the
recovery of sulfuric acid from aqueous solutions, Hydrometallurgy, 97, 173-179.
Kocieński, P.J., 2005. “Protecting Groups, 3rd Edition”. Druckhaus Thomas
Muntzer, Bad Langensalza, Germany, 454-457.
Sarangi, K., Padhan, E., Sarma, P.V.R.B., Park, K.H., Das, R.P., 2006.
Removal/recovery of hydrochloric acid using Alamine 336, Aliquat 336, TBP and
Cyanex 923, Hydrometallurgy, 84, 125-129.
Tahraoui, A., Morris, J.H., 1995. Decomposition of solvent-extraction media during
nuclear reprocessing - literature review, Sep. Sci. Technol., 30, 2603-2630.
Zhang, P., Inoue, K., 1995. Recovery of metal values from spent
hydrodesulfurization catalysts by liquid-liquid extraction, Energy and Fuels, 9, 231-239.
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Table 1 Summary of conditions used in the predominantly aqueous-free experiments.
Table 2 Summary of conditions used in the primarily aqueous-containing experiments.
Table 3 Concentration (g/L) of butyl phosphinate observed with time in the 70°C systems
along with annualised rate of formation and calculated rate coefficient.
Table 4 Concentration (g/L) of butyl phosphinate observed with time in the 20 % Cyanex
272 / 5.0 % TBP systems at different temperatures along with the annualised rate of formation
and calculated rate coefficient.
Table 5 Concentration (g/L) of butyl phosphinate observed with time in the various
systems at 70°C along with annualised formation rate and calculated rate coefficient.
Table 6 Estimated butyl phosphinate concentration (g/L) in the Murrin circuit over time.
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24
Table 1 Summary of conditions used in the predominantly aqueous-free experiments.
Expt. Experiment Temp. NotesNo. Code* (M) % (v/v) (M) % (v/v) (°C)1 2-5-70C 0.054 2 0.18 5.0 702 5-5-70C 0.14 5 0.18 5.0 703 10-5-70C 0.27 10 0.18 5.0 70
4, 5 20-5-70C 0.54 20 0.18 5.0 706, 7 20-5-70C 0.54 20 0.18 5.0 70 Murrin TBP used
8 20-5-70C-Acid 0.54 20 0.18 5.0 70 Aqueous present9 20-5-70C-Pure 0.54 20 0.18 5.0 70 Pure phos. acid
10 20-10-70C 0.54 20 0.36 10.0 7011 20-2.5-70C 0.54 20 0.091 2.5 7012 20-1.0-70C 0.54 20 0.036 1.0 7013 20-9-70C-TEHP 0.54 20 0.18 5.0 70 TEHP used
14, 15 20-5-60C 0.54 20 0.18 5.0 6016, 17 20-5-50C 0.54 20 0.18 5.0 5018, 19 20-5-40C 0.54 20 0.18 5.0 4020, 21 20-5-55C 0.54 20 0.18 5.0 5522, 23 20-5-75C 0.54 20 0.18 5.0 75
TBPPhosphinic acid
* Code is Cyanex 272 concentration (% v/v)-TBP concentration (% v/v)-Temperature (°C)-unique identifier, e.g. 'acid' is sample mixed with sulfuric acid, 'pure' used pure phosphinic acid and 'TEHP' used tris-2-ethyl hexyl phosphate instead of TBP. For instance 20-5-70C refers to an experiment using 20 % Cyanex 272, 5 % TBP at 70°C.
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Table 2 Summary of conditions used in the primarily aqueous-containing experiments.
Expt. Organic* Condition Aqueous phase No.
24, 25 B Anhydrous nil26, 27 B Strip 20 g/L H2SO4
28, 29 B Extract pH 5.0, 10 g/L Na2SO4
30, 31 T Anhydrous nil32, 33 T Strip 20 g/L H2SO4
34, 35 T Strip 20 g/L H2SO4 plus 10 g/L each Co, Ni, Zn36, 37 T Extract pH 5.0, 10 g/L Na2SO4
38, 39 T Extract pH 5.0, 10 g/L Na2SO4 plus 10 g/L Ni40, 41 T Extract pH 5.0, 10 g/L Na2SO4 plus 8.8 g/L Co42, 43 T Extract pH 5.0, 10 g/L Na2SO4 plus 17.7 g/L Co44, 45 T Extract pH 5.0, 10 g/L Na2SO4 plus 9.8 g/L Zn46, 47 T Extract pH 5.0, 10 g/L Na2SO4 plus 19.5 g/L Zn
* Contains 30% v/v Cyanex 272 and either 10% v/v TBP (T) or 20% v/v n-butanol (B).
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Table 3 Concentration (g/L) of butyl phosphinate observed with time in the 70°C systems
along with annualised rate of formation and calculated rate coefficient.
Expt. Experiment Rate coeff.No. Code 10 20 34 45 55 67 (g/L p.a) (mM p.a.) (k, M-1 p.a.)1 2-5-70C 0.06 0.10 0.16 0.17 0.21 0.26 1.5 4.2 0.432 5-5-70C 0.11 0.22 0.44 0.50 0.59 0.70 4.0 11.5 0.473 10-5-70C 0.27 0.50 0.87 1.10 1.25 1.46 8.4 24.3 0.504 20-5-70C (a) 0.47 0.87 1.51 2.01 2.15 2.67 15.0 43.4 0.445 20-5-70C (b) 0.36 0.76 1.34 1.71 2.02 2.43 13.6 39.1 0.406 20-5-70C (c) 0.37 0.76 1.43 1.80 2.04 2.38 13.7 39.5 0.407 20-5-70C (d) 0.50 1.00 1.72 2.10 2.50 2.80 16.4 47.3 0.488 20-5-70C-Acid 0.38 0.77 1.34 1.69 1.98 2.35 13.3 38.4 0.399 20-5-70C-Pure 0.58 1.04 1.42 1.73 2.11 2.45 14.1 40.8 0.42
10 20-10-70C 0.78 1.47 2.52 3.28 3.92 5.18 27.2 78.4 0.4011 20-2.5-70C 0.20 0.43 0.76 0.97 1.17 1.40 7.8 22.4 0.4612 20-1.0-70C 0.06 0.15 0.26 0.35 0.41 0.52 2.8 8.1 0.42
Formation rateDay
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Table 4 Concentration (g/L) of butyl phosphinate observed with time in the 20 % Cyanex
272 / 5.0 % TBP systems at different temperatures along with the annualised rate of formation
and calculated rate coefficient.
Expt. Experiment Rate coeff.No. Code 10 20 34 45 55 112 (g/L p.a) (mM p.a.) (k, M-1 p.a.)14 20-5-60C (a) 0.10 0.17 0.36 0.51 0.69 1.36 4.4 12.6 0.1315 20-5-60C (b) 0.07 0.18 0.36 0.50 0.66 1.41 4.4 12.8 0.1316 20-5-50C (a) 0.02 0.05 0.08 0.10 0.13 0.21 0.75 2.2 0.0217 20-5-50C (b) 0.03 0.05 0.09 0.13 0.15 0.23 0.84 2.4 0.0218 20-5-40C (a) 0.02 0.02 0.04 0.04 0.05 0.08 0.29 0.8 0.0119 20-5-40C (b) 0.02 0.03 0.04 0.05 0.05 0.09 0.33 0.9 0.01
7 16 25 31 4920 20-5-55C (a) 0.05 0.11 0.17 0.21 0.23 2.0 5.9 0.0621 20-5-55C (b) 0.08 0.12 0.16 0.20 0.21 2.0 5.7 0.0622 20-5-75C (a) 0.42 1.25 2.16 2.93 32.4 93.7 0.9523 20-5-75C (b) 0.43 1.17 2.15 2.97 32.4 93.6 0.95
Formation rateDay
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Table 5 Concentration (g/L) of butyl phosphinate observed with time in the various
systems at 70°C along with annualised formation rate and calculated rate coefficient.
Expt Rate coeff.No. 7 16 25 31 g/L p.a. mM p.a. k, M-1 p.a.24 0.0 0.0 0.0 0.0 0.0 0.00 0.0025 0.0 0.0 0.0 0.0 0.0 0.00 0.0026 0.0 0.0 0.0 0.0 0.0 0.00 0.0027 0.0 0.0 0.0 0.0 0.0 0.00 0.0028 0.0 0.0 0.0 0.0 0.0 0.00 0.0029 0.0 0.0 0.0 0.0 0.0 0.00 0.0030 0.8 1.9 3.1 3.8 45.2 0.13 0.4431 0.9 2.1 3.2 4.0 47.1 0.14 0.4632 0.7 1.7 2.4 3.1 36.2 0.10 0.3533 0.6 1.5 2.3 2.8 33.3 0.10 0.3334 0.7 1.6 2.4 2.9 34.9 0.10 0.3435 0.7 1.7 2.4 2.9 35.2 0.10 0.3436 0.6 1.4 2.3 2.8 33.3 0.10 0.3337 0.7 1.3 2.3 2.8 32.7 0.09 0.3238 0.7 1.6 2.4 2.9 35.4 0.10 0.3539 0.8 1.7 2.6 3.2 37.8 0.11 0.3740 0.8 1.7 2.6 3.2 38.1 0.11 0.3741 0.8 1.8 2.6 3.2 38.4 0.11 0.3842 0.9 2.2 3.1 4.0 46.7 0.13 0.4643 0.9 2.0 3.2 4.0 47.1 0.14 0.4644 0.7 1.5 2.4 3.0 35.3 0.10 0.3545 0.6 1.4 2.2 2.6 31.0 0.09 0.3046 1.5 3.6 5.7 6.7 81.2 0.23 0.8047 1.9 4.5 6.3 7.7 93.1 0.27 0.91
Formation rateDay
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Table 6 Estimated butyl phosphinate concentration (g/L) in the Murrin circuit over time.
k rate formed(M-1) (g/L p.a.) '00 '01 '02 '03 '04 '05 '06 '07 '08 '090.124 9.5 8 14 19 23 25 27 29 30 31 31
Year
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Figure 1 Structure of butyl bis(2,4,4-trimethylpentyl)phosphinate.
Figure 2 GC traces highlighting the growth of the butyl phosphinate peak at 4.83 min with
time in a 20-5-70C system.
Figure 3 Butyl phosphinate generation observed over time at different phosphinic acid
concentrations (2-20 % v/v Cyanex 272; 0.054-0.54 M). TBP concentration was fixed at 5.0 %
v/v (0.18 M).
Figure 4 Butyl phosphinate generation per annum with changing phosphinic acid
concentration at a fixed TBP concentration of 0.18 M (5.0 % v/v, squares), and changing TBP
concentration at a fixed phosphinic acid concentration (0.54 M, 20 % v/v Cyanex 272,
triangles).
Figure 5 Arrhenius plot describing the relationship between the rate coefficient, k, and
temperature.
Figure 6 Plot of butyl phosphinate rate coefficient versus cobalt loading.
Figure 7 Butyl phosphinate formation via the proposed SN2 reaction mechanism.
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31
P
O
(CH3)3CCH2CH(CH3)CH2
(CH3)3CCH2CH(CH3)CH2
O(CH2)3CH3
Figure 1 Structure of butyl bis(2,4,4-trimethylpentyl)phosphinate.
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3 4 5 Minutes0
10
20
30
40
mVolts
Octadecane4.05 min Butyl phosphinate
4.83 min
Day 45
Day 0
Day 67
Phosphinic acid4.42 min
Phosphine oxide5.55 min
TBP3.48 min
Day 20
Diluent region
Figure 2 GC traces highlighting the growth of the butyl phosphinate peak at 4.83 min with
time in a 20-5-70C system.
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0.0
0.5
1.0
1.5
2.0
2.5
3.0
0 10 20 30 40 50 60 70Time (days)
But
yl p
hosp
hina
te (g
/L) .
2-5-70C5-5-70C10-5-70C20-5-70C (a)20-5-70C (b)20-5-70C (c)20-5-70C (d)20-5-70C-Acid20-5-70C-Pure
Figure 3 Butyl phosphinate generation observed over time at different phosphinic acid
concentrations (2-20 % v/v Cyanex 272; 0.054-0.54 M). TBP concentration was fixed at 5.0 %
v/v (0.18 M).
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34
y = 26.8xR2 = 0.97
y = 77.4xR2 = 0.98
0
3
6
9
12
15
18
21
24
27
30
0.00 0.10 0.20 0.30 0.40 0.50Reagent concentration (M)
But
yl p
hosp
hina
te (g
/L p
.a.)
.
TBPphosphinic acid
Figure 4 Butyl phosphinate generation per annum with changing phosphinic acid
concentration at a fixed TBP concentration of 0.18 M (5.0 % v/v, squares), and changing TBP
concentration at a fixed phosphinic acid concentration (0.54 M, 20 % v/v Cyanex 272,
triangles).
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35
y = -14653x + 41.90
R2 = 0.991
-5.0
-4.0
-3.0
-2.0
-1.0
0.0
0.0028 0.0029 0.0030 0.0031 0.00321/T (K-1)
ln(k
)
Ea = = 122 kJ/molA = 1.57 x 1018 p.a.
Figure 5 Arrhenius plot describing the relationship between the rate coefficient, k, and
temperature.
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36
0.33
0.35
0.37
0.39
0.41
0.43
0.45
0.47
0 0.04 0.08 0.12 0.16 0.2 0.24 0.28Loaded Cobalt (M)
Rat
e co
effic
ient
Figure 6 Plot of butyl phosphinate rate coefficient versus cobalt loading.
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P O-
RR
O
SN2 POC4H9R
R
O-O
O
POBu
OBuOBuOBu
P
O
H
O
H
C3H7
C +
Figure 7 Butyl phosphinate formation via the proposed SN2 reaction mechanism.