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\date{\small \em Received: 1 January 1970 Accepted: 1 January 1970 Published: 1 January 1970}

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\begin{abstract}
        




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{{\textit{CrossRef DOI of original article:}} \underline{}}
\end{textblock*}\let\tabcellsep& 	 	 		 
\section[{I. INTRODUCTION}]{I. INTRODUCTION}\par
Most organic compounds containing nitrogen (N-heterocyclic), sulfur? long carbon chain, or aromatic, and oxygen atoms are used as a corrosion inhibitors. Among them? organic compounds have many advantages such as large molecular size, soluble in water, availability, cheap? low toxicity? easy for using, and easy production \hyperref[b0]{[1]}. Natural heterocyclic mixes have been utilized for the corrosion inhibitor on the C-steel \hyperref[b1]{[2]}, copper \hyperref[b2]{[3]}, aluminum \hyperref[b3]{[4]}, and various metals in various aqueous medium \hyperref[b4]{[5]}. Adsorption of the drug molecules on the metal surface facilitates its inhibition \hyperref[b5]{[6]}. Heterocyclic mixes have demonstrated more hindrance effectiveness, for C-steel in both HCl \hyperref[b6]{[7]} and H 2 SO 4 arrangements \hyperref[b7]{[8]}, such as the medications are used inhibitors, that can compete favorably with green inhibition of corrosion, and the most medications can be synthesized from natural products. Selection of some medication as corrosion inhibitors due to the followings: (1) drug molecules contain oxygen, sulfur, and nitrogen as active sites, (2) it is environmentally friendly furthermore vital in organic responses, \hyperref[b2]{(3)} drugs can be easily produced, and purified, (4) nontoxic compering organic inhibitors. Some medications have been investigated to be great corrosion inhibitors for metals such as Biopolymer gave 86\% inhibition efficiency (IE) for Cu in NaCl \hyperref[b8]{[9]}, pyromellitic diimide linked to oxadiazole cycle gave 84.6\% IE for mild steel (MS) in HCl \hyperref[b9]{[10]}, 2-mercaptobenzimidazole gave 82\% IE for MS in HCl Antidiabetic Drug Janumet gave 88.7\% IE for MS in HCl \hyperref[b10]{[11]}. Januvia gave 79.5 \% IE for Zn in HCl \hyperref[b11]{[12]},Cefuroxime Axetil gave 89.9\% IE for Al in HCl \hyperref[b13]{[13]}, Phenytoin sodium gave 79\% for MS in HCl \hyperref[b14]{[14]}, Aspirin gave71\% IE for MS in H 2 SO 4 \hyperref[b15]{[15]}, Septazole gave 84.8\% IE for Cu in HCl \hyperref[b16]{[16]} and London Journal of Research in Science: Natural and Formal using Chloroquine diphosphate gave 80\% IE for MS in HCl \hyperref[b17]{[17]}. Study on Structural, Corrosion, and Sensitization Behavior of Ultrafine and Coarse Grain 316 Stainless Steel Processed by Multiaxial Forging and Heat Treatment \hyperref[b18]{[18]}. Investigating the corrosion of the Heat-Affected Zones (HAZs) of API-X70 pipeline steels in aerated carbonate solution by electrochemical methods \hyperref[b19]{[19]}. Predictions of corrosion current density and potential by using chemical composition, and corrosion cell characteristics in microalloyed pipeline steels \hyperref[b20]{[20]}. Predictions of toughness, and hardness by using chemical composition, and tensile properties in microalloyed line pipe steels \hyperref[b21]{[21]}.\par
The scope of this article is used Egy-dronate drug as save corrosion inhibitor for CS in the acid medium by electrochemical method, and to elucidate the mechanism of corrosion inhibition. 
\section[{II. EXPERIMENTAL}]{II. EXPERIMENTAL} 
\section[{Metal samples}]{Metal samples}\par
The sample of CS was used in this study that have the chemical composition of the metal sample was determined by using an emission spectrometer, with the aid of ARL quant meter (model 3100-292 IC) and listed in the Table \hyperref[tab_0]{1}.  
