Zingiber Officinal Roscoe Extract Using as Green Corrosion inhibitor for Mild Steel in 1M HCl Media

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Der Pharma Chemica, 2015, 7(7):377-388 (http://derpharmachemica.com/archive.html)

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Zingiber Officinal Roscoe Extract Using as Green Corrosion inhibitor for Mild Steel in 1M HCl Media

F. Yousfi1, M. El Azzouzi1, M. Ramdani1;*, H. Elmsellem1, A. Aouniti1, N. Saidi1, B. El

Mahi 1, A. Chetouani1, 2 and B. Hammouti1

1URAC18, COST, Laboratoire de Chimie Appliquée et environnement, Department of

Chemistry, Faculty of Sciences, Mohamed 1st University, P.O. Box 717, Oujda, 60000, Morocco 2Laboratoire de chimie physique, Centre Régionale des Métiers de l'Education et de Formation

''CRMEF'', Région de l'Orientale, Oujda, Morocco _____________________________________________________________________________________________ ABSTRACT Various techniques carried out to reduce or decrease the corrosion rate of materials and metal alloys. The use of green inhibitors is one of the most practical techniques used against this phenomenon. In this work, we have studied the influence of aqueous extracts of ginger rhizomes on the corrosion of mild steel in 1M HCl acid medium by electrochemical measurements: polarization curve, electrochemical impedance spectroscopy and weight loss measurements. The results showed that the inhibition efficiency was found to increase with inhibitor content to attain 95% in the presence of the ginger concentration 10-3M at 308K. The effect of temperature on the behaviour of corrosion showed that the inhibition efficiency of deferent extracts decreased significantly with temperature. The adsorption of various extracts on the steel surface follows the Langmuir’s adsorption isotherm. Key words: Corrosion, Zingiber Officinal Roscoe, Green inhibitor, Mild Steel, HCl. _____________________________________________________________________________________________

INTRODUCTION

Corrosion is a deterioration of a metal or a metal alloy and an alteration of its physical properties under the influence of its environment. These phenomena have major impacts in various fields, particularly in industry. For example, the work stoppage and change of corroded material for the industry is very high financial burden [1]. The use of inhibitors is one of the best techniques that can prevent corrosion of materials and alloy with its environment. Inhibitors are substances that added to the small quantities in the middle to reduce the corrosion rate of the material. Several synthetic compounds exhibit a good anti-corrosion action, although most of them are not only expensive, but also toxic and present a danger for the environment [2]. This justifies the orientation of scientific research towards new means of protection such as using green inhibitors. Plants extracts considered an important source, easily accessible, renewable and can offer very high inhibitory properties for many metal alloys [3-6]. Ginger or Zingiber Officinal Roscoe is one of the most recognized spices in the world for medicinal and flavouring properties, attributed to the constituents of the essential oil and extracts, which are of great interest in the food and cosmetics industry [7, 8]. Several studies have shown that consumption of fresh ginger or dried was beneficial to health. Besides ginger has several activities such as, anti-tumour, anti-inflammatory, anticancer, antioxidant, antiallergic, antinauseant, antiemetic, antihepatotoxic, antipyretic, antiseptic, antitussive, hypoglycaemic, antiplatelet, hypolipidemic, carminative, aromatic, stimulant, stomachic and tonic activities [9-18]. For the first time Akhani and col. have shown that ginger possesses anti-diabetic activity by virtue of 5-HT modulators present in Z. officinal [19]. However, the use of the ginger extract as a corrosion inhibitor is limited. In the literature, few studies have been carried out recently in various conditions and indicated an excellent protective effect. Recently,

M. Ramdani et al Der Pharma Chemica, 2015, 7 (7):377-388 _____________________________________________________________________________


