Studies on the inhibition of carbon steel corrosion in hydrochloric acid solution by expired Carvedilol drug

ABSTRACT

An expired pharmaceutical product, Carvedilol, was studied as save drug to prevent carbon steel (CS) corrosion in acidic environments by using weight loss, potentiodynamic polarization, electrochemical impedance spectroscopy (EIS) and electrochemical frequency modulation (EFM) techniques. The inhibition efficiency increased with increasing drug dose and decreased with increasing temperature, reaching a maximum value of 98.94% at 25°C and 1.6 × 10⁻⁴ M. Polarization data showed that the drug is of a mixed type. The inhibition of CS corrosion by Carvedilol can be attributed to the adsorption ability of drug molecules onto the reactive sites of the metal surface. The adsorption process follows the Langmuir isotherm via physical adsorption. The surface morphologies of CS were examined by atomic force spectroscopy (AFM). The results obtained from different techniques are in good agreement.

GRAPHICAL ABSTRACT

KEYWORDS:

• Carvedilol drug
• corrosion
• CS
• hydrochloric acid
• adsorption
• AFM

1. Introduction

Carbon steel (CS) is the most worldwide used material for industrial and domestic applications, because of its good mechanical properties, availability and relatively reasonable cost. Hydrochloric acid is widely used in various technological processes in industry (in pickling baths, in the extraction and processing of oil and gas) and in other chemical and petrochemical industries. The corrosion behavior of CS in acidic media is an area of great interest due to its importance in applications. It has been found that one of the best methods of protecting metals against corrosion involves the use of synthetic organic compounds as corrosion inhibitors (1–3) which are substances that slow down the rate of corrosion (4,5). But many of these compounds unfortunately are highly toxic to both human beings and the environment (6). Due to the toxicity of some corrosion inhibitors, researches are concentrated toward the introduction of new, safe, non-toxic and environmentally benign natural products such as pharmaceutical compounds, leaves, fruits or seeds extracts, which can be used as corrosion inhibitors. Recently, several studies have been carried out on the use of drugs as potential candidate for the inhibition of metal corrosion because, through their functional groups, they form complexes with metal ions on metal surfaces. Antibiotics fall under the category of eco-friendly compounds and hence claimed as green correction inhibitors which are completely soluble in water and obtainable with high purity and relatively cheap. These properties would validate their use as corrosion inhibitors in various media. Likewise, the use of expired drugs as non-toxic corrosion inhibitors for CS and Al in acidic media was reported before (7–11). The use of expired drugs as corrosion inhibitors can be traced back to 2009's and 2011's when Abd El-Hameed (7) used expired ranitidine as corrosion inhibitor for carbon steel (8) and for mild steel (8) in HCl corrosive medium, respectively. The expired Carvedilol drug is big enough (molecular mass = 406.474, mol. formula = C₂₄H₂₆N₂O₄) and likely to effectively cover more surface area (due to adsorption) of the CS. Furthermore, Carvedilol drug is very cheap, easily available, environmentally friendly and non-toxic. Due to these properties, Carvedilol drug was chosen for the corrosion studies. The following table gives a comparison of %IE with different investigated drugs:

Table

Inhibitor (drug)	Sample	Medium	IE%	References
Pencillin G (15 × 10^−4M)	Mild steel	H2SO4	90.0	(12)
Penicillin V (15 × 10^−4M)	Mild steel	H2SO4	63.3	(13)
Cefalexin (11 × 10^−4M)	Mild steel	HCl	67.5	(14)
Ceftriaxone (400 ppm)	Mild steel	HCl	87,6	(15)
Cefotaxime (300 ppm)	Mild steel	HCl	90.0	(16)
Cefixime (8.8 × 10^−4M)	Mild steel	HCl	62.0	(17)
Ceftobiprole (9.31 × 10^−4M)	Mild steel	HCl	92.2	(18)
Norfloxacin (50 ppm)	Mild steel	HCl	22.3	(19)
Ciprofloxacin (50 ppm)	Mild steel	HCl	20.8	(19)
Pefloxacin (50 ppm)	Mild steel	HCl	15.1	(19)
Amifloxacin (50 ppm)	Mild steel	HCl	17.1	(19)
Enofloxacin (50 ppm)	Mild steel	HCl	18.3	(19)
Methocarbamol (2 × 10^−3 M)	Mild steel	HCl	67.1	(20)
Ranitidine (400 ppm)	Mild steel	HCl	90	(7)
Ranitidine (500 ppm)	Carbon steel	HCl	79	(8)