\section[{Preparation of metal sample (working electrode)}]{Preparation of metal sample (working electrode)}\par
Working electrode having the surface area, which, exposed to corrosion media is (1Cm 2 ) cross-section area, and the rod was weld from one side to a copper wire used for electric connection. The sample was embedded in a glass of just a larger diameter than the sample. Epoxy resin was used to stick the sample to glass tube. These also ensured that a constant cross-sectional area would be exposed to corrosive media, through the experiments. The sample was scraped with SiC polisher sheet coarseness sizes (400, 800, and 1200), and clean with (CH3)2CO. Then, clean a few times with bi-distilled water, and dried by soft tissue. Finally, the polishing of sample surface become like a mirror bright, just before immersion in the electrolyte cell. 
\section[{Egy-dronate drug as an inhibitor}]{Egy-dronate drug as an inhibitor}\par
Egy -dronate drug is mixed inhibitors which consists of two substances Alendronic acid, and Cholecalciferol which describing in Table \hyperref[tab_1]{2}.  
\section[{Solution}]{Solution}\par
The aggressive solution, 0.5 M H 2 SO 4 was prepared by dilution of analytical grade (98 \%) H 2 SO 4 with bi-distill water. The concentrations range of the inhibitor were used between 50 ppm to 250 ppm. 
\section[{Potentiodynamic polarization measurement}]{Potentiodynamic polarization measurement}\par
Cathodic, and anodic polarization technique were used for determination the rate of corrosion, by using the electrochemical cell that consists of three electrodes \hyperref[b22]{[22]}:\par
1-A platinum electrode (as an auxiliary electrode).\par
2-Calomel electrode (as the reference electrode). (Hg (l) â?"? Hg 2 Cl 2(s) , KCl (aq) sat,), E equal -241 mV at 25 o C. 3-The working electrode is the CS sample. The electrolytic cell was filled with 100 ml of the solution, and the sample was immersed in the medium. Then, the cathodic polarization was firstly measured, and after reverse the current direction the anodic polarization was measured. 
\section[{Calculation of the rate of corrosion}]{Calculation of the rate of corrosion}\par
The anodic, and cathodic polarization were measured by using the over-potential cells. The corrosion current density (I corr ), the corrosion potential (E corr ), and the corrosion rates (R) are calculated according to the Tafel extrapolation method \hyperref[b23]{[23]}.\par
It is clear that the line representing Tafel region refer by either cathodic, and anodic polarization curve, to obtain the corrosion potential (E corr ), and corrosion current density (I corr ), which can be used to calculate the rate of corrosion by the equation (1) \hyperref[b24]{[24]}\hyperref[b25]{[25]}.\par
Corrosion rate (mpy) = 0.1288 I (mA/cm2) Eq.wt /d (g/cm3)\par
Where, Corrosion rate (mpy) = mils per yea ,I = the corrosion current density, d = Specimen density, and, Eq.wt = Specimen equivalent weight.\par
The corrosion current density (I corr ), corrosion potential (E corr ), and corrosion rate are recorded in Table \hyperref[tab_5]{5}. 
\section[{Applied Evans technique}]{Applied Evans technique}\par
The Evans diagrams give good and suitable interpretation of the electrode-electrolyte interface reactions. We can use the following definitions for the items of Evans diagram as follows \hyperref[b26]{[26]}:\par
1-?? e,m and ?? e,so are anodic and cathodic potentials at equilibrium at the electrode-electrolyte interface (at I =the exchange current i o ) respectively, where ??e,x = E e,x ± â?"?E c -E a â?"?i=i o ; m= metal, so= solution, 2-?? = ?? corr = the relative corrosion potential determined from the position of the intersection of the two curves (de-electronation and electronation processes) where I considered as the i corr .\par
London Journal of Research in Science: Natural and Formal These data can be used for kinetic calculations, and to know, which additive is favorable, or which is faster to the electrode surface at the same conditions. It can be used for studying the inhibition mechanism. 