Kurniawan and col. [20] showed good inhibition efficiency about 81.66% by using 500 ppm of ginger toward corrosion of steel in 3.5% of sodium chloride and 0.1M HCl. Fouda and col. [21] reported that the use of 250 ppm of ginger presented 84.8% of inhibition efficiency for steel in 3.5% of NaCl with 16 ppm of Na2S. A synergistic effect on corrosion inhibition efficiency of ginger extract in controlling corrosion of mild steel in 0.5N H2SO4 media was reported by Subramanian and col. [22]. 100 ppm of methanolic extract of ginger with 50 ppm of KI conducted to 88.61% of inhibition efficiency. Ginger exhibited an excellent inhibitory effect on corrosion of steel in HCl [23]. The objective of this work is to study the influence of aqueous extracts of ginger rhizomes on the corrosion of mild steel in 1M HCl acid medium by electrochemical measurements: weight loss, polarization curve and electrochemical impedance spectroscopy. Also, the effects of ginger concentration and temperature immersion were controlled.

MATERIALS AND METHODS 2.1. Preparation of Extracts Ginger was purchased from the local market and ground into a fine powder, figure 1. Three samples were prepared at different temperatures. For each sample 25g of powder was macerated in 70ml of distilled water under magnetic agitation for 2 hours at room temperature (AE1), 40 °C (AE2) and 100 °C (AE3). After filtration, the aqueous extract was evaporated in an incubator for 2 to 3 days at 40 °C. The aggressive solutions of 1.0 M HCl were prepared by dilution of an analytical grade 37% HCl with double distilled water.

(a) (b)

Figure 1: (a): Zingiber Officinal Roscoe, (b): Zingiber powder Different concentrations (0.125, 0.25, 0.5 and 1 g/l) were prepared from the ginger powder by dissolving the required amount of ginger in 100 ml of 1 M HCl with stirring at room temperature. 100 ml of 1 M HCl without inhibitor was used as blank test solution. 2.2. Preparation of Specimens Coupons of mild steel specimens were cut into 2× 2 × 0.25 cm3 dimensions having composition (0.09% P, 0.01 % Al, 0.38 % Si, 0.05 % Mn, 0.21 % C, 0.05 % S and Fe balance) used for weight loss measurements. Prior to all measurements, the exposed area was mechanically abraded with 180, 400, 800, 1000, 1200 grades of emery papers. The specimens are washed thoroughly with bidistilled water degreased and dried with ethanol. 2.3. Weight Loss Method Gravimetric measurements are carried out in a double walled glass cell equipped with a thermostated cooling condenser. The solution volume is 100 cm3. The immersion time for the weight loss is 6 h at (308±1) K. In order to get good reproducibility [24-26], experiments were carried out in duplicate. The weight of each specimen before and after immersion was determined using shimadzu balance, model Ay 62. The corrosion rate (V) is calculated using the following equation:

V = w / st (1)

Where: W is the average weight loss, S the total area, and t is the immersion time. The inhibition efficiency (Ew) is determined as follows:

Ew % = (V0 - V / V0) x 100 (2)

Where: V0 and V are the corrosion rates in the absence and presence of the inhibitor, respectively. 2.4. Polarization Measurements The electrochemical study was carried out using a potentiostat PGZ100 piloted by Volta master soft-ware. This potentiostat is connected to a cell with three electrode thermostats with double wall. A saturated calomel electrode (SCE) and platinum electrode were used as reference and auxiliary electrodes, respectively. Anodic and cathodic potentiodynamic polarization curves were plotted at a polarization scan rate of 0.5mV/s. Before all experiments, the potential was stabilized at free potential during 30 min. The polarization curves are obtained from −800 mV to −200



mV at 308 K. The solution test is there after de-aerated by bubbling nitrogen. Inhibition efficiency (Ep %) is defined as Equation (3), [27, 28]

Ep % = (Iocorr – Icorr / Iocorr) x 100 (3)

Where, I°corr and Icorr represent corrosion current density values in the absence and presence of the inhibitor, respectively. 2.5. Impedance measurements The electrochemical impedance spectroscopy (EIS) measurements are carried out with the electrochemical system, which included a digital potentiostat model Volta lab PGZ100 computer at Ecorr after immersion in solution without bubbling. After the determination of steady-state current at a corrosion potential, sine wave voltage (10 mV) peak to peak, at frequencies between 100 kHz and 10 mHz are superimposed on the rest potential. Computer programs automatically controlled the measurements performed at rest potentials after 0.5 hour of exposure at 308 K. The impedance diagrams are given in the Nyquist representation. Inhibition efficiency (IE %) is estimated using the relation (4), [27, 28].

IE % = (Rct – R°ct / Rct) x 100 (4)

Where, R°

ct and Rct are the charge transfer resistance values in the absence and presence of inhibitor, respectively:

RESULTS AND DISCUSSION

Weight Loss Measurements 3.1.1 Inhibitor concentration effect The corrosion rates and inhibition efficiency values, calculated using weight loss data, for various concentrations (0.125, 0.25, 0.5 and 1 g/l) at 308K of three ginger aqueous extracts (AE1, AE2 and AE3) for the corrosion of carbon steel in 1 M HCl solution are presented in Table 1. It was apparent that the inhibition efficiency increased with the increase in inhibitor concentration, figure 2. This behaviour can be explained based on the strong interaction of the inhibitor with the metal surface resulting in adsorption. The extent of adsorption increased with the increase in concentration of the inhibitor leading to increased inhibition efficiency. The maximum inhibition efficiency (93%) was observed at an inhibitor concentration of 1g/l for the AE3 aqueous extracts. However, a minor difference was detected comparing the results obtained for the three extracts at 1g/l as concentration. Also, we noted that good inhibition efficiency (84%) was observed for AE1 extract at only a low concentration (0.125 g/l). This result constituted the bust experimental and economical conditions for the corrosion inhibition because the extract was prepared at ambient temperature and the inhibitor concentration was relatively low comparing with the two other extracts.

Table 1. Effect of ginger aqueous extracts on the corrosion rate of mild steel in 1 M HCl at 308K.

Inhibitor Concentration g/l

Corrosion rate mg/cm2.h

E (%)

Blank 1M 9.07 _ AE1 1 0.84 91

0.5 1.14 87 0.25 1.25 86 0.125 1.40 84

AE2 1 0.95 89 0.5 1.17 87 0.25 2.84 69 0.125 3.00 67

AE3 1 0.65 93 0.5 0.77 91 0.25 0.92 90 0.125 1.24 86

Generally, the inhibitor suppers the metal dissolution by forming a protective film adsorbed to the metal surface and separating it from the corrosion medium.



0.0 0.2 0.4 0.6 0.8 1.065

70

75

80

85

90

95

Concentrations

Effi

cien

cy (

%)

AE1 AE2 AE3

Figure 2: Variation of the inhibition efficiency of different concentrations of extracts in 1M HCl medium

3.1.2 Temperature effect: The effect of temperature on the inhibition efficiency, in the temperature range 313-343 K, in 1 M HCl, was studied using gravimetric experiments in the absence and presence of 1 g/l of inhibitor after 1 h of immersion time. The results obtained are summarized in Table 2. The fractional surface coverage θ can be easily determined from weight loss measurements by the ratio E % / 100 if one assumes that the values of E % do not differ substantially from θ. It is clear from Table 2 and Figure 3 that increasing the corrosion rate (V) was more pronounced with the rise of temperature for blank solution. In the presence of the ginger extracts inhibitors, the corrosion rate of mild steel decreased at any given temperature due to the increasing of the degree of surface coverage. The results showed clearly that the inhibition efficiency decreased with increasing of the temperature, Figure 3.

Table 2. Effect of temperature on the corrosion rate of mild steel in 1 M HCl at 1g/l as extracts concentration for 1h.