The main objective here is to investigate the corrosion process of CS in 1 M HCl solution in the absence and presence of different doses of expired Carvedilol drug and to test the various electrochemical studies towards the corrosion of CS. Also, our study was focused on the usage of expired drugs because most of the pharmaceutically active substances are more expensive than the organic inhibitors currently used. Also, the use of expired drugs will solve two problems: (a) economical which reduce the disposal costs of expired drugs and (b) environmental which limits the environmental pollution with pharmaceutically active compounds.

Carvedilol drug is the commercial name of ((±)-[3-(9H-carbazol-4-yloxy)-2-hydroxypropyl][2-(2-methoxyphenoxy)ethyl]amine) as shown in Figure 1.

Figure 1. Chemical structure of the Carvedilol drug.

2. Experimental methods

2.1. Material

The composition of the CS specimen (in weight %) is C 0.2, Mn 0.6, P 0.04, Si 0.003 and Fe rest.

2.2. Solutions

All solutions and reagents were prepared from analytical reagent-grade compounds in bi-distilled water. The aggressive solutions of 1 M HCl were prepared by dilution of analytical grade 37% HCl with bi-distilled water.

2.3. Inhibitor

Carvedilol drug was kindly supplied by Boehringer Mannheim GmbH. A stock solution of 2.5 × 10⁻² M Carvedilol was prepared by dissolving an accurate weight of the drug in ethanol and stored in the dark at 4°C. Dilute solutions of the drug were then prepared daily just before use in dark polyethylene bottles. The standard stock solutions were protected from light during the experimental procedures to prevent any possible degradation of the drug before use.

2.4. Weight loss measurements

Coupons cut into 2 × 2 × 0.2 cm dimensions are used for weight loss (WL) measurements. Prior to all measurements, the exposed area was mechanically abraded with 180, 320, 800 and 1200 grades of emery papers. The specimens were washed thoroughly with bi-distilled water, degreased and dried with ethanol. The solution volume is 100 mL, the immersion time for the WL is 30, 60, 90, 120 and 180 min at 25°C, 35°C, 45°C and 55°C. In order to get good reproducibility, parallel triplicate experiments were performed and the average WL value of three parallel CS sheets was obtained.

2.5. Electrochemical measurements

The electrochemical tests were conducted in a classical three-electrode cell with platinum as counter electrode, saturated calomel as the reference electrode, and CS specimen as the working electrode. Before starting the experiment, the working electrode with an area of 1 cm² was treated as in WL experiments and then immersed in a test solution for 30 min until a steady-state open circuit potential (OCP) was attained. The Stern-Geary method (21) used for the determination of corrosion current is performed by extrapolation of anodic and cathodic Tafel lines to a point which gives log i_corr and the corresponding corrosion potential (E_corr) for inhibitor free acid and for each dose of drug. All experiments were carried out three times for reproducibility and all measurements were conducted at 25°C.ll measurements were conducted at 25C

EIS was carried out at OCP in the frequency range 10⁵–10⁻¹ Hz, and the AC signal was 0.005 V in amplitude. EIS diagrams are given in the Nyquist and Bode representations.

PP was made by changing the electrode potential automatically from –800 to –200 mV versus OCP at a scan rate of 0.1 mV s⁻¹.

EFM were conducted using two frequencies of 0.2 and 0.5 Hz with amplitude of 20 mV RMS. EFM were conducted using two frequencies of 02 and 05 Hz with amplitude of 20 mV RMS The base frequency was 0.1 Hz, so the waveform repeats after 1 s. The higher frequency must be at least two times the lower one and must also be sufficiently slow that the charging of the double layer does not contribute to the current response. Often, 10 Hz is a reasonable limit. The large peaks were used to calculate the corrosion current density (i_corr), the Tafel slopes (β_a and β_c) and the causality factors CF-2 and CF-3 (22). The electrode potential was allowed to stabilize 30 min before starting the measurements.

