EXTRACTION OF COBALT (II) IONS FROM AQUEOUS MEDIUM INTO CHLOROFORM SOLUTION OF 4-PROPIONYL-2, 4-DIHYDRO-5-METHYL-2-PHENYL-3H-PYRAZOL-3-ONE (HPRP): EFFECTS OF PH, ACIDS AND COMPLEXING AGENT

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ABSTRACT

The extraction of Cobalt (II) ions from various buffered aqueous solutions was studied using chloroform solutions of 4-Propionyl-2, 4-dihydro-5-methyl-2-phenyl-3H-pyrazol-3-one (HPrP) Schiff base. The complexing agent and concentration effect of 4-propionyl-2, 4-dihydro5-methyl-2-phenyl-3H-pyrazol-3-one (HPrP) in these extractions were also studied and optimized. The effects of certain mineral acids were examined alongside metal ions under a suitable extraction condition.  From the mineral acids studied, cobalt didn’t form non extractable complex. Increase in pH above 10.0 resulted to a decrease in cobalt extraction. Increase in the concentration of various acids above 2.0 pushed the percentage extraction to zero (0).





TABLE OF CONTENTS

                                                                                                                   Page

Cover page                                                                                                 i

Title page                                                                                                    ii

Declaration                                                                                                           iii

Certification                                                                                                iv

Dedication                                                                                                  v

Acknowledgments                                                                                                vi

Table of contents                                                                                        vii

List of Tables                                                                                              ix

List of Figures                                                                                            x

Abstracts                                                                                                    xi

 

 

CHAPTER 1: Introduction                                                                      1

1.1 Statement of Problems                                                                         5       

1.2 Objectives of the Study                                                                        6

1.3 Justification of the Study                                                                      6

1.4 Scope of the Study                                                                               7

 

CHAPTER 2: Literature Review                                                              8

2.1.1 Sources of Cobalt                                                                                     8

2.1.2 Compounds of Cobalt                                                                       9

2.2 Origins and use of  Heavy Metals                                                               9

2.3 Factors Affecting Liquid-Liquid Extraction of Metal Ions                    10

2.4 Buffer                                                                                                   14

2.4.1 Types of buffer solution                                                                          15

2.4.2 Mechanism of buffering action                                                          16

2.4.3 Preparation of buffer solution                                                           16

2.4.4 Preparation of acid buffer                                                                      18

2.5 Schiff Base                                                                                          19

2.5.1 Synthesis of schiff base                                                                     19

2.5.2 Application of schiff base                                                                  20

                                                                                               

 

CHAPTER 3: Material and Methods                                                       27                                                    

3.1 Materials and Apparatus                                                                        27

3.2. Methods                                                                                                 29

3.2.1   Synthesis of 4-propionyl-2,4-dihydro-5-methyl-2-phenyl-

3h-pyrazol-3-one (HprP)                                                                                      29     

3.2.3  Preparation of stock solutions of ligand.                                          31

3.2.4  Preparation of stock solutions of mineral acids                                31

3.2.5  Preparation of stock solutions of salts and base                               31

3.2.6    Preparation of buffer solutions for calibration of pH meter           32

3.2.7  Preparation of buffer solutions                                                                   33

3.2.8  Preparation of metal stock solutions                                                34

3.2.9  Preparation of stock solutions for anions and complexing agents              34

3.2.10 Extraction of metal ions from aqueous phase at different pH values        34

3.2.11 Extractions with various metal concentrations with ligand             35

3.2.12         Extractions with various ligand concentrations                                35

3.2.13         Extraction in the presence of some mineral acids                             36

3.2.14  Extraction in the presence of some anions                                               36

3.2.15  Extractions with various metal concentrations with ligand only              36

 

 

CHAPTER 4: Result and Discussion                                                       37

 

CHAPTER 5: Conclusion                                                                         43

5.2 Recommendation                                                                                  43

Reference                                                                                                    44

 

 

 

 

 

 

 

LIST OF TABLES

 

Standard for cobalt (II) calibration curve                                                   37

Data for 50mg/L Co (II) in buffered solution into 0.05M HPrP                           38

Data for Effect of H3PO4 in Co (II) Extractions with HPrP                       39

Data for Effect of H2SO4 in Co (II) Extractions with HPrP                       40

Data for effect of NO3- in Co (II) extraction with (HPrP)                                    41

Data for effect of PO42- in Co (II) extraction with (HPrP)                         42

 


 


LIST OF FIGURES

Standard for Cobalt (II) Calibration curve                              37

Effect of pH on extraction of Co (II) ions into 0.05M HPrP in chloroform solution                                                                                                     38

Effect of H3PO4 in Co (II) extraction with (HPrP)                           39

Effect of H2SO4 in Co (II) Extractions with HPrP                           40

Effect of NO3- in Co (II) extraction with (HPrP)                     41

Effects of PO42- in Co (II) extraction with HPrP                    42


 





 CHAPTER 1

INTRODUCTION 

1.1 BACKGROUND OF THE STUDY

Liquid–liquid extraction (LLE), also known as solvent extraction and partitioning, is a method to separate compounds or metal complexes, based on their relative solubility in two different immiscible liquids, usually water (polar) and an organic solvent (non-polar). There is a net transfer of one or more species from one liquid into another liquid phase, generally from aqueous to organic. The transfer is driven by chemical potential, i.e. once the transfer is complete, the overall system of chemical components that make up the solutes and the solvents are in a more stable configuration (lower free energy) (Reyes-Labarta & Grossmann, 2015). The solvent that is enriched in solute(s) is called extract. The feed solution that is depleted in solute(s) is called the raffinate. LLE is a basic technique in chemical laboratories, where it is performed using a variety of apparatus, from separatory funnels to countercurrent distribution equipment called as mixer settlers. This type of process is commonly performed after a chemical reaction as part of the work-up, often including an acidic work-up (Reyes-Labarta et al., 2013).

Solvent extraction is an old, established process and together with distillation constitute the two most important industrial separation procedures. The first commercially-successful liquid-liquid extraction operation was developed for the petroleum industry in 1909 when Edeleanu’s process was employed for the removal of aromatic hydrocarbons from kerosene, using liquid sulfur dioxide as solvent. Since then many other processes have been developed by the petroleum, chemical, metallurgical, nuclear, pharmaceutical and food processing industries (Mackenzie & Murdoch 2012).

From a hydrometallurgical perspective, solvent extraction is exclusively used in separation and purification of uranium and plutonium, zirconium and hafnium, separation of cobalt and nickel, separation and purification of rare earth elements etc., its greatest advantage being its ability to selectively separate out even very similar metals.

One obtains high-purity single metal streams on 'stripping' out the metal value from the 'loaded' organic wherein one can precipitate or deposit the metal value. Stripping is the opposite of extraction: Transfer of mass from organic to aqueous phase (Marcilla et al., 2011)

The term partittioning is commonly used to refer to the underlying chemical and physical processes involved in liquid-liquid extractuion, but on another reading may be fully synonymous with it. The term solvent extraction can also refer to the separation of a substance from a mixture by preferentially dissolving that substance in a suitable solvent. In that case, a soluble compound is separated from an insoluble compound or a complex matrix (Reyes-Labarta, et al., 2012).

Whereas distillation affects a separation by utilizing the differing volatilities of the components of a mixture, liquid-liquid extraction makes use of the different extent to which the components can partition into a second immiscible solvent. This property is frequently characteristic of the chemical type so that entire classes of compounds may be extracted if desired. The petroleum industry takes advantage of this characteristic of the process and has used extraction to separate, for example, aromatic hydrocarbons from paraffin hydrocarbons of the same boiling range using solvents such as liquified sulfur dioxide, furfural and diethylene glycol (Filiz et al., 2014). In general, extraction is applied when the materials to be extracted are heat-sensitive or nonvolatile and when distillation would be inappropriate because components are close-boiling, have poor relative volatilities or form azeotropes (Sanchez et al., 2012).

The simplest extraction operation is single-contact batch extraction in which the initial feed solution is agitated with a suitable solvent, allowed to separate into two phases after which the solvent containing the extracted solute is decanted. This is analagous to the laboratory procedure employing a separating funnel. On an industrial scale, the extraction operation more usually involves more than one extraction stage and is normally carried out on a continuous basis. The equipment may be comprised of either discrete mixers or settlers or some form of column contactor in which the feed and solvent phases flow counter currently by virtue of the density difference between the phases (Lee, 2014)

Although heavy metals are naturally occurring elements that are found throughout the earth’s   crust,   most   environmental   contamination   and   human   exposure   result   from anthropogenic activities  such as mining and smelting operations, industrial production and use,  and  domestic  and  agricultural  use of  metals and  metal-containing compounds   (Sanchez et al., 2003). Environmental   contamination   can   also   occur   through   metal   corrosion,   atmospheric deposition, soil erosion of metal ions and leaching of heavy metals, sediment re-suspension and metal evaporation from water resources to soil and ground water. Natural phenomena such as weathering and volcanic eruptions have also been reported to significantly contribute to heavy metal pollution (Giridhar et al., 2016).

Some solutes such as noble gases can be extracted from one phase to another without the need for a chemical reaction (see absorption). This is the simplest type of solvent extraction. When a solvent is extracted, two immiscible liquids are shaken together (Takeshitaet et al., 2018). The more polar solutes dissolve preferentially in the more polar solvent, and the less polar solutes in the less polar solvent. Some solutes that do not at first sight appear to undergo a reaction during the extraction process do not have distribution ratio that is independent of concentration. A classic example is the extraction of carboxylic acids (HA) into nonpolar media such as benzene. Here, it is often the case that the carboxylic acid will form a dimer in the organic layer so the distribution ratio will change as a function of the acid concentration (measured in either phase). 

Using solvent extraction it is possible to extract uraniumplutoniumthorium and many rare earth elements from acid solutions in a selective way by using the right choice of organic extracting solvent and diluent. One solvent used for this purpose is the organophosphate tributylphosphate (TBP). The PUREX process that is commonly used in nuclear reprocessing uses a mixture of tri-n-butyl phosphate and an inert hydrocarbon (kerosene), the uranium(VI) are extracted from strong nitric acid and are back-extracted (stripped) using weak nitric acid. An organic soluble uranium complex [UO2(TBP)2(NO3)2] is formed, then the organic layer bearing the uranium is brought into contact with a dilute nitric acid solution; the equilibrium is shifted away from the organic soluble uranium complex and towards the free TBP and uranyl nitrate in dilute nitric acid. The plutonium (IV) forms a similar complex to the uranium VI), but it is possible to strip the plutonium in more than one way; a reducing agent that converts the plutonium to the trivalent oxidation state can be added (Alloway, 2016). This oxidation state does not form a stable complex with TBP and nitrate unless the nitrate concentration is very high (circa 10 mol/L nitrate is required in the aqueous phase). Another method is to simply use dilute nitric acid as a stripping agent for the plutonium. This PUREX chemistry is a classic example of a solvation extraction.

Liquid-liquid (or solvent) extraction is a countercurrent separation process for isolating the constituents of a liquid mixture. In its simplest form, this involves the extraction of a solute from a binary solution by bringing it into contact with a second immiscible solvent in which the solute is soluble. In practical terms, however, many solutes may be present in the iCotial solution and die extracting ‘solvent’ may be a mixture of solvents designed to be selective for one or more solutes, depending upon their chemical type (Adamo  et al., 2013). Liquid–liquid extraction is possible in non-aqueous systems: In a system consisting of a molten metal in contact with molten salts, metals can be extracted from one phase to the other. This is related to a mercury electrode where a metal can be reduced, the metal will often then dissolve in the mercury to form an amalgam that modifies its electrochemistry greatly. For example, it is possible for sodium cations to be reduced at a mercury cathode to form sodium amalgam, while at an inert electrode (such as platinum) the sodium cations are not reduced. Instead, water is reduced to hydrogen. A detergent or fine solid can be used to stabilize an emulsion, or third phase (Marcilla et al., 2017).

The use of new Schiff bases in liquid-liquid extraction of metals is one area which has generated lots of interesting and positive research results in the past couple of years.

Pyrazolone is 5-membered heterocycle containing two adjacent Nitrogen atoms. It can be viewed as a derivative of pyrazole possessing an additional carbonyl (C=O) group. Compounds containing this functional group are useful commercially in analgesics and dyes

Pyrazolones are prominent analytical reagents, potent drugs or pharmaceutical agents, inhibitors of emzymes and intermediates in the biosynthesis of Nitrogen oxides. In continuation of our work on the synthesis, characterization of 1-phenyl-3-methyl-4-acylpyrazolone-5 derivatives and their application in the extraction of transition metal ion such as Co(II) we are reporting the use of the Schiff base N,N’-ethylenbis(4-propionyl-2,4-dihydro-5methyl-2-phenyl-3H-pyrazol-3-oneimine) as a potential extractant for Cobalt (II) ions. In studying the solvent extraction of Cobalt (II) ions from aqueous media using N, N’-ethylenbis (4-propionyl-2, 4-dihydro-5-methyl-2-phenyl-3H-pyrazol-3-oneimine) 4-propionyl-2, 4-dihydro-5-methyl-2-phenyl-3H-pyrazol-3-one (HPrP).


1.1 STATEMENT OF PROBLEMS

One of the problems in liquid-liquid metal extract is devising an extraction procedure that would be allowed to perform bulk separation of different metals ions. Distribution coefficient represents the equilibrium constant for this process. If the main goal is to extract a solute from the aqueous phase into the organic phase, the problem relates to the relative volumes of the phases which is another problem in liquid liquid extraction. One major problem is that an aqueous sample contains a complex mixture of organic compounds, all of which are at trace concentrations.


1.2 OBJECTIVES OF THE STUDY

The main objective of this study focus on liquid-liquid extraction of heavy metal ions and complexation of ligands. While the specific objectives are to;

        i.            To determine the effect of the complexing agent

      ii.            To determine the effect of concentration

    iii.            To determine the mineral acids of H3PO4 and H2SO4 on the extraction of Cobalt (II)

    iv.            To determine the effect of Nitrate ion and Phosphate ion on the extraction of Cobalt (II)


1.3 JUSTIFICATION OF THE STUDY

Liquid-liquid extraction should be considered as a desirable route for product recovery and purification along with fractional crystallization and distillation (Feng et al., 2020). The ability to make separations according to chemical type, rather than according to physical properties such as freezing point or vapor pressure, is one of extraction’s major attractions. The liquid–liquid extraction process offers several advantages such as high capacity of the extractant and high selectivity of separation. Liquid–liquid extraction was successfully used for the recovery of 2, 3-butanediol during fermentation (Birajdar et al., 2015). Liquid-liquid extraction can be envisaged to play a central role in the future of the hydrometallurgical exploitation of low-grade ores, the reclamation of scrap metal, the processing of industrial waste products, and the elimination of environmental pollution, specifically the removal of heavy metal ions from muCocipal and industrial wastewater. Energy frequently can be saved in the recovery of valuable products from dilute broth solution since a small quantity of a selective solvent can be used, and recovery from the concentrated extract is then facilitated. Selectivity of potentially attractive solvents can frequently be determined from simple shake-outs over the desired concentration range. From these distribution data, the combinations of amount of solvent and number of theoretical stages can be calculated (Cocola et al., 2020). Today there exist only a few commercial metal ion specific reagents suitable for liquid-liquid extraction.


1.4 SCOPE OF THE STUDY

The study is limited to extraction of inorganic metals from synthesized ligands and the effect of concentration and complexing agent.

 

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