\section[{Surface Examinations [27]}]{Surface Examinations [27]}\par
The morphology of the CS surface is used for the analysis by examination nature of the surface, and study of changing that appeared on the metal surface. The specimens were prepared by abraded mechanically by using different emery papers up to 1200 grit size, and immersed in 0.5 M H 2 SO 4 (blank) then with 250 ppm of Egy-dronate at room temperature for one day (24 h). Then, after that the specimen was washed gently with distilled water, dried carefully, and take care to the system of surface examinations by Fourier Transforms infrared (FT-IR), scanning electron microscope (SEM), energy dispersive x-ray (EDX), and atomic force microscope (AFM). 
\section[{III. RESULT AND DISCUSSION}]{III. RESULT AND DISCUSSION} 
\section[{Potentiodynamic polarization technique}]{Potentiodynamic polarization technique}\par
Study the polarization of the different medium, and with added the various concentrations of Egy-dronate as a corrosion inhibitor. 
\section[{Dissolution of CS sample in 0.5N H 2 SO 4 at different temperatures}]{Dissolution of CS sample in 0.5N H 2 SO 4 at different temperatures}\par
Results of the anodic, and cathodic polarization processes for the CS sample in 0.5M H 2 SO 4 at different temperatures in the absence of Egy-dronate are shown in Figure \hyperref[fig_1]{1}, and Table \hyperref[tab_5]{5}. It was obvious that the corrosion current density (I corr ) is increased as the temperature increased, and the corrosion potential (E corr ) is slightly shafted to the more positive value. The polarization processes are started with a potential between about 547, and 553 mV. London Journal of Research in Science: Natural and Formal The positive potential is increased by anodic polarization, i.e., increase the dissolved component while that the potential decreased by cathodic polarization, i.e., increase the undissolved components. The dissolved component is formed as the following chemical equations \hyperref[b28]{[28]}:Fe ? Fe 2+ + 2e Fe 2+ + 2H 2 O ? HFeO - 2 + 3H +\par
Where HFeO - 2 Di-hypo-ferrite, green.\par
In the same time occurs asHFeO 2 - + H + ? Fe (OH) 2\par
Where the undissolved hydrated, and the (FeO) can be considered. So that at anodic polarization in the presence of H 2 SO 4 , the iron is dissolved, and formed ferrous sulfate as:Fe 2+ + H 2 SO 4(aq) ? Fe SO 4(aq) + 2H +\par
And the cathodic processes in the presence of H 2 SO 4 occurred asi) 2H + + 2e ? H 2 hydrogen evolution ii) O 2(g) + 4H + (aq) + 4e ? 2H 2 O (l) reduced of oxygen\par
The hydrogen ions adsorbed on the metal surface where an electrochemical reaction takes place in the presence of O 2 as:M + H 3 O + + e ? Mâ?"?H + H 2 O\par
Where three steps can be done as:a. 2Mâ?"?H ? 2M + H 2(g) ? b. Mâ?"?H + H 3 O + + e ? M + H 2(g) ? + H 2 O or c. 4Mâ?"?H + + dissolved O 2 + 4e ? 4M + 2H 2 O (l)\par
London Journal of Research in Science: Natural and Formal\par
The positive potential is increased by anodic polarization, i.e. increase the dissolved component while that the potential decreased by cathodic polarization, i.e., increase the undissolved components.\par
According to the following equation:Fe ? Fe 2+ + 2e anodic reaction 2H 2 O + 2e ? H 2 (g) ? + 2OH - cathodic reaction\par
In total process:Fe + H 2 O ? Fe 2+ + 2OH -? Fe (OH) 2\par
In the bulk the ferrous hydroxide dissolved as:2Fe (OH) 2 ? 2FeOH ++ + 2OH - And, 2Fe OH ++ + 2e ? 2Fe O + H 2 ? 
\section[{Effect of add different concentration of Egy-dronate inhibitor}]{Effect of add different concentration of Egy-dronate inhibitor}\par
The anodic, and cathodic polarization of the CS in a mixed solution 0.   
\section[{Potentiodynamic polarization technique}]{Potentiodynamic polarization technique}\par
It is obvious that the presence of different concentrations are shifted the potentials to low positive values, both anodic potential E a , and cathodic potential E c are shifted to low positive values \hyperref[b29]{[29]}. The anodic current (i a ) slightly decreased (shifted to low values) while the cathodic (i c ) decreased, and shifted to low values too, that are shown in Figure \hyperref[fig_0]{3}. The values of the corrosion potential (E corr ), the corrosion current density (I corr ), and the rate of corrosion in (mpy) are given in Table \hyperref[tab_5]{5}. London Journal of Research in Science: Natural and Formal  \hyperref[tab_2]{3}, it is clear that \hyperref[b30]{[30]}:\par
The parameters (?? corr ), (i corr ), (??' m ), (? a ), (??' a / ?I a ), and (??' c / ?I c ) are decreased with increasing the temperatures. In the other hand the (??' s ), From the above results that are illustrated by Evans diagrams for the electrode-electrolyte interface of the CS. It is clear that:\par
In the presence various concentrations of the Egy-dronate under polarization technique. At low Egy-dronate concentrations the de-electronation potential shifted toward more positive values (positive direction), this means that the polarization are affected the donor functional groups of the Egy-dronate molecules, oriented them to the electron sink area on the electrode surface, and slow done the dissolution of the metal. The size of the Egy-dronate molecules allow to cover somewhat area of electron source, so that the electronation potential of acceptor spices shifted to low positive value. It is observed that the shifted of the de-electronation potential is larger than the shifted of the electronation potential. In the other hand the Egy-dronate concentrations increasing the shift of the electronation potential i.e., the Egy-dronate molecules are covered more electron source area on the corroded metal surface with increasing Egy-dronate concentrations, and the electronation potential shift is being that the larger than the de-electronation potential shift, which indicating that the slightly formation of multilayer, which adsorbed on the metal surface. It is clear that the polarization process affects the orientation, and the adsorption of the inhibitor molecules, so that both the metal dissolution, and the hydrogen evolution are slowing down more.\par
London Journal of Research in Science: Natural and Formal   
\section[{Effect of temperature on corrosion behavior}]{Effect of temperature on corrosion behavior}\par
The results of the anodic, and cathodic polarization processes for the CS sample in the corrosive medium are listed in Table \hyperref[tab_5]{5}. The E corr , I corr , and the rate of corrosion were increased with the temperatures increased at the same concentration 150 ppm of Egy-dronate Figure \hyperref[fig_7]{5}. 
\section[{Potentiodynamic polarization technique}]{Potentiodynamic polarization technique}\par
The behavior of the anodic, and cathodic polarization are indicated that the rate of corrosion of the CS are stimulated by increasing of of temperatures will be enhance the rate of diffusion of hydrogen (H + ) ion to the metal surface beside the ionic mobility, and increasing the conductivity of the electrolyte. Also, at lower temperatures, absorbed hydrogen atoms which are blocked on the cathodic areas, otherwise the increasing the temperatures of the solution, hydrogen will be disrobed from the cathodic area, i.e., the corrosion rate was increased.   
\section[{1-Apply Evans technique}]{1-Apply Evans technique}\par
From the Evans diagrams in the presence of 150 ppm Egy-dronate, which are viewed in Figure \hyperref[fig_8]{6}, and the Evans diagram parameters are listed in Table \hyperref[tab_4]{4}, it is clear that:\par
The parameters (?? corr ), (??' m ), (? a ), | ??' c |, (??' a /?I a ), and (??' c /?I c ) are decreased with increasing the temperatures. In the other hand (i corr ), (??' s ), (? c ), ??' a |, |?I a |, |?I c | are increased the temperatures.\par
From the results that illustrated in Evans diagrams for the electrode-electrolyte interface it is clear that:\par
The effect of the temperature on the behavior of the Egy-dronate as an inhibitor of the CS corrosion at 150 ppm is discussed. It is obvious that both the electronation, and the de-electronation potentials are shifted to negative, and positive direction respectively by increasing the temperature. This behavior clarify that the metal surface divided the electron sink, and electron source area to the small parts, so that the size of the Egy-dronate sufficient to cover more electron source area be side electron sink.   
\section[{Inhibition efficiency (IE \%)}]{Inhibition efficiency (IE \%)}\par
The Egy-dronate compound possess eight active centers like nitrogen, oxygen atoms, and ?-bonding are acted as a donor centers. As a result of the restricted un-plainer structure of the Egy-dronate, and some active sites are acted as a donor centers. These centers are oriented, and adsorbed on anodic sites (iron carbide), due to the Egy-dronate molecule is attached to the anodic site, and covered somewhat of cathodic area, so that the corrosion rate in the presence of Egy-dronate is regarded anodic-cathodic control. The inhibition efficiency (IE \%) is calculated as following \hyperref[b31]{[31]}. 
\section[{IE \% = [(I corr -I' corr )/I corr ] × 100 (1)}]{IE \% = [(I corr -I' corr )/I corr ] × 100 (1)}\par
Where I corr , and I corr ' are the corrosion current densities in the absence, and the presence of an inhibitor respectively. The inhibition efficiency data is listed in Table7. It is obvious that the IE \% for the CS sample increases with increasing the Egy-dronate concentrations.\par
Plot IE \% against logarithm of the concentrations of Egy-dronate inhibitor (log [In]). It is obvious that the increases of the IE \% with the temperatures of the medium are increased, this behavior is indicated that chemisorption's occurs. See Figure \hyperref[fig_9]{7}. The extra part in the curvatures that obtained from polarization technique like f shape indicating that the multilayer proceed from the orientation of functional group under polarization where causes second chemical adsorption over the first layer \hyperref[b32]{[32]}.  
\section[{Scanning Electron Microscopy (SEM)}]{Scanning Electron Microscopy (SEM)}\par
The micrographs are obtained for CS specimens in the nonexistence, and in the existence of 250 ppm of Egy-dronate drug after exposure for immersion one day in corrosive medium 0.5 M H 2 SO 4 . It is clear that CS has suitable surfaces for corrosion attack in the blank or corrosive medium only Figures  {\ref 8 a, b} and {\ref c}. When the Egy-dronate is existence in the corrosive medium, the morphology of CS surfaces is quite different from the previous one, and the specimen surface was smoother. It is clear that the formation of a thin film layer adsorbed on the metal surface, which distributed in a disorder way overall surface of the CS \hyperref[b33]{[33]}. This may be due to the adsorption of the Egy-dronate on the CS surface, and made up the passive film in order to block the active site present on the CS surface. The Egy-dronate molecule is interacted with active sites of CS surface, resulting the decreasing contact between CS, and the corrosive medium. From the above sequentially Egy-dronate is exhibited excellent inhibition effect.  
\section[{Energy Dispersion Spectroscopy (EDX) [34]}]{Energy Dispersion Spectroscopy (EDX) [34]}\par
To determination the elements, and molecules that existence are adsorbed on the surface of CS after one day that immersion in acid with optimum doses of Egy-dronate by using the EDX spectra. The EDX analysis of CS in 0.5 M H 2 SO 4 with in the presence of 250 ppm of the Egy-dronate is given by Figure \hyperref[fig_11]{9}. The spectra show additional lines, demonstrating the existence of C (owing to the carbon atoms of some Egy-dronate). These data shows that the carbon, nitrogen, and oxygen atoms are covered the specimen surface. The EDX analysis is indicated that only carbon, nitrogen, and oxygen are detected, and show that the passivation film is contained the chemical formula of the Egy-dronate drag that adsorbed on the CS surface. It is clear that, the percent weight of adsorbed elements C, N, and O were presented in the spectra, and recorded in Table \hyperref[tab_6]{6}.   
\section[{5 Atomic Force Microscopy (AFM)}]{5 Atomic Force Microscopy (AFM)}\par
AFM is a powerful tool to investigate the surface morphology of various samples at nano-micro scale that is currently used to study the influence of corrosion inhibitor on the metal solution interface. From the analysis, it can be gained regarding the roughness on the surface. The roughness profile values is played an important role to identifying, and report the efficiency of the inhibitor under study. Among the roughness is tacked a role for the explanation of adsorption, and illustrated the nature of the adsorbed film on the metal surface \hyperref[b35]{[35]}\hyperref[b36]{[36]}. Figure \hyperref[fig_12]{10} a, shows the 3D images as well as elevation profiles of polished of the CS in the absence, and the presence the Egy-dronate as an inhibitor.  
\section[{6 Fourier transforms infrared spectra (FT -IR)}]{6 Fourier transforms infrared spectra (FT -IR)}\par
The (FT -IR) spectrophotometer is a powerful instrument that can be used to identify the function group that presence in organic compounds and the type of interaction that occur between function group with metal surface. Since, pharmaceutical drug compound contain variety of organic compound, and these organic compounds (inhibitor) are adsorbed on the metal surface providing thin film that protection them against corrosion, they can be analyzed by using (FT -IR). To confirm the nature of the chemical constituent is adsorbed on the metal surface, by the Fourier transform infrared (FT -IR) spectra \hyperref[b37]{[37]}.\par
The pharmaceutical drug compounds are certain have function group according to the chemical formula like OH, C=C and P=O. In order to find the nature of constituents involved in the adsorption using (FT -IR) spectrum of material that are coated the metal surface gives in Figures 11. The spectrum of Egy -dronate before, and after adsorption that seen the wave number of the function groups OH abroad peak at 3400 cm -1 starching, C=C is sharp peak at 1630 cm -1 starching, and P=O a sharp peak between 1140 -1000 cm -1 starching. It is clear that the function groups of Egy -dronate inhibitor appear on the metal surface that confirm to the adsorption process \hyperref[b38]{[38]}.  
\section[{Mechanism of inhibition}]{Mechanism of inhibition}\par
To illustrate the mechanism of inhibition of corrosion on the CS surface in acid medium by using pharmaceutical drug compound as an inhibitor, it is must be know the nature of metal surface, and the nature of the component of inhibitor structure. The CS is regarded the metal ?-phase \hyperref[b39]{[39]}, It is obvious that ?-phase state consists of grains, and grain boundaries in the surface of the metal, Figure \hyperref[fig_14]{12}. A cross-section of a piece or specimen of the metal that is a corroding to clarify that there are both anodic, and cathodic sites in the metal surface structure. The surface of iron is usually, coated with a thin film of iron oxide. However, if this iron oxide film develops some cracks, anodic area are created on the surface, while other metal parts acts as cathodic sets. It follows that the anodic areas are small surface, while nearly the rest of the surface of the metal large cathodes. Electrochemical corrosion involves flow of electric current between the anodic, and London Journal of Research in Science: Natural and Formal cathodic areas called inter-granular corrosion. Figure \hyperref[fig_15]{13}, SEM image is shown the corrosion of the CS in 0.5 N H 2 SO 4 in one day immersion that illustrated inter-granular corrosion. All previous results prove that the pharmaceutical drug compound under study were actually inhibit the corrosion of the CS in 0.5 M H 2 SO 4 solution as a corrosive medium. The corrosion inhibition is due to their physical, and chemical adsorption for formation of protection thin film adsorbed on the metal surface. The effect of Egy-dronate as inhibitor may be corresponding to the accumulation of the inhibitor molecules on the metal surface, which prevent the direction contact of the metal surface with corrosive environment. The surface of the CS sample have positively charge in aqueous acid solution, and the adsorption occur according to \hyperref[b40]{[40]}:\par
1-The unshared electrons of nitrogen, oxygen atoms, and electron density of ? bonding donate to the vacant orbital on the metal surface make chemisorption. 2-The partial negative charge that present in function group containing Oxygen, nitrogen, and electron density of ?-bond in Egy-dronate may be adsorbed on the positively charge of the metal surface like electrostatic attraction between the opposite charge, in the form of neutral molecules, that involving displacement of water molecules from the metal surface.\par
The inhibition action of the Egy-dronate can be accounted by the interaction between the lone pair of electrons in the nitrogen, oxygen, and electron density of ?-bond with positively charged (anodic sites) on the metal surface, and the skeleton of inhibitor compound cover the cathodic sites this action form thin layer adsorbed on the metal surface and prevent corrosion processes Figure \hyperref[fig_16]{14}. This meaning, the Egy-dronate molecule attached with anodic site, and covered somewhat of cathodic area, so that the corrosion rate in presence of Egy-dronate is anodic-cathodic control. 
\section[{IV. CONCLUSION}]{IV. CONCLUSION}\par
Inhibition of the corrosion of the CS in 0.5 M H 2 SO 4 solution by Egy-dronate is determine by potentiodynamic polarization, Evans techniques, and surface examination by Scanning Electron Microscopy (SEM), Energy Dispersive X-ray (EDX), Atomic Force Microscopy (AFM), and Fourier Transforms Infrared (FT-IR). It was found that the inhibition efficiency depends on concentration, nature of metal surface, and the type of adsorption of the inhibitor. The observed corrosion data in the presence the Egy-dronate as an inhibitor:\par
1) The tested Egy-dronate inhibitor establish a very good an inhibition efficiency for the CS corrosion in 0.5 M H 2 SO 4 solution.\par
2) Egy-dronate inhibit the CS for the corrosion by the adsorption on its surface, and make thin film layer protective them from corrosion process.\par
3) The inhibition efficiencies of the Egy-dronate increases with the increasing of their concentrations.\par
4) The values of inhibition efficiencies obtained from all techniques that using are seen the validity of the obtained results. 5) The Egy-dronate molecule attached with anodic site, and covered somewhat of cathodic area, so that the corrosion rate in the presence of the Egy-dronate is anodic-cathodic control.\begin{figure}[htbp]
\noindent\textbf{3}\includegraphics[]{image-2.png}
\caption{\label{fig_0}3 -}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{1}\includegraphics[]{image-3.png}
\caption{\label{fig_1}Figure 1 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{}\includegraphics[]{image-4.png}
\caption{\label{fig_2}}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{2}\includegraphics[]{image-5.png}
\caption{\label{fig_3}Figure 2 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{3}\includegraphics[]{image-6.png}
\caption{\label{fig_4}Figure 3 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{}\includegraphics[]{image-7.png}
\caption{\label{fig_5}}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{4}\includegraphics[]{image-8.png}
\caption{\label{fig_6}Figures 4 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{5}\includegraphics[]{image-9.png}
\caption{\label{fig_7}Figure 5 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{6}\includegraphics[]{image-10.png}
\caption{\label{fig_8}Figure 6 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{7}\includegraphics[]{image-11.png}
\caption{\label{fig_9}Figure 7 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{}\includegraphics[]{image-12.png}
\caption{\label{fig_10}}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{9}\includegraphics[]{image-13.png}
\caption{\label{fig_11}Figure 9 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{10}\includegraphics[]{image-14.png}
\caption{\label{fig_12}Figure 10 b}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{11}\includegraphics[]{image-15.png}
\caption{\label{fig_13}Figure 11 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{12}\includegraphics[]{image-16.png}
\caption{\label{fig_14}Figure 12 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{13}\includegraphics[]{image-17.png}
\caption{\label{fig_15}Figure 13 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{14}\includegraphics[]{image-18.png}
\caption{\label{fig_16}Figure 14 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{1} \par 
\begin{longtable}{P{0.14468085106382977\textwidth}P{0.12659574468085105\textwidth}P{0.14468085106382977\textwidth}P{0.12659574468085105\textwidth}P{0.1627659574468085\textwidth}P{0.14468085106382977\textwidth}}
Sample\tabcellsep C\%\tabcellsep Mn\%\tabcellsep V\%\tabcellsep Fe\%\tabcellsep Si\%\\
CS\tabcellsep 0.26\tabcellsep 0.77\tabcellsep 0.11\tabcellsep 98.51\tabcellsep 0.35\end{longtable} \par
 
\caption{\label{tab_0}Table 1 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{2} \par 
\begin{longtable}{P{0.04975609756097561\textwidth}P{0.09951219512195122\textwidth}P{0.39390243902439026\textwidth}P{0.11195121951219512\textwidth}P{0.07463414634146341\textwidth}P{0.12024390243902437\textwidth}}
Inhibitor\tabcellsep Structure\tabcellsep IUPAC\tabcellsep Molecular\tabcellsep Active\tabcellsep Chemical\\
\tabcellsep \tabcellsep Name\tabcellsep weight\tabcellsep centers\tabcellsep formula\\
\tabcellsep \tabcellsep sodium\tabcellsep \tabcellsep N\tabcellsep C 4 H 13 NOP 2\\
\tabcellsep \tabcellsep {}[4-amino-1-hydr\tabcellsep \tabcellsep 7O\tabcellsep \\
\tabcellsep \tabcellsep oxy-1-(hydroxy-\tabcellsep \tabcellsep 2?\tabcellsep \\
\tabcellsep \tabcellsep \tabcellsep 249.097\tabcellsep \tabcellsep \\
(1)\tabcellsep \tabcellsep oxido-phosphor\tabcellsep \tabcellsep \tabcellsep \\
\tabcellsep \tabcellsep \tabcellsep g/mol\tabcellsep \tabcellsep \\
\tabcellsep \tabcellsep yl)-\tabcellsep \tabcellsep \tabcellsep \\
\tabcellsep \tabcellsep butyl]phosphoni\tabcellsep \tabcellsep \tabcellsep \\
\tabcellsep Alendronic acid\tabcellsep c acid trihydrate\tabcellsep \tabcellsep \tabcellsep \end{longtable} \par
 
\caption{\label{tab_1}Table 2 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{3} \par 
\begin{longtable}{}
\end{longtable} \par
 
\caption{\label{tab_2}Table 3 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{4} \par 
\begin{longtable}{}
\end{longtable} \par
 
\caption{\label{tab_4}Table 4 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{5} \par 
\begin{longtable}{P{0.85\textwidth}}
at various temperatures\end{longtable} \par
 
\caption{\label{tab_5}Table 5 :}\end{figure}
 \begin{figure}[htbp]
\noindent\textbf{6} \par 
\begin{longtable}{P{0.5469565217391303\textwidth}P{0.18478260869565216\textwidth}P{0.03695652173913043\textwidth}P{0.03695652173913043\textwidth}P{0.04434782608695652\textwidth}}
London Journal of Research in Science: Natural and Formal\tabcellsep \tabcellsep \tabcellsep \tabcellsep \\
\tabcellsep \multicolumn{2}{l}{of the Egy-dronate}\tabcellsep \tabcellsep \\
Wt \%\tabcellsep Fe\tabcellsep C\tabcellsep N\tabcellsep O\\
Egy -dronate\tabcellsep 75.97\tabcellsep 2.08\tabcellsep 1.88\tabcellsep 20.68\end{longtable} \par
 
\caption{\label{tab_6}Table 6 :}\end{figure}
 			\label{foot_0}\footnote{\label{foot_0} © 2023 London Journals Press Volume 23 | Issue 3 | Compilation 1.0} 			\label{foot_1}\footnote{\label{foot_1} © 2023 London Journals Press} 			\label{foot_2}\footnote{\label{foot_2} © 2023 London Journals Press} 			\label{foot_3}\footnote{\label{foot_3} Electrochemical Study for using Eg-Dronate Drug as a Green Corrosion Inhibitor in 0.5 M H2SO4 Solution by Applied: Potentiodynamic and Evans Techniques} 			\label{foot_4}\footnote{\label{foot_4} © 2023 London Journals Press Volume 23 | Issue 3 | Compilation 1.0 Electrochemical Study for using Eg-Dronate Drug as a Green Corrosion Inhibitor in 0.5 M H2SO4 Solution by Applied: Potentiodynamic and Evans Techniques} 			\label{foot_5}\footnote{\label{foot_5} © 2023 London Journals Press} 			\label{foot_6}\footnote{\label{foot_6} London Journal of Research in Science: Natural and Formal} 			\label{foot_7}\footnote{\label{foot_7} © 2023 London Journals Press Volume 23 | Issue 3 | Compilation 1.0} 			\label{foot_8}\footnote{\label{foot_8} © 2023 London Journals Press Volume 23 | Issue 3 | Compilation 1.0} 		 		\backmatter  			  				\begin{bibitemlist}{1}
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\end{bibitemlist}
 			 		 	 
\end{document}