All electrochemical experiments were carried out using Gamry instrument PCI300/4 Potentiostat/Galvanostat/Zra analyzer, DC105 Corrosion software, EIS300 software for EIS tests, EFM140 software for EFM tests and Echem Analyst 5.5 for results plotting, graphing, data fitting and calculating.

2.6. Surface analysis studies

Atomic force microscope (AFM) was used for surface morphology studies. The polished metal specimens were immersed in acid solutions in the absence and presence of 1.6 × 10⁻⁶ M drug. After a few hours, the specimens were taken out, washed with bi-distilled water and dried. The protective film was examined with AFM using Nano Surf Easyscan 2 Flex AFM instruments (Nanotechnology Center, Mansoura University). The topology of the studied samples for a scanned area of 4 or 8 μm is evaluated for a set point of 20 nN and a scan speed of 10 mm s⁻¹. The three dimensional topology of surface films gave various roughness parameters of the film, i.e. square mean value.

3. Results and discussion

3.1. WL measurements

The WL results of CS in 1 M HCl in the absence and presence of different doses of Carvedilol after 30, 60, 90, 120 and 180 min of hold time immersion at temperatures ranging of 25–55°C was studied and from the WL results, the %IE of the drug and θ were calculated using the following equation (23):(1) where W_inh and W_free are the WL for CS in the existence and nonexistence of the drug in HCl solution, respectively.

The data of Table 1 revealed that the values of the %IE increased with an increase in the Carvedilol doses. This behavior could be attributed to the increase in the CS surface area covered by the adsorbed molecules of Carvedilol with the increase in its dose which makes a barrier for mass transfer and prevents further corrosion. On the other hand, WL of CS decreases with an increase in Carvedilol doses, this means that Carvedilol acts as an inhibitor. The maximum %IE for Carvedilol 98.94% was achieved at 1.6 × 10⁻⁴ M at 25°C after immersion time 30 min.

Table 1. Variation of %IE with dose of Carvedilol in 1 M HCl solution at 25°C after immersion time 30 min.

Concentration (M)	Blank (1 M HCl)	1 × 10^−5	4 × 10^−5	8 × 10^−5	1.2 × 10^−4	1.6 × 10^−4
IE%	–	86.0	90.6	95.0	97.9	98.9
θ	–	0.860	0.906	0.950	0.979	0.989

In order to elucidate the influence of immersion time on the corrosion rate of CS, the data as shown in Figure 2 show the WL time plots for CS corrosion with and without different doses of the extract. The WL of CS increases with immersion time and by increasing the dose of Carvedilol, the WLs of CS samples are decreased indicating that Carvedilol is adsorbed on the CS surface in HCl (24).

Figure 2. WL - time plots for CS in 1 M HCl solution with and without different doses of Carvedilol at 25°C.

3.2. Effect of temperature on %IE

Temperature has a great effect on the corrosion phenomenon. The effect of temperature on the %IE of the Carvedilol drug was determined by the WL method as shown in Figure 4. The data in Table 2 revealed that the %IE decreased by increasing the temperature, this is due to increased rate of the dissolution process of CS and partial desorption of the drug from the metal surface with temperature (25). This indicates that the Carvedilol drug is physically adsorbed on the metal surface (26).

Table 2. The effect of temperature on the %IE of the Carvedilol drug.

Drug concentration (M)	%IE
	25°C	35°C	45°C	55°C
1.0 × 10^−5	86.0	82.4	73.9	67.2
4.0 × 10^−5	90.6	88.5	84.3	72.0
8.0 × 10^−5	95.0	92.4	87.4	84.7
1.2 × 10^−4	97.9	95.8	94.7	91.8
1.6 × 10^−4	98.9	97.6	96.7	95.7

3.3. Thermodynamic activation parameters of the corrosion process

Thermodynamic parameters are important and useful tool for clarifying the adsorption behavior of inhibitors. The thermodynamic parameters such as activation energy (), enthalpy () and entropy () of activation for the corrosion of CS in HCl solution were calculated. These parameters were computed with and without various doses of Carvedilol drug by applying Arrhenius equation (2) and transition-state equation (3) respectively (27):(2) (3) where CR is the corrosion rate, R is the universal gas constant, A is Arrhenius pre exponential factor, T is the absolute temperature, h is Planck’s constant and N is Avogadro’s number. Figure 3 shows the Arrhenius plot (log CR vs. 1/T). This plot gives straight lines and slope equal to /2.303R from which the values of for the inhibited corrosion reaction of CS have been calculated and recorded in Table 3. It was observed, for the HCl solution the has a value 28.87 kJ mol⁻¹ but in the presence of various doses of drug it had values from 52.89 to 65.73 kJ mol⁻¹ revealing the retardation of the corrosion reaction. This change in may be either precipitation in the electrode or may change the potential difference of the metal solution interface by adsorption. Figure 4 shows the transition-state plot (log CR/T vs. 1/T). This plot gives straight lines with a slope equal to –()/2.303R) and intercept (log R/2.303R + ()/2.303R), from which and values were calculated and listed in Table 3. The positive sign of reveals that the formation of the activated complex is endothermic. The negative values of indicate that the inhibitor molecules were adsorbed in an orderly manner onto the CS surface causing the entropy to decrease (28).

Figure 3. Arrhenius plots (log CR vs. 1000/T) for CS in 1 M HCl with and without different doses of Carvedilol drug.

Figure 4. Arrhenius plots (log CR/T vs. 1000/T) for carbon steel in 1 M HCl with and without different doses of Carvedilol drug.

Table 3. Activation parameters for dissolution of CS in absence and presence of different doses of Carvedilol drug in 1 M HCl.

Concentration (M)	(J mol^−1K^−1)	(kJ mol^−1)	(kJ mol^−1)	–
Blank 1 M HCl	185.99	26.29	28.87	2.58
1.0 × 10^−5	121.99	50.30	52.89	2.59
4.0 × 10^−5	108.80	55.40	57.93	2.53
8.0 × 10^−5	105.50	57.63	60.26	2.63
1.2 × 10^−4	100.95	60.97	63.59	2.62
1.6 × 10^−4	99.25	63.04	65.73	2.69

3.4. Adsorption consideration

The adsorption isotherm is necessary in studying the mechanism of adsorption. In order to gain more information about the mode of adsorption (physisorption, chemisorption or comprehensive adsorption) of the drug on the surface of CS, the experimental data have been tested with several adsorption isotherms (Langmuir, Freundlich, Temkin, kinetic-thermodynamic model and Flory–Huggins isotherm). A very good fit is observed with a regression coefficient (R² = 0.9994) for the Langmuir adsorption isotherm which confirms the validity of this approach (29). The Langmuir adsorption isotherm is based on the view that every adsorption site is identical and energetically equivalent (30). The Langmuir isotherm is expressed as in the following equation:(4) where K_ads is the adsorption equilibrium constant. Figure 5 shows the Langmuir adsorption isotherm for Carvedilol drug on the CS surface. The data derived from this isotherm are recorded in Table 4. The slight deviation of the slopes from unity is attributed to the molecular interaction among the adsorbed drug species, a factor which was not taken into consideration during the derivation of the Langmuir equation.

Figure 5. Langmuir adsorption isotherm plotted as C/Θ vs. C of Carvedilol drug for the corrosion of CS in 1 M HCl at 25°C.

Table 4. Equilibrium constant (K_ads) and standard free energy () of adsorption of the drug on CS in 1 M HCl at different temperatures.

Temp (°C)	Slope	(kJ mol^−1)	Kad × 10^4 (M^−1)	Intercept
25		41.3	30.87
35	3.753× 10^−5	42.2	25.36	12.87 × 10^−5
45		42.3	15.55
55		42.1	9.12

The standard free energy of adsorption (ΔG°_ads) was calculated by the following equation (31):(5) where 55.5 is the molar dose of water in the solution in mol L⁻¹. The negative value of indicates the stability of the adsorbed layer on the CS surface (32). It is well known that values up to −20 kJ mol⁻¹ are consistent with the electrostatic interaction between the charged molecules and the charged metal (physical adsorption) while those more negative than −40 kJ mol⁻¹ involve sharing or transfer of electron from the drug molecule to the metal surface to form a coordinate bond (chemisorption) (33). The values of obtained are in the range of −40 kJ mol⁻¹ indicating that the adsorption of Carvedilol on the CS surface in 1 M HCl solutions was of mixed type (chemisorption and physisorption).

3.5. Tafel polarization measurements

Figure 6 demonstrates the Tafel polarization curves for CS in 1 M HCl with and without the addition of different doses of the expired drug at 25°C. The obtained kinetic parameters such as corrosion current density (i_corr), cathodic Tafel slope (b_c), anodic Tafel slope (b_a), corrosion potential (E_corr) and %IE found from these curves are given in Table 5. The data in Table 5 revealed that i_corr decreased in the presence of drug while %IE increased. Also, it is noticed that b_a and b_c were not affected and the Tafel lines are parallel, denoting that the inhibiting effect of this drug has arisen by merely blocking of the available surface area via adsorption, i.e. the tested drug reduced the anodic dissolution and hydrogen evolution without changing the reaction mechanism (34). The shift of the E_corr values is not more than 85 mV (34 mV); hence, the studied drug may be classified as a mixed-type inhibitor.

Figure 6. Potentiodynamic anodic and cathodic polarization curves recorded for CS in 1 M HCl solutions without and with various doses of Carvedilol at 25°C.

Table 5. Electrochemical parameters obtained from polarization curves for CS in 1 M HCl without and with various doses of Carvedilol at 25°C.

Concentration (M)	–Ecorr (mV)	icorr (mA cm^−2)	%IE	CR (mm Y^−1)	ba (mV dec^−1)	–bc (mV dec^−1)
Blank	320.4	1.87	–	21.90	74.6	227.1
4.0 × 10^−5	295.1	0.15	92.1	1.74	38.3	163.3
8.0 × 10^−5	302.7	0.11	94.2	1.26	41.3	105.7
1.2 × 10^−4	286.4	0.07	96.3	0.81	31.2	70.4
1.6 × 10^−4	289.6	0.03	98.1	0.41	29.8	62.3

3.6. EIS measurements

The experimental results obtained from EIS measurements for the corrosion of CS in the presence of Carvedilol drug in 1 M HCl at room temperature are summarized in Table 6. Figure 7 displays the Nyquist (a) and Bode (b) plots for CS in 1 M HCl in the absence and presence of various doses of expired Carvedilol drug. Clearly, the impedance spectra exhibit a single semicircle. The semicircle indicates that the corrosion of CS in 1 M HCl is mainly controlled by a charge transfer process (35) and usually related to the charge transfer of the corrosion process and double-layer behavior. The diameter of the capacitive loop in the presence of the drug is bigger than in the absence of the drug (blank solution) and increases with inhibitor dose. This indicates that the impedance of inhibited substrate increases with the inhibitor dose. Noticeably, these impedance spectra are not perfect semicircles which can be attributed to the frequency dispersion effect. This anomalous behavior is generally attributed to the roughness and inhomogeneity of the metal surface (36). The impedance spectra exhibit a single semicircle corresponding to one time constant in the Bode plots (Figure 7(b)). It can be concluded that the charge transfer resistance R_ct value increased with increase in the dose of the drug, whereas the values of double-layer capacitance (C_dl) decreased, with an increase in the inhibitor dose, which is most probably due to the decrease in the local dielectric constant and/or increase in the thickness of the electrical double layer (37). The equivalent circuit model shown in Figure 8 was used to analyze the Nyquist curves and it consists of R_s and CPE (constant-phase element) parallel to the R_ct.

Figure 7. Nyquist (a) and Bode (b) plots for CS corrosion in 1 M HCl solution with and without different doses of Carvedilol at 25°C.

Figure 8. Equivalent circuit model used to fit experimental EIS data.

Table 6. Impedance parameters and inhibition efficiency for CS corrosion in1.0 M HCl solution in the absence and presence of different doses of expired Carvedilol drug at 25°C.

Concentration (M)	Rct (ohm cm^2)	Cdl (μF cm^−2)	Θ	%IE
Blank	3.069	55.81	–	–
1.0 × 10^−5	22.27	13.81	0.862	86.2
4.0 × 10^−5	36.14	8.92	0.915	91.5
8.0 × 10^−5	58.93	6.16	0.948	94.8
1.2 × 10^−4	111.23	4.47	0.972	97.2
1.6 × 10^−4	222.9	2.61	0.986	98.6

3.7. EFM method

The EFM is a non-destructive corrosion measurement technique that can directly give values of the corrosion current without prior knowledge of Tafel constants (37). Figure 9(a,b) shows the EFM spectrum obtained for CS corrosion in 1 M HCl solution in the absence and presence of 1 × 10⁻⁴ M of the investigated Carvedilol at 25°C, respectively. The larger peaks were used to calculate the corrosion current. Each spectrum is a current response as a function of frequency. Table 7 shows the corrosion kinetic parameters such as inhibition efficiency (%IE), corrosion current density i_corr, Tafel constants (b_a, b_c) and causality factors (CF-2, CF-3) as a function of drug dose in the absence and presence of the expired Carvedilol drug. It is obvious from Table 7 that corrosion current density (i_corr) values decrease, while those of inhibition efficiency (%IE) increase with an increase in Carvedilol drug dose. The great strength of the EFM is the causality factor, which serves as an internal check on the validity of the EFM measurement (38). The standard values for CF-2 and CF-3 are 2.0 and 3.0, respectively. The deviation of causality factors from their ideal values might be due to that the perturbation amplitude was too small or that the resolution of the frequency spectrum is not high enough. The results obtained from EFM showed good agreement with those obtained from WL, polarization and EIS methods.

Figure 9. EFM recorded for CS corrosion in 1 M HCl solution (a) in the absence and (b) in the presence of 1.6 × 10⁻⁴ M expired Carvedilol drug at 25°C.

Table 7. EFM spectra of CS corrosion in 1 M HCl solution with and without different doses of Carvedilol at 25°C.

Concentration (M)	icorr (μA cm^−2)	ba (mV dec^−1)	–bc (mV dec^−1)	CR, mpy	CF2	CF3	%IE
Blank	296.40	92	117	648.8	2.02	2.93	–
1.0 × 10^−5	40.99	93	135	89.71	1.95	2.81	86.2
4.0 × 10^−5	25.33	92	137	55.47	2.00	3.24	91.5
8.0 × 10^−5	17.98	103	171	39.35	1.92	3.54	93.9
1.2 × 10^−4	10.72	98	154	23.50	2.04	3.15	96.4
1.6 × 10^−4	5.76	68	148	12.56	2.13	2.80	98.1

3.8. Surface studies (AFM characterization)

AFM is a powerful technique to investigate the surface morphology at nano-to-micro-scale and has become a new choice to study the influence of the inhibitor on the generation and the progress of the corrosion at the metal/solution interface (39,40). Analysis of the images allowed quantification of surface roughness over an area scale of 8 μm. The 3D AFM images of CS surface without and with inhibitor are shown in Figure 10(a–c). The surface roughness of the CS surface in 1 M HCl is up to 392.6 nm while in the presence of drug (Figure 10(b)), the roughness decreases to 75.9 nm (Figure 10(c)). It shows that the CS surface in the presence of the drug is more compact and uniform compared with Figure 10(a,b); so it can efficiently protect the CS surface from corrosion. Also, AFM images give the root-mean-square roughness and maximum peak to peak height values. Table 8 confirms that the height values are less in the inhibited solution compared with the uninhibited one. These parameters confirm that the inhibited surface is smoother than the uninhibited one. This is due to the formation of a protective film on the metal surface.

Figure 10. AFM 3D images of CS (a) free specimen (b) in 1 M HCl for 12 h (c) in 1 M HCl containing 1.6 × 10⁻⁴ M for 12 h expired Carvedilol drug at 25°C.

Table 8. AFM parameters for CS: (a) free specimen (b) in 1 M HCl for 12 h (c) in 1 M HCl containing 1.6 × 10⁻⁴ M expired Carvedilol drug at 25°C for 12 h immersion.

Parameters	a	b	c
The roughness average (Sa) in nm	14.1	392.6	75.9
The mean value (Sm) in nm	−18.0	−17.3	−17.6
The root-mean-square (Sq) in nm	18.1	493.2	96.1
The valley depth (Sv) in nm	−58.3	−3141.9	−345.1
The peak height (Sp) in nm	40.8	1557.9	447.5
The peak-valley height (Sy) in nm	99.1	4699.8	801.6

3.9. Mechanism of inhibition

It is generally assumed that the adsorption of the drugs at the metal/solution interface is the first step in the mechanism of inhibition in aggressive media. Also, it is accepted that the first step during the adsorption of an organic drug on a metal surface usually involves replacement of one or more water molecules absorbed at the metal surface (41,42). The adsorption is influenced by the nature and charge of the metal, chemical structure of inhibitor and type of aggressive electrolyte. The inhibitory action of Carvedilol drug may be due to the following mechanism; in acidic solutions, this compound could be protonated easily in the HCl solution, . The CS surface aquires positive charge (43,44). Accordingly, chloride ions are first adsorbed on the CS surface and consequently the CS surface becomes negatively charged, then the protonated molecules get adsorbed. Both molecular and protonated species can adsorb on the CS surface. The high %IE may be due to the larger molecular size of the drug which covers large areas from the CS surface.

4. Conclusions

The expired Carvedilol drug acts as good and efficient corrosion inhibitor for the corrosion of CS in 1 M HCl solution. The IE decreases with rise in temperature, but increases with an increase in the dose of the drug. The inhibition of CS corrosion by Carvedilol can be attributed to the adsorption ability of drug molecules onto the reactive sites of the metal surface. The adsorption of the drug on CS obeys the Langmuir adsorption isotherm. Polarization data indicate that the drug acts as a mixed-type inhibitor. AFM reveals the formation of a smooth uniform surface on CS in the presence of the drug which indicates the formation of a good protective layer on the metal surface. The results obtained from different measurements gave consistent results.

Disclosure statement

No potential conflict of interest was reported by the authors.

Notes on contributors

A.S. Fouda received his B.Sc. Chemistry, Cairo University, Egypt, 1972, M.Sc. in Physical and Inorganic Chemistry, from El-Mansoura University, Egypt, 1975 and Ph.D. in Physical Chemistry, El- Mansoura University, Egypt, 1979, 1988, Prof. of Physical Chemistry, B.Sc. in Chemistry 2013. He is a member of Egyptian corrosion Bulletin, Member of the editorial many Journals. He granted the Chemical Engineering Department and Material Science, Minnesota University, USA 1982–1983 and Institute, Bonn University Germany 1989. He had prizes from National Award for Chemistry from Academy of Scientific Research and Technology in Cairo, 1982, first class State Medal of Sciences and Arts, 1984 and Prize of El-Nasr Company for Fertilizers, Talkha, 1981. He is an international reviewer for a huge number of thesis, journals and projects. He had published more than 200 papers in international journals. His main research interests are in the field of Physical Chemistry, Especially electrochemistry (Corrosion and corrosion inhibition in all media for metals and alloys, Fuel cells, Electrode position of metals and oxides).

Dr. M.A. El Morsi got his B.Sc. in Chemistry 1973, M.Sc. in physical Chemistry 1977, Ph.D. in physical chemistry 1981. He pointed as lecturer in Tanta University 1981 to 1987, and as associate professor at Tanta University from 1987 to 1999 and full professor from 1999 till now. He published several papers in electrochemistry in international journals.

T. El Mogy is a student studying Ph.D. He got his B.Sc. 2000 and his M.Sc. 2013 in Electroanalytical chemistry, he registered in Ph.D. degree since 2013 in physical chemistry until now.