Inhibitor Temperature (K)

Corrosion rate (g/cm².h)

E (%)

Θ

HCl

313 10.117 - - 323 19.718 - - 333 22 .108 - - 343 41.61 - -

AE1

313 1.67 83 0.83 323 4.24 78 0.78 333 6.88 69 0.69 343 16.65 60 0.60

AE2

313 2.15 79 0.79 323 4.69 76 0.76 333 7.52 66 0.66 343 17.56 58 0.58

AE3

313 1.51 85 0.85 323 3.96 80 0.80 333 5.13 77 0.77 343 13.0065 69 0.69



310 315 320 325 330 335 340 3450

5

10

15

20

25

30

35

40

45

HCl 1M AE1 AE2 AE3

Cor

rosi

on r

ate

(g/c

m².

h)

Temperature (K)

Figure 3: Variation of the corrosion rate of extracts on the mild steel in 1M HCl medium versus several temperatures

In order to calculate activation parameters for the corrosion process, Arrhenius Eq. (5) and transition state Eq. (6) were used [29]:

= (− ) (5)

= exp

°

exp(∆°

) (6)

Where Ea is the apparent activation corrosion energy; R is the universal gas constant; k is the Arrhenius pre-exponential factor; h is Plank’s constant; N is Avogadro’s number; ∆Sa is the entropy of activation and ∆Ha is the enthalpy of activation. Arrhenius plots for the corrosion rate of mild steel are given in Figure 4 and Figure 5. Values of apparent activation energy of corrosion (Ea) for mild steel in 1.0 M HCl with the absence and the presence of various concentrations of extracts were determined from the slope of Ln(v) versus 1/T plots ginger extracts and shown in Table 3. The relationship between temperature and corrosion rate it does not just show the corrosion behaviour of the mild steel against changing temperature, it providing us several information including the activation thermodynamic parameters such as activation energy Ea, activated entropy ∆Sa and enthalpy ∆Ha by using Arrhenius equation :

(ѵ) = () − (7)

ѵ = ( +

∆ ) −

∆" (8)

Where V is the corrosion rate; A is a constant depends on metal type and electrolyte; #$ is the apparent activation energy; h is the Planck’s constant (6.626176 x 10-34 Js); N is the Avogadro number (6.02252 x 1023 mol-1); R is the universal gas constant; T is the absolute temperature, ∆%$ and ∆&$ are the enthalpy and the entropy of activation, respectively. All the parameters are listed in Table 3.



2,90 2,95 3,00 3,05 3,10 3,15 3,200,0

0,5

1,0

1,5

2,0

2,5

3,0

3,5

4,0 EA1 EA2 EA3HCl 1M

Ln(ν

) (g/

cm².

h)

1000/T (K-1)

Figure 4: Arrhenius Plots in the absence and presence of extracts in 1M HCl medium

2,90 2,95 3,00 3,05 3,10 3,15 3,20-5,5

-5,0

-4,5

-4,0

-3,5

-3,0

-2,5

-2,0

EA1 EA2 EA3 HCl 1M

Ln (

ν/Τ)

(g/c

m².

h.K

)

1000/T (K-1)

Figure 5: Variation of Ln( ν/T) versus 1000/T with different extracts in 1M HCl medium

Table 3: Activation parameters for the steel dissolution in 1.0 M HCl in the absence and the presence of ginger extracts at 1 g/l of

concentration

Inhibitor Concentration (g/l)

Ea

(kJ mol-1) ∆Ha

(kJ mol-1) ∆Sa

(kJ mol-1) HCl 1M 38.884 36.167 110.113 AE1 1 65.786 63.061 39.278 AE2 1 60.359 57.616 54.783 AE3 1 59.860 57.175 58.774

According to the results listed in the table 3, we conclude that: • The activation energy Ea in absence of the extracts is lower than in the presence of AE1, AE2 and AE3. It indicates that the adsorption process is physical (electrostatic) [30-32] • The positive values of ∆Ha indicate the endothermic process of metal dissolution. • The positive values of entropies ∆Sa imply that the activated complex in the rate determining step represents an association rather than a dissociation step, meaning that a decrease in disordering takes place ongoing from reactants



to the activated complex and suggesting that the dissolution reaction will be more blocked sites from the metal surface [33]. 3.1 Adsorption isotherm and standard adsorption free energy In order to gain more information about the mode of adsorption of ginger extracts on the surface of mild steel, the experimental data have been tested with several adsorption isotherms, including Langmuir, Frumkin, Freundlich and Temkin isotherms. However, the best fit was obtained from the Langmuir isotherm. This isotherm can be represented as [34]:

'ϴ= () + * (5)

Where K is the adsorption constant; C is the concentration of the inhibitor and surface coverage values (θ) are obtained from the weight loss measurements for various concentrations. Kads is the equilibrium constant of the adsorption process and is related to the standard Gibbs energy of adsorption, ∆Gads, according to [35]:

∆Gads = -RTLn(55.55Kads) (6)

Where R is the universal gas constant and T is the absolute temperature. The value 55.55 in the above equation is the concentration of water in solution in mol/l. Thermodynamic parameters is important to study the inhibitive mechanism. The values of Kads, R2 and ∆Gads are calculated and are (out) given in Table 4. The relation between Cinh/θ and Cinh is shown in Figure 6. These plots are linear with a slope equal to unity. This suggests that the adsorption of ginger extracts on metal surface followed the Langmuir adsorption isotherm.

0,2 0,4 0,6 0,8 1,0

0,2

0,4

0,6

0,8

1,0 EA1 EA2 EA3

C/Θ

(g/l)

Concentration (g/l)

Figure 6 : Langmuir adsorption of AE1, AE2 and AE3 on the mild steel in 1M HCl medium

The free energy of adsorption ∆G°ads negative values show a spontaneous process, according to the reference, if the ∆G°

ads value is up to -20 kJ/mol, it is consistent with a physisorption; and those around -40 kJ/mol or higher are consistent with chemisorptions. Our results reveal some values in the average of -20 kJ/mol, which means that the adsorptions of AE1, AE2 and AE3 on the mild steel are physisorption.

Table 4: Parameters of the linear regression between C/θ and C and thermodynamic values of adsorption extracts on the steel mild in

1M HCl media.

Inhibitor Linear correlation

Slope K ∆G°ads (kJ mol-1)

AE1 0.99957 1.089 58.82 -20.718 AE2 0.99508 1.041 13.88 -17.022 AE3 0.99999 1.066 83.33 -21.610

3.3 Potentiodynamic polarization curves: The electrochemical measurement was carried out to understand the kinetic process of the anodic and cathodic reactions. The mild steel electrode maintained at corrosion potential for 30 min and thereafter pre-polarized at 800 mV for 10 min. The potential starts from -800 mV to -200 mV with a scan rate of 1 mV/s.



Potentiodynamic polarization curves of carbon steel in 1.0 M HCl containing ginger extracts at 308K are shown in Figure 7. The electrochemical corrosion parameters including corrosion current density (Icorr); corrosion potential (Ecorr); cathodic Tafel slope (βc) and inhibition efficiency EP(%) values were derived from cathodic current-potential curves. They are presented in Table 4. The EP(%) was calculated from polarization measurements according to the relation given below [27]:

#% = ,-.//. 0,-.//,-.//. × 100 (7)

Where iocorr and icorr are the corrosion current densities for steel electrode in the uninhibited and inhibited solutions, respectively.

-800 -700 -600 -500 -400 -300 -200-3

-2

-1

0

1

2

HCl 1M 1 g/l0,5 g/l0,25 g/l0,125 g/l

Log

i (µ

A,c

m²)

E (mv)

-800 -700 -600 -500 -400 -300 -200-3

-2

-1

0

1

2

HCl 1M 1 g/l0,5 g/l0,25 g/l0,125 g/l

Log

i (µ

A,c

m²)

E (mv)

-800 -700 -600 -500 -400 -300 -200-3

-2

-1

0

1

2

HCl 1M 1 g/l0,5 g/l0,25 g/l0,125 g/l

Log

i (µ

A,c

m²)

E (mv)

Figure 7: Polarization curves AE1, AE2 and AE3 in absence and presence of different concentrations in 1M HCl



Table 5: Corrosion parameters in the presence and absence of inhibitor obtained from polarization measurements

Inhibitor Concentration (mol l-1)

Ecorr

(mV/SCE) I corr

(µA/cm2) βc

(mV/dec) E %

Blank 0 -453 0.7602 -147 -

AE1

1 -452 0.0376 -149 95% 0.5 -452 0.0518 -223 93% 0.25 -468 0.0623 -154 91% 0.125 -466 0.083 -156 89%

AE2

1 -458 0.0476 -155 93% 0.5 -478 0.0673 -185 91% 0.25 -477 0.0830 -157 89% 0.125 -483 0.1211 -156 84%

AE3

1 -445 0.0143 -121 98% 0.5 -449 0.0475 -165 93% 0.25 -469 0.0644 -156 91% 0.125 -447 0.0689 -170 90%

Inspection of the figure 7 shows that the addition of ginger extracts has an inhibitive effect in the both anodic and cathodic parts of the polarization curves and generally shifted the Ecorr value towards the positive direction compared to the uninhibited mild steel. Thus, addition of this inhibitor reduces the mild steel dissolution as well as retards the hydrogen evolution reaction. The presence of ginger extracts does not prominently shift the corrosion potential, which indicates that the studied ginger extracts inhibitor act as mixed-type inhibitor [23-26]. Furthermore, in the presence of this inhibitor, the slight change of βc indicates that the cathodic corrosion mechanism of steel does not change. The table 5 represent different electrochemical parameters including corrosion potential Ecorr; corrosion current density Icorr; cathodic Tafel slope βc and the inhibition efficiency E%. The results revealed that AE3 is the best inhibitor with a relatively higher inhibition efficiency (98%), following by AE1 extract with 95% and AE2 extract with 93%. The Ecorrvalues shifted slightly to the cathodic potential, according to literature if the displacement in Ecorr is more than ±85mV relating to the corrosion potential of the blank, the inhibitor can be considered as a cathodic oranodic type, if the change in Ecorr is less than ±85 mV, the corrosion inhibitor may be regarded as a mixed type [27,28]. In our case the maximum displacement is 30 mV lower than ±85 mV indicating that our inhibitors act as mixed-type.

3.4 Electrochemical impedance spectroscopy: The electrochemical impedance spectroscopy was carried out using a Volta lab (Tacussel- Radiometer PGZ 100) potentiostate and controlled by Tacussel corrosion analysis software model (Voltamaster 4) at under static condition. The corrosion cell used had three electrodes. The reference electrode was a saturated calomel electrode (SCE). A platinum electrode was used as auxiliary electrode of surface area of 1 cm2. The working electrode was carbon steel. All potentials given in this study were referred to this reference electrode. The working electrode was immersed in test solution for 30 minutes to a establish steady state open circuit potential (Eocp). After measuring the Eocp, the electrochemical measurements were performed. All electrochemical tests have been performed in aerated solutions at 308 K. The EIS experiments were conducted in the frequency range with high limit of 100 kHz and different low limit 10 Hz at open circuit potential, with 10 points per decade, at the rest potential, after 30 min of acid immersion, by applying 10 mV ac voltage peak-to-peaks. Nyquist plots were made from these experiments. The best semicircle can be fit through the data points in the Nyquist plot using a non-linear least square fit so as to give the intersections with the x-axis [27]. The next equation represents the relationship between the inhibition efficiency and the charge transfer values taken from the table 6 [26]:

#% = 404.4× 100 (8)

The Nyquist plots for carbon steel obtained by adding AE1, AE2 and AE3 in 1M HCl at 308K are represented in figure 8. The existence of a single semicircle indicating the presence of a single transfer process, also the Nyquist plots characterized by one capacitive loop either in presence or in absence of the inhibitors. The capacitive loops are not perfect semicircles because of the non-homogeneity and roughness of the carbon steel surface [35]. The increase in the concentration of the inhibitors implies to an increase in the inhibition efficiency values. The double layer capacitance Cdl given as in the Helmotz model by:

Cdl = ℇ6×ℇδ

S (9)



Where δ is the thickness of the deposit; S is the surface of the electrode; ε0 is the permittivity of the air and ε is the medium dielectric constant. The decrease in Cdl values could be interpreted either by a decrease of local dielectric constant ε [36] or by the thickness of the adsorb inhibitor layer on the metal surface [37]. The decrease in Cdl values with the addition of inhibitor is due to the adsorption of the inhibitor molecules replacing water at the metal–solution interface. That led to the decrease in local dielectric constant and/or an increase in the thickness of the electrical double layer.

0 100 200 300 400 500

0

50

100

150

200

250

HCl 1M 1 g/l 0,5 g/l 0,25 g/l 0,125 g/l

-Zim

(Ω .c

m²)

Zr (Ω .cm²)

0 100 200 300 400 500

0

50

100

150

200

250

HCl 1M 1 g/l 0,5 g/l 0,25 g/l 0,125 g/l

-Zim

(Ω .c

m²)

Zr (Ω .cm²)

0 200 400 600 800 1000

0

100

200

300

400

500

HCl 1M 1 g/l 0,5 g/l 0,25 g/l 0,125 g/l

-Zim

(Ω .c

m²)

Zr (Ω .cm²)

Figure 8: Nyquist plots of AE1, AE2 and AE3 in absence and presence of different concentrations in 1M HCl



Table. 6. Corrosion parameters obtained by impedance measurements for mild steel in 1M HCl at various concentrations of extracts.

Compounds Concentrations

(g/l) Rct (ohm.cm2) fmax

(Hz) Cdl

(µF/cm2) E

(%) Blank 0 43.94 25 1.48 10-4 -

AE1

1 477.3 3,16 1.06 10-4 90 0.5 426.5 6,32 0.59 10-4 89 0.25 408 6,32 0.61 10-4 88 0.125 364.1 6,32 0.69 10-4 87

AE2

1 428.7 4 0.92 10-4 89 0.5 355 4 1.12.10-4 87 0.25 304.5 7.93 0.65 10-4 85 0.125 226.9 10 0.70 10-4 80

AE3

1 912.4 3.164 0.55 10-4 95 0.5 625.8 3.32 0.76 10-4 92 0.25 479.4 4 0.83 10-4 90 0.125 423 5 0.75 10-4 89

From Table 6 we noted the same order of the inhibition efficiency for the aqueous extracts using impedance spectroscopy: AE3 > AE1> AE2. It indicated the reproducibility of these results via the investigation of the inhibition phenomenon in the use of: weight loss, impedance and polarization methods.

CONCLUSION

The following conclusions summarize this study: • Zingiber Officinal Roscoe Extracts had a considerable inhibition effect on carbon steel corrosion in 1.0 M HCl solution. Inhibition efficiency increases with increasing concentrations; it follows the order AE3 > AE1> AE2 in all methods employed with small differences in their numerical values. • The polarization plots indicated that the inhibitor inhibits both anodic metal dissolution and cathodic hydrogen evolution reaction and acts as mixed type inhibitors. Impedance measurements indicate that with increasing inhibitor concentration, the transfer charge resistance (Rt) increases, while the double layer capacitance (Cdl) decreases. • The adsorption of this inhibitor on the carbon steel surface obeys the Langmuir adsorption isotherm. The thermodynamic activation parameters were calculated and discussed. • Inhibition efficiencies calculated using weight loss, impedance and polarization were in good agreement. Acknowledgments The publication cost of this paper was supported by the CNRST of Morocco.

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Zingiber Officinal Roscoe Extract Using as Green Corrosion inhibitor for Mild Steel in 1M HCl Media

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