# Experimental and Theoretical Studies on the Corrosion Inhibition of Brass in Hydrochloric Acid by N-(4-((4-Benzhydryl Piperazin-1-yl) Methyl Carbamoyl) Phenyl) Furan-2-Carboxamide

Authors: N. Zulfareen; T. Venugopal; K. Kannan
Journal: International Journal of Corrosion
 (2018)

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## Abstract

The corrosion inhibition effect of N-(4-((4-Benzhydryl piperazin-1-yl) methyl Carbamoyl) Phenyl) Furan-2-Carboxamide (BFC) on brass in 1M HCl has been investigated using weight loss method, potentiodynamic polarization, electrochemical impedance spectroscopy (EIS), and cyclic voltammetry (CV). The result reveals that BFC acts as a mixed type corrosion inhibitor with more pronounced effect on anodic domain and the inhibition efficiency of BFC increases with increase in temperature ranges from 30°C to 60°C. AC impedance implies thatRct value of BFC increases with increase in concentration. CV indicates that the addition of inhibitor controls the oxidation of the copper on the brass metal. The structural confirmation of BFC was carried out by the spectral studies like FT-IR, 1H NMR, 13C NMR, and the molecular weight was confirmed by LC-MS. Surface characterization of brass with BFC was analysed using scanning electron microscope (SEM). Quantum chemical parameter was used to calculate the electronic properties of BFC in order to confirm the correlation between the inhibitor effect and molecular structure of BFC. BFC has more negative charge on nitrogen and oxygen atom, which facilitates the adsorption of BFC on the surface of brass.


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## Body

## 1. Introduction

Copper and its alloys are one of the most important nonferrous materials having a wide range of applications in industries due to its electrical conductivity, thermal conductivity, ease of fabrication, resistance to biofouling, and mechanical properties. Copper and copper based resources are intentionally or unintentionally exposed to acid solutions. However copper and its alloys are corrosion resistance towards the atmosphere and many chemicals due to the formation of cuprous oxide layer, when exposed to the atmosphere. They are susceptible to corrosion problems in acid medium such as dezincification and pitting corrosion [1].The most important method for corrosion protection is by the addition of organic inhibitors on the brass. Many of the inhibitors are organic compounds containing nitrogen, oxygen, sulphur, Phosphorous, and aromatic rings that cause adsorption on the metal surface [2]. Nowadays the synthesized Mannich base compounds have been of interest in order to obtain efficient corrosion inhibitors since they provide much greater inhibition efficiency compared to corresponding amines and aldehydes. The presence of C=N group in Mannich base enhances the adsorption ability and inhibition efficiency.The present work reports on the anticorrosive behaviour of a Mannich base namely N-(4-((4-Benzhydrylpiperazin-1-yl) methyl Carbamoyl) Phenyl) Furan-2-Carboxamide (BFC) for brass in hydrochloric acid solution. The kinetics of dissolution and dezincification mechanism of brass in hydrochloric acid solution was investigated using electrochemical studies. For this purpose electrochemical technique such as potentiodynamic polarization, electrochemical impedance spectroscopy (EIS) and cyclic voltammetry in the presence and absence of BFC were studied [3].It is also aimed to study the quantum chemical parameters and thermodynamic feasibility of the inhibitor using the surface coverage of brass. The interaction of inhibitor (BFC) was correlated with coefficient of their molecular orbitals highest occupied molecular orbital (HOMO), lowest unoccupied molecular orbital (LUMO), energy difference (ΔE) betweenEHOMO and ELUMO, atomic charges, and dipole moments. The coordination of ligand to the surface of metal was confirmed by FT-IR. The characterization of BFC was further confirmed by NMR and LC-MS.


## 2. Experiment

### 2.1. Synthesis of CFC

N-(4-Carbamoylphenyl)Furan-2-Carboxamide (CFC) was prepared by a procedure similar to that reported in the literature; 4-Amino benzamide (3.00g, 0.0220 mol) and 2-furoyl chloride (3.428 g, 0.0264 mol) were dissolved in mixture of MDC (70 ml) and THF (25 ml). Triethylamine (7.77g) was added, and the mixture was stirred in the presence of nitrogen atmosphere for 24 hours. The reaction mixture was washed with water, filtered, and dried over high vacuum pump. The CFC was characterized by spectral techniques like FT-IR, NMR, and LC-MS. Figure1 represents the synthesis of CFC.Figure 1
Synthesis of CFC.


### 2.2. Characterization of CFC

Yeild 93%, white solid, m.p.186-190°C., IR (KBr,νmax cm−1; 3387, 3179(NH, St, Amide), 1658 (C=O), 1617 (NH, Bend, Amide), 1400 (CN, Amide), 1474, 1527 (C=C), 1179 (C-O, furan), 841 (CH, Ar,oop). 1H NMR (400 MHz, DMSO-d6) d(ppm): 6.71(1H, Furan), 7.36 (1H, furan), 7.80-7.84 (4H), 7.85-7.87 (2H, Amide), 7.95 (1H, furan), 10.36 (1H, Amide). 13C NMR (400 MHz, DMSO-d6) d(ppm): δ 112.1, 115.0, 119.2, 128.1, 129.1, 141.1, 145.0, 147.2, 156.2(C=O), 167.3 (C=O). MS (EI): m/z (%) = 231.02 Figures 2(a), 2(b), 2(c), and 2(d) represent the FT-IR, 13C, 1H, and LC-MS of CFC respectively.Figure 2 (a)
FT-IR spectrum of CFC (b)
13C spectrum of CFC (c)
1H spectrum of CFC (d)
LC-MS spectrum of CFC


### 2.3. Synthesis of BFC

The mixture of CFC (0.0130 mol, 3 g), benzhydryl piperazine (0.0130 mol, 1.1363 g), and formaldehyde (0.01956 mol, 0.587 g) were dissolved in ethanol.The reaction mixture was refluxed for 48 hrs at 90°C. The white solid obtained was filtered, washed with cold ethanol, and followed by petroleum ether. The resulting mass is dried and recrystallized from ethanol [4]. The BFC was characterized by spectral techniques like FT-IR, NMR, and LC-MS. Figure 3 represents the synthesis of BFC.Figure 3
Synthesis of BFC.


### 2.4. Characterization of BFC

Yield 90%, white solid, m.p.190-198°C., IR (KBr,νmax cm−1; 3265 (NH), 3058, 3029 (CH, Ar), 2942, 2808, 2757, 2698 (CH, Aliph), 1663 (C=O), 1591 (NH, bend), 1534, 1472 (C=C), 1335 (C-N, amide), 1188 (C-O, furan) 1138 (C-O), 1027 (C-N, Amine), 841 (CH, Ar, oop). 1H NMR (300 MHz, CDCl3) d(ppm): 2.46 (4H), 2.71 (4H), 4.24 (s, 1H), 4.35 (d, 2H, J=6 HZ), 6.59-6.63(m, 2H), 7.15-7.20 (m, 2H), 7.24-7.31 (m, 5H), 7.43(d, 4H, J=8.4 HZ), 7.55-7.56(m, 1H), 7.77 (d,2H, J=8.7 HZ), 7.85 (d, 2H, J=8.7 HZ), 8.23 (s, 1H). 13C NMR (300 MHz, CDCl3) d(ppm): δ MS (EI): m/z (%) = 494.44. Figures 4(a), 4(b), 4(c), and 4(d) represent the FT-IR, 13C, 1H, and LC-MS of CFC, respectively.Figure 4 (a)
FT-IR spectrum of BFC (b)
13C spectrum of BFC (c)
1H spectrum of BFC (d)
LC-MS spectrum of BFC


### 2.5. Medium

The standard solution of 1M hydrochloric acid was prepared using double distilled water. The concentration of the inhibitor BFC ranges from 0.20 mM to 1.61 mM in 1M hydrochloric acid. All the solutions were prepared in double distilled water.


### 2.6. Brass Sample

The chemical composition of working electrode, brass electrode [Cu (60.66%), Zn (36.58%), Sn (1.02%), and Fe (1.74%) was used in rectangular form having dimension of 3.0 cm length and width 0.2 cm thickness with an exposed area of 7.6 cm2 for weight loss method. The specimen was mechanically ground with 320, 400, 600, 800, 1000, and 1200 emery paper, washed in acetone and bi-distilled water, then dried, and placed in a cell.


### 2.7. NMR Analysis

NMR and13C NMR spectrum of the Mannich bases BFC were recorded on a Bruker AC 300 F (300 and 400 MHz) NMR spectrometer using CDCl3, DMSO as solvents, and TMS as an internal standard.


### 2.8. Weight Loss Measurements

Weight loss experiments were carried out according to the method described previously [5]. Weight loss measurements were performed by immersing the brass coupons in 100 ml of 1M HCl solution with and without various amounts of inhibitor for 2 hours by varying the temperatures range from 30°C to 60°C. After the elapsed time, the specimens were taken out, washed, dried, and weighed accurately. Triplicate test was performed for both blank and inhibitor and the average values were reported with standard deviation. The inhibition efficiency (IE) and surface coverage (θ) was determined by the following:(1)I.Eorη%=W0-W1W0×100(2)θ=W0-W1W0where W1 and W0 are the weight loss values in the presence and absence of inhibitor.


### 2.9. Electrochemical Measurement

A three-electrode system consisting of brass coupons of 1.0 cm2 area exposed as working electrode (WE), platinum sheet as a counterelectrode (CE), and saturated calomel electrode (SCE) as a reference electrode was used for electrochemical measurements. The entire test was performed in atmospheric condition without stirring. Experiments were carried out in Electrochemical Workstation Model 608 D/E Series in 1M HCl in the presence and absence of inhibitor. Prior to the electrochemical measurements, a stabilization period of 30 minutes was allowed, which is enough to attain stable Ecorr value. Potentiodynamic polarization measurement was performed with the potential range of ±200 mV and the scan rate is 1.0 mV s−1. The inhibition efficiency (IE) and corrosion rate (CR) were calculated by using the following:(3)I.Eorη%=1–i′corricorr×100(4)CRmmpy=3270×M×icorrρ×Zwherei′corr and icorr are the corrosion current density of brass in the absence and presence of BFC. M is atomic mass of metal, ρ is density of corroding metal, and Z is number of electrons transferred per metal atom (Z=2) [6].After polarization measurements electrochemical impedance was carried out by varying the frequency from 100 MHz to 100 KHz [7]. The following equation is used to calculate inhibition efficiency (η %) and double layer capacitance (Cdl) of BFC was calculated by(5)η%=Rict 1-R0ct 1Rict 1(6)Cdl=12×3.14×fmax×RctwhereR0ct 1 and Rict 1 are charge transfer resistance in the absence and presence of BFC, fmax is the frequency, and Rct are the charge transfer resistance.


### 2.10. DFT Study

Quantum chemical calculations were performed using DFT method, and the structural parameters were geometrically optimized using functional hybrid RB3LYP with electron basis set 6-311G (d,p) for the atoms. All the calculations were performed with Gaussian 09. The quantum chemical parameters likeEHOMO, ELUMO, energy gap (ΔE= ELUMO - EHOMO), dipole moment (μ), absolute electronegativity (χ), global hardness (η), global softness (σ), and Mulliken charge were calculated.


## 2.1. Synthesis of CFC

N-(4-Carbamoylphenyl)Furan-2-Carboxamide (CFC) was prepared by a procedure similar to that reported in the literature; 4-Amino benzamide (3.00g, 0.0220 mol) and 2-furoyl chloride (3.428 g, 0.0264 mol) were dissolved in mixture of MDC (70 ml) and THF (25 ml). Triethylamine (7.77g) was added, and the mixture was stirred in the presence of nitrogen atmosphere for 24 hours. The reaction mixture was washed with water, filtered, and dried over high vacuum pump. The CFC was characterized by spectral techniques like FT-IR, NMR, and LC-MS. Figure1 represents the synthesis of CFC.Figure 1
Synthesis of CFC.


## 2.2. Characterization of CFC

Yeild 93%, white solid, m.p.186-190°C., IR (KBr,νmax cm−1; 3387, 3179(NH, St, Amide), 1658 (C=O), 1617 (NH, Bend, Amide), 1400 (CN, Amide), 1474, 1527 (C=C), 1179 (C-O, furan), 841 (CH, Ar,oop). 1H NMR (400 MHz, DMSO-d6) d(ppm): 6.71(1H, Furan), 7.36 (1H, furan), 7.80-7.84 (4H), 7.85-7.87 (2H, Amide), 7.95 (1H, furan), 10.36 (1H, Amide). 13C NMR (400 MHz, DMSO-d6) d(ppm): δ 112.1, 115.0, 119.2, 128.1, 129.1, 141.1, 145.0, 147.2, 156.2(C=O), 167.3 (C=O). MS (EI): m/z (%) = 231.02 Figures 2(a), 2(b), 2(c), and 2(d) represent the FT-IR, 13C, 1H, and LC-MS of CFC respectively.Figure 2 (a)
FT-IR spectrum of CFC (b)
13C spectrum of CFC (c)
1H spectrum of CFC (d)
LC-MS spectrum of CFC


## 2.3. Synthesis of BFC

The mixture of CFC (0.0130 mol, 3 g), benzhydryl piperazine (0.0130 mol, 1.1363 g), and formaldehyde (0.01956 mol, 0.587 g) were dissolved in ethanol.The reaction mixture was refluxed for 48 hrs at 90°C. The white solid obtained was filtered, washed with cold ethanol, and followed by petroleum ether. The resulting mass is dried and recrystallized from ethanol [4]. The BFC was characterized by spectral techniques like FT-IR, NMR, and LC-MS. Figure 3 represents the synthesis of BFC.Figure 3
Synthesis of BFC.


## 2.4. Characterization of BFC

Yield 90%, white solid, m.p.190-198°C., IR (KBr,νmax cm−1; 3265 (NH), 3058, 3029 (CH, Ar), 2942, 2808, 2757, 2698 (CH, Aliph), 1663 (C=O), 1591 (NH, bend), 1534, 1472 (C=C), 1335 (C-N, amide), 1188 (C-O, furan) 1138 (C-O), 1027 (C-N, Amine), 841 (CH, Ar, oop). 1H NMR (300 MHz, CDCl3) d(ppm): 2.46 (4H), 2.71 (4H), 4.24 (s, 1H), 4.35 (d, 2H, J=6 HZ), 6.59-6.63(m, 2H), 7.15-7.20 (m, 2H), 7.24-7.31 (m, 5H), 7.43(d, 4H, J=8.4 HZ), 7.55-7.56(m, 1H), 7.77 (d,2H, J=8.7 HZ), 7.85 (d, 2H, J=8.7 HZ), 8.23 (s, 1H). 13C NMR (300 MHz, CDCl3) d(ppm): δ MS (EI): m/z (%) = 494.44. Figures 4(a), 4(b), 4(c), and 4(d) represent the FT-IR, 13C, 1H, and LC-MS of CFC, respectively.Figure 4 (a)
FT-IR spectrum of BFC (b)
13C spectrum of BFC (c)
1H spectrum of BFC (d)
LC-MS spectrum of BFC


## 2.5. Medium

The standard solution of 1M hydrochloric acid was prepared using double distilled water. The concentration of the inhibitor BFC ranges from 0.20 mM to 1.61 mM in 1M hydrochloric acid. All the solutions were prepared in double distilled water.


## 2.6. Brass Sample

The chemical composition of working electrode, brass electrode [Cu (60.66%), Zn (36.58%), Sn (1.02%), and Fe (1.74%) was used in rectangular form having dimension of 3.0 cm length and width 0.2 cm thickness with an exposed area of 7.6 cm2 for weight loss method. The specimen was mechanically ground with 320, 400, 600, 800, 1000, and 1200 emery paper, washed in acetone and bi-distilled water, then dried, and placed in a cell.


## 2.7. NMR Analysis

NMR and13C NMR spectrum of the Mannich bases BFC were recorded on a Bruker AC 300 F (300 and 400 MHz) NMR spectrometer using CDCl3, DMSO as solvents, and TMS as an internal standard.


## 2.8. Weight Loss Measurements

Weight loss experiments were carried out according to the method described previously [5]. Weight loss measurements were performed by immersing the brass coupons in 100 ml of 1M HCl solution with and without various amounts of inhibitor for 2 hours by varying the temperatures range from 30°C to 60°C. After the elapsed time, the specimens were taken out, washed, dried, and weighed accurately. Triplicate test was performed for both blank and inhibitor and the average values were reported with standard deviation. The inhibition efficiency (IE) and surface coverage (θ) was determined by the following:(1)I.Eorη%=W0-W1W0×100(2)θ=W0-W1W0where W1 and W0 are the weight loss values in the presence and absence of inhibitor.


## 2.9. Electrochemical Measurement

A three-electrode system consisting of brass coupons of 1.0 cm2 area exposed as working electrode (WE), platinum sheet as a counterelectrode (CE), and saturated calomel electrode (SCE) as a reference electrode was used for electrochemical measurements. The entire test was performed in atmospheric condition without stirring. Experiments were carried out in Electrochemical Workstation Model 608 D/E Series in 1M HCl in the presence and absence of inhibitor. Prior to the electrochemical measurements, a stabilization period of 30 minutes was allowed, which is enough to attain stable Ecorr value. Potentiodynamic polarization measurement was performed with the potential range of ±200 mV and the scan rate is 1.0 mV s−1. The inhibition efficiency (IE) and corrosion rate (CR) were calculated by using the following:(3)I.Eorη%=1–i′corricorr×100(4)CRmmpy=3270×M×icorrρ×Zwherei′corr and icorr are the corrosion current density of brass in the absence and presence of BFC. M is atomic mass of metal, ρ is density of corroding metal, and Z is number of electrons transferred per metal atom (Z=2) [6].After polarization measurements electrochemical impedance was carried out by varying the frequency from 100 MHz to 100 KHz [7]. The following equation is used to calculate inhibition efficiency (η %) and double layer capacitance (Cdl) of BFC was calculated by(5)η%=Rict 1-R0ct 1Rict 1(6)Cdl=12×3.14×fmax×RctwhereR0ct 1 and Rict 1 are charge transfer resistance in the absence and presence of BFC, fmax is the frequency, and Rct are the charge transfer resistance.


## 2.10. DFT Study

Quantum chemical calculations were performed using DFT method, and the structural parameters were geometrically optimized using functional hybrid RB3LYP with electron basis set 6-311G (d,p) for the atoms. All the calculations were performed with Gaussian 09. The quantum chemical parameters likeEHOMO, ELUMO, energy gap (ΔE= ELUMO - EHOMO), dipole moment (μ), absolute electronegativity (χ), global hardness (η), global softness (σ), and Mulliken charge were calculated.


## 3. Results and Discussion

### 3.1. Weight Loss Method

Table1 indicates the effect of concentration of BFC on the corrosion of brass in 1M HCl. From the table the inhibition efficiency (IE) of BFC increases with an increase in the concentration of inhibitor and temperature [8]. The maximum inhibition efficiency obtained by this method was found to be 77.37 % at a concentration of 1.41 mM and further increase in the concentration and temperature of inhibitor (1.61 to 2.01 mM, 60°C) did not cause any appreciable change in the efficiency of BFC. This is due to the surface blocking effect of inhibitor on the metal by adsorption and film formation mechanism and also due to the presence of protonated nitrogen and the oxygen atom of BFC. The presence of nitrogen and oxygen atom present in BFC absorbs quickly on the metal surface with formation of an insoluble stable film; this makes the inhibitor more effective.Table 1
Weight loss measurements of brass in IM HCl with BFC from 30°C to 60°C.
S.No. Temp. (°C) Con. of inhibitor (mM) Corrosion rate (mmpy) Surface coverage(θ) Inhibition efficiency (I.E)% 1 30°C Blank 35.781 - -  0.20 15.742 0.4278 42.78  0.40 13.552 0.4566 45.66  0.60 9.840 0.4610 46.10  0.80 7.174 0.5052 50.52  1.01 6.711 0.5676 56.76  1.21 5.061 0.6018 60.18  1.41 4.770 0.6149 61.49  2 40°C Blank 65.517 - -  0.20 18.731 0.4681 46.81  0.40 16.874 0.4707 47.07  0.60 15.364 0.4935 49.35  0.80 12.809 0.5309 53.09  1.01 9.781 0.5866 58.66  1.21 6.846 0.6211 62.11  1.41 5.224 0.6324 63.24  3 50°C Blank 98.182 - -  0.20 50.175 0.4920 49.20  0.40 48.011 0.5013 50.13  0.60 43.521 0.5367 53.67  0.80 37.540 0.5671 56.71  1.01 35.839 0.5930 59.30  1.21 29.743 0.6388 63.88  1.41 22.585 0.6500 65.00  4 60°C Blank 468.822 - -  0.20 62.743 0.5486 54.86  0.40 58.770 0.5637 56.37  0.60 50.982 0.6053 60.53  0.80 46.418 0.6652 66.50  1.01 44.730 0.7192 71.92  1.21 36.641 0.7632 76.32  1.41 30.150 0.7737 77.37


### 3.2. Tafel Polarization Measurements

Figures5(a), 5(b), 5(c), and 5(d) indicate the potentiodynamic polarization curves for the brass electrode in 1M HCl solution with and without different concentrations of BFC at 60°C, 50°C, 40°C, and 30°C. It was clear that the current density decreases with the presence of BFC which indicates that inhibitor is adsorbed on the surface of metal. The values of corrosion potential (Ecorr) and corrosion current density (icorr) are obtained by Tafel extrapolation method, anodic (ba) and cathodic (bc) These polarization curves indicate that there is a clear reduction of both anodic and cathodic currents in the presence of BFC compared with Blank solution.Figure 5 (a)
Potentiodynamic polarization curves of BFC for brass in 1M HCl at 60°C (b)
Potentiodynamic polarization curves of BFC for brass in 1M HCl at 50°C (c)
Potentiodynamic polarization curves of BFC for brass in 1M HCl at 40°C (d)
Potentiodynamic polarization curves of BFC for brass in 1M HCl at 30°CThe rate of corrosion for brass decreases as the concentration of BFC increases with respect to temperature. The presence of inhibitor decreases the rate of corrosion andicorr prominently with an increase in the concentration of inhibitor related to a shift of corrosion potential (Ecorr) to more positive [9–11].Further, the inhibition efficiency of BFC increases with an increase in concentration and temperature. It is due to physisorption of BFC molecule adsorbed at low temperature on brass surface, which is altered to chemisorptions at higher temperature. The maximum inhibition efficiency of BFC was found to be 86.79% in 1.41 mM at 60°C.The corrosion kinetic parameters like corrosion potential (Ecorr), corrosion current density (icorr), and anodic (ba) and cathodic (bc) slopes in the presence and absence of inhibitor obtained from polarization curves were summarized in Table 2. The corrosion current density (icorr) is more compared with the inhibitor, because in HCl there is no inhibitor to cover brass surface. Hence dissolution of metal occurs on the surface of brass. The presence of inhibitor minimizes the acid attack due to the formation of compact and coherent layer on the surface of copper. The addition of inhibitor manifests the shift Ecorr to a positive direction, which suppresses hydrogen evolution and metal dissolution reaction [12].Table 2
Tafel polarization parameters for brass in 1M HCl with BFC from 30°C to 60°C.
S.No. Temp. (°C) Conc. of inhibitor (mM) E c o r r (V/SCE) -ba (mV dec−1) -bc (mV dec−1) i c o r r (mA cm−2) IE% 1 30°C Blank -0.483 6.85 6.78 3.846 -  0.20 -0.516 11.63 5.94 1.882 51.06  0.40 -0.548 10.54 5.70 1.723 55.20  0.60 -0.549 11.77 4.88 1.570 59.17  0.80 -0.546 11.10 4.17 1.401 63.57  1.01 -0.550 11.62 6.72 1.398 63.65  1.21 -0.566 11.82 6.87 1.354 64.79  1.41 -0.599 12.68 6.11 1.136 70.46  2 40°C Blank -0.466 5.663 6.36 5.728 -  0.20 -0.468 6.631 6.77 2.457 57.10  0.40 -0.470 6.178 8.82 2.280 60.19  0.60 -0.466 8.817 8.70 2.161 62.27  0.80 -0.474 8.875 8.97 1.986 65.32  1.01 -0.478 9.957 8.18 1.804 68.50  1.21 -0.482 13.25 8.50 1.629 71.56  1.41 -0.493 11.50 6.90 1.472 74.30  3 50°C Blank -0.433 6.307 6.09 8.532 -  0.20 -0.446 6.128 8.51 3.428 59.82  0.40 -0.451 8.695 7.62 3.276 61.60  0.60 -0.459 13.30 7.84 3.174 62.79  0.80 -0.466 13.81 6.81 2.862 66.45  1.01 -0.472 11..68 6.22 2.650 68.94  1.21 -0.473 8.105 8.90 2.266 73.44  1.41 -0.461 11.73 6.78 1.951 77.13  4 60°C Blank -0.423 5.681 6.36 9.578 -  0.20 -0.436 7.897 7.45 3.773 60.60  0.40 -0.437 11.32 6.95 3.562 62.81  0.60 -0.442 12.92 7.98 3.118 67.44  0.80 -0.448 10.91 7.44 3.046 68.19  1.01 -0.451 10.17 6.76 2.852 70.22  1.21 -0.457 10.33 9.06 2.312 75.86  1.41 -0.478 13.42 7.63 1.268 86.79Many researchers discussed about the corrosion potential of inhibitor, if the potential shift exceeds with ±85mV with respect to the potential of uninhibited solution, the inhibitor acts as either anodic or cathodic type, in addition to thatEcorr vary within ±50mV, and then the inhibitor is mixed type inhibitor. In this present study, BFC acts as a mixed type inhibitor and undergoes both cathodic reaction (hydrogen evolution) and anodic reaction (metal dissolution) [13]. There was no definite trend observed for cathodic Tafel slope and anodic Tafel slope indicates that BFC was first adsorbed on the surface and impeded by merely blocking the reaction sites of the metal without affecting the reaction mechanism [14, 15]. The result obtained from polarization technique was in good agreement with conventional weight loss method.


### 3.3. Electrochemical Impedance Spectroscopy.

Nyquist plot of brass in 1M HCl solution in the absence and presence of different concentration of BFC at 60°C, 50°C, 40°C, and 30°C was shown in Figures6(a), 6(b), 6(c), and 6(d). The Nyquist plot consists of a large capacitive loop at high frequency followed by a small inductive loop at low frequency value. The high frequency capacitive loop is due to charge transfer resistance of the corrosion process and electrical double layer [16]. At lower frequency the loop is attributed to the relaxation process of the adsorbed intermediates by controlling the anodic process [17]. The impedance spectra of BFC were deviated from perfect semicircle due to frequency dispersion effect as a result of roughness and in-homogeneity on the metal surface [18, 19]. Furthermore, the diameter of the capacitive loop in presence of BFC is higher than in HCl and its magnitude is a function of the inhibitor concentration.Figure 6 (a)
AC impedance curves of BFC for brass in 1M HCl at 60°C (b)
AC impedance curves of BFC for brass in 1M HCl at 50°C (c)
AC impedance curves of BFC for brass in 1M HCl at 40°C (d)
AC impedance curves of BFC for brass in 1M HCl at 30°C (e)
Randle’s Equivalent circuit used to fit the impedance spectraThe values of charge transfer resistance (Rct) and double layer capacitance (Cdl) obtained from the Nyquist plot and the calculated inhibition efficiency value were reported in Table3. From the table it is obvious that the value of Cdl decreases as the concentration of inhibitor increases. The decrease in Cdl value is due to increase in local dielectric constant and increase in electrical double layer, suggesting that the inhibitor undergoes adsorption by forming a protective layer on the metal surface with dissolution [20, 21]. The maximum inhibition efficiency of BFC was found to be 91.07% at 60°C for 1.41 Mm of BFC.Table 3
AC impedance parameters for brass in 1M HCl with BFC from 30°C to 60°C.
S.No. Temp. (°C) Conc.of inhibitor (mM) Rct(ohm cm2) Cdl(ohm µF/cm2) I.E % 1. 30°C Blank 28.9 298.0 -  0.20 62.6 167.5 53.83  0.40 68.7 155.0 57.93  0.60 73.5 149.3 60.68  0.80 79.4 141.7 63.60  1.01 86.3 136.2 66.51  1.21 94.1 135.4 69.28  1.41 103.6 113.9 72.10  2. 40°C Blank 21.7 382.0 -  0.20 51.8 268.7 58.10  0.40 58.3 229.0 62.77  0.60 66.5 215.0 67.36  0.80 74.3 209.0 70.74  1.01 78.9 195.7 72.49  1.21 85.2 191.6 74.53  1.41 89.5 177.0 75.78  3. 50°C Blank 10.67 975.0 -  0.20 28.1 582.4 62.02  0.40 30.5 570.0 65.01  0.60 37.2 559.8 71.31  0.80 40.9 533.0 73.91  1.01 45.3 517.9 76.44  1.21 47.6 507.5 77.58  1.41 59.8 480.2 82.15  4. 60°C Blank 7.5 1126 -  0.20 24.8 954.0 62.09  0.40 27.9 922.8 63.74  0.60 35.4 879.0 68.37  0.80 39.7 823.0 71.73  1.01 47.5 760.5 73.51  1.21 56.3 731.0 80.57  1.41 84.0 674.4 91.07To fit the experimental impedance data of brass a simple Randle’s equivalent circuit was shown in Figure6(e) in the absence and presence of BFC. In Figure 6(e) (Rs) is solution resistance, (Rct1) is charge transfer resistance with porous structure on brass surface, (Rct2) is charge transfer resistance with adsorption of inhibitor on brass surface and it acts as a resistor, (W) is Warburg impedance, (CPE1) is first constant phase element, and (CPE2) is second constant phase element. In this Randle’s equivalent circuit, (CPE) is used instead of a pure capacitor owing the frequency dispersion of semicircle.The rough solid electrode, a constant phase element and (ZCPE) were described by the following:(7)ZCPE=Y0-1iω–nwhere Y0 is a proportionality factor, ω is the angular frequency, and n is the CPE exponent whose value lies between 0 and 1 and it is used as a gauge of in-homogeneity or roughness on the brass surface. The n-values of first constant phase element (CPE 1) lie between 0.47 to 0.76 representing double layer capacitance. Addition of inhibitor increases the n value thereby decreasing the CPE. The second constant phase element (CPE 2) is nearly Warburg impedance [22].


### 3.4. Cyclic Voltammetry Measurements

The mechanism of copper corrosion in HCl solution has been studied by many researchers and the main reaction that can take place in the acidic medium is given as follows [23, 24]:(8)Cus+Cl-aq⇌CuClaq+e(9)CuClaq+Cl-aq⇌CuCl2-aq(10)CuCl2-aq⇌Cu2+aq+2Cl-aq+e-(11)2CuCl2-aq+2OH-l⟶Cu2Os+4Cl-aq+H2Oaq(12)Cu2Os+12O2aq+Cl-aq+2H2Oaq⟶Cu2OH3+OH-In this mechanism,CuClaq is adsorbed on the surface of copper electrode. In acidic medium the presence of CuClaq layer is destroyed and the rate of corrosion is more. In presence of inhibitor the CuClaq layer adsorption is strong which is formed on the surface of copper acts as protective layer thereby preventing the oxidation of copper. The dissolution of CuCl2-aq takes place from CuClaq occurring according to (10). Further there is an opportunity of oxidation reaction (11) and (12).The cyclic voltammogram for brass in 1M HCl in the absence and presence of inhibitor was shown in Figures7(a), 7(b), 7(c), and 7(d) at 60°C, 50°C, 40°C, and 30°C. It was observed that bare brass shows an oxidation peaks at the forward scan of 0.289V (SCE). The formation of oxidation peak is due to the Cu2+ or due to the formation of an insoluble Cu2O or due to hydroxychloride reactions from (9)-(12). In reverse sweep also there is a reduction peak occurring at -0.468V (SCE) which is due to the reduction of Cu2+ and insoluble Cu2O layer formed during the oxidation process.Figure 7 (a)
CV for brass in 1M HCl in the absence and presence BFC at 60°C (b)
CV for brass in 1M HCl in the absence and presence BFC at 50°C (c)
CV for brass in 1M HCl in the absence and presence BFC at 40°C (d)
CV for brass in 1M HCl in the absence and presence BFC at 30°CThe cyclic voltammogram as shown in Figures shows the effect of the addition of various concentrations of the inhibitor. It is interesting to note that two main changes have occurred with the addition of the inhibitor. First one exhibits only one peak for brass in both forward and reverse sweep at around -0.12V(SCE) for the forward scan and +0.214 for the reverse sweep. The reduction in the Volt is attributed to adsorption of the inhibitor on the brass surface. The second change is the reduction of the oxidation and reduction peak, which diminishes drastically with the addition of the inhibitor. This observation indicates that the inhibitor added to the solution is adsorbed on the brass surface effectively and reduces the oxidation of the copper in the brass.By comparing the cyclic voltammogram of brass and BFC modified brass, the addition of inhibitor diminishes the oxidation and reduction peak drastically and there are shifts of peak potential from positive to negative direction, respectively. These observations reveal that the addition of inhibitor is adsorbed on the surface of brass effectively and reduces the oxidation of the copper in the brass.The cyclic voltammogram of brass and various concentrations of the inhibitor was carried out at the voltage range of -1.2V to 1V and scan rate was 0.05V. These range was fixed to carry out the oxidation and reduction potential of Zn and copper ions in various oxidation state.


### 3.5. Dezincification Factor by AAS

Dezincification factor is used to measure the percentage of copper and zinc ion present in the HCl solution from weight loss method using atomic absorption spectroscopy (AAS) (Elico-India). Dezincification factor is calculated by the following equation where the concentration of zinc and copper is in ppm [25].(13)Dezincification factorZ=Zn/CusolutionZn/CUAlloyDezincification of 1M HCl and the optimum concentration of the inhibitor (700ppm) were shown in Table4. From the table it was observed that copper and zinc both are leached in the HCl solution. The ratio of copper to zinc ion present in the HCl solution was much lesser than in the alloy.Table 4
Solution analysis by AAS for brass in 1M HCl with BFC.
Conc. of inhibitor (ppm) Solution Analysis Dezincification factor Inhibition (%) Cu (ppm) Zn (ppm) Cu Zn 1 M HCl 0.1170 8.179 62.16 - -  BFC (700 ppm) 0.0524 0.804 34.22 81.07 92.11This is due to the diffusion of ion and it is mainly controlled by the dissolution of the alloy. Copper is less leached than zinc in HCl solution, becauseEo(cu2+/Cu) for copper (+0.34V) has a positive value and Eo(Zn2+/Zn) for Zn is (-0.76) negative. The diffusion of ion is very much related to the size of the ion; zinc (II) ion having an atomic radius of 0.074nm diffuses faster than the copper (II) ion which has atomic radius of 0.096nm. The leaching of copper and zinc ion was minimized by the addition of the inhibitor. But the percentage of the zinc present in inhibitor was much higher than the copper. The dezincification factor of BFC is 34.22 compared with 1M HCl which was 62.16. This indicates that the dezincification factor is reduced by the addition of inhibitor by 27.94%. Results reveal that BFC inhibits the dezincification of brass in 1M HCl at optimum concentration efficiently [26].


### 3.6. Langmuir Adsorption Isotherm

The corrosion action of BFC was characterized by various adsorption isotherm like Langmuir, Freundlich, Temkin, Flory-Huggins, and El-Awady. All these adsorption isotherms follow a general expression as given in the following:(14)fθ,xe-2aθ=KCwhere f(θ,x) is the configurational factor, θ is the surface coverage, K is the constant of the adsorption process and can be equated to equilibrium constant, C is the inhibitors concentration expressed in molarity, and a is the molecular interaction parameter. By careful examination of the R2 value of the various isotherm, Langmuir isotherm was found to fit well with the data of corrosion inhibition. Langmuir isotherm model for the adsorption of BFC on the Brass surface can be represented as follows [27]:(15)Cθ=1K+CPlot of C/θ versus C for various temperatures of BFC is shown in Figure 8 Table 5 shows the values of R2, slope, ΔG, and Kads. The table implies that the slope of the line for the adsorption isotherm is greater than 1.12 at all temperatures which shows that each molecule of BFC occupies more than one site of adsorption in the brass metal. Higher adsorption capacity of BFC means there would be higher corrosion efficiency on the brass.Table 5
Equilibrium and statistical parameter for adsorption of MFC on Brass surface in 1M HCl.
Temperature (K) R2 K a d s slope ΔG 303 0.979 3276 1.452 -30.5087  313 0.984 3839 1.345 -31.931  323 0.991 4735 1.294 -33.514  333 0.983 4135 1.124 -34.17Figure 8
Plot of C/θ versus C for various temperature with BFC.The inhibition of corrosion mechanism of the BFC on the surface of brass was monitored using the surface coverage. Tafel polarization was used for the measurement of the surface coverageθ at different inhibitor concentration. Calculation of surface coverage (θ) calculation was given in the following formula:(16)θ=Vo-VVo(17)ΔGoads=-RTln⁡55.5Kadswhere Vo is the corrosion rate without inhibitor and V is the corrosion rate with inhibitor. Various isotherms were tried with the value ofθ and the best fit was found and as described earlier Langmuir isotherm showed the best fit.Δ G o a d s was calculated using (17) and is give in Table 5 and the value at 60°C was found to be -34.17kJ/mol. Table 5 shows a high value of Kads and the negative sign of ΔGoads which indicates the, as already discussed, strong adsorption of BFC and surface of alloy. ΔGoads values can be used to determine whether physical or chemical adsorption has occurred on the surface of the alloy. When ΔGoads value is less than -20 kJ/mol, physical adsorption (physisorption) is considered to be the major contributor to the adsorption process because of the Vander walls forces of attraction between the alloy and the inhibitor and when ΔGoads value is lesser than -30 kJ/mol; then contribution by chemical adsorption is high. From the table it can be seen BFC shows ΔGoads value more negative than -30kJ/mol at all temperature, so it can be seen that chemical adsorption contributes to higher percentage of adsorption of BFC on the alloy surface. At high temperature ΔGoads becomes more negative which suggest that chemical bond formation takes place to a larger extent at high temperature compared to low temperature.


### 3.7. Effect of Temperature

The effect of temperature on the inhibition action of BFC was studied at different temperature ranges from 30°C to 60°C using Tafel polarization method and EIS measurement. It was observed that change in temperature changes the rate of the corrosion and rate of adsorption of the BFC on the alloy surface. Increase in temperature increases both the chemical adsorption and also the corrosion rate. Increase in the corrosion rate was found to be high in blank compared to the alloy in the presence of the inhibitor as a result the corrosion inhibition efficiency of the BFC increases with increase in temperature. Rapid desorption of the inhibitor, etching of metal, chemisorption of the inhibitor, decomposition of the inhibitor, and rearrangement of the inhibitor are the various process that can take place when the temperature increases. At high temperature BFC forms strong covalent coordinate bond compared to the physical adsorption which dominates at low temperature. At each temperature there is an equilibrium between the adsorption and desorption of the inhibitor on the surface of the brass alloy. When the temperature changes the equilibrium is shifted and a new equilibrium is reached, with BFC the shift in equilibrium is towards the adsorption towards the alloys and an increase in the K value could be observed.Arrhenius equation and transition state equations can be used to calculate the activation energy, enthalpy of adsorption, and entropy of adsorption The Arrhenius and transition state plots are shown in Figures9 and 10. The equation for the calculation of activation energy and thermodynamic parameter is given in the following:(18)logIcorr=-Ea2.303RT+log⁡A(19)Icorr=RTNhexp⁡ΔS∗Rexp⁡-ΔH∗RTFigure 9
Arrhenius plot of logIcorr versus 1/T 10−3for the effect of temperature on the performance of BFC on brass in 1M HCl.Figure 10
Transition state plot for brass corrosion with and without BFC in 1 M HCl at 60°CIn these equationsIcorr represents the corrosion current, R is the universal gas constant, T is the absolute temperature, N is the Avogadro number, h is the plank’s constant, ΔS∗ is the entropy change for the adsorption process, and ΔH∗ is the enthalpy change.Figure9 represents the plot of log (Icorr) versus 1/ (T x 10−3K) for blank and various concentration of inhibitors. A straight line was obtained. Slope of the plot of (18) was used for the calculation of Ea, and Table 6 shows the results. An increase in Ea was observed when the temperature decreases. Radovici classification of the inhibitor was applied to BFC inhibition on Brass surface. Inhibitors were classified according to their behaviour at high temperature. There were three cases: when energy of activation of inhibitor is equal to energy of activation of blank, then with change in temperature there would not be any increase or decrease of inhibition. In the second case when the enthalpy of activation of the blank is greater than enthalpy of activation of inhibitor, then with increase in temperature there would be an increase in the corrosion inhibition; in the last condition when Ea of the blank is less than Ea of inhibitor then increase in temperature decreases the inhibition efficiency [28, 29].Table 6
Thermodynamic parameters for corrosion of brass in 1M HCl with BFC.
Concentration (ppm) E a(kJ/mol) A (A/cm2) Δ H o(kJ/mol) Δ S o(J/K.mol) Δ G o(kJ/mol) 303 313 323 333 Blank 32.824 157.20 20.71 -110.221 51.07 52.07 53.07 54.08  100 24.695 11.16 16.56 -128.532 51.97 53.14 54.31 55.48  300 20.152 10.20 15.75 -133.615 52.55 53.77 54.98 56.20  500 15.974 8.27 15.06 -137.39 52.90 54.15 55.40 56.65  700 11.542 6.11 14.93 -139.779 53.43 54.70 55.97 57.24BFC molecules has heteroatoms like oxygen and nitrogen which can form bonds with the brass surface and can form covalent coordinate bond. With increase in temperature the reaction rate increases as the number of covalent bond formations increases since the activation energy for the formation of the covalent bond decreases. Hence more attraction by the heteroatom of the BFC with the brass metal increases the surface coverage and decrease in the corrosion was observed.It can be inferred from the table that the activation energy is lowest at (11.542) 700 ppm for the adsorption of BFC on the brass surface. Table6 shows that at the inhibitor concentration of 700 ppm the activation energy value is the lowest which is also the optimum condition of inhibitor concentration.The plot of log (Icorr/T) versus 1000/T was shown in Figure 10. ΔHo and ΔSo are calculated from the slope and intercept of straight line is obtained and the values are given in Table 6. ΔHo and ΔSo values at optimum condition of inhibitor in 1M HCl on the brass surface (14.93 kJ/mol and -139.78 J/(mol K)) are less than the values in the absence of inhibitor. The desorption of the solvent molecule and the attraction of the inhibitor towards the surface of the brass makes ΔSo negative because one molecule of inhibitor desorbs more than 1 molecule of the solvent. So the randomness decreases on the surface of the brass, hence decreases in entropy are observed.


### 3.8. Surface Analysis

The surface morphology of the corroded and inhibited brass specimen was studied by the FT-IR and SEM analysis.


#### 3.8.1. FT-IR Analysis

The FT-IR spectrum of BFC was recorded by coating the inhibitors on the KBr disc. The FT-IR spectrum of the brass specimen in the presence and absence of inhibitor was immersed in 1M HCl solution. After the elapsed time the specimens were cleaned with double distilled water and dried at room temperature with cold air. Then it is characterized by Perkin Elmer Make–Model Spectrum RX (FT-IR).FT-IR spectrum of brass in 1 M HCl, BFC, and brass in 1 M HCl with BFC was shown in Figures11(a), 4(a), and 11(b). The corresponding peak values are presented in Table 7. The broad peak at 3732.61 cm−1 is assigned to superficial absorbed water stretching mode of an OH. The stretching frequency of secondary amine shifts from 3216.55 to 3329.56 cm−1 due to lone pair of electrons present in the nitrogen atom which coordinates with Cu2+ to form a complex. A peak between 1300 to 1602.11 cm−1 indicates the presence of secondary amide of BFC. The peak at 1032.87 cm-i indicates the formation of complex. The peaks between the ranges of 400 to 700 cm−1 were mainly due to ZnO2 and CuO2.Table 7
FT-IR analysis of brass in 1 M HCl, BFC, and brass in 1 M HCl with BFC.
FT-IR peak values Possible groups Brass in 1 M HCl ( c m - 1 ) BFC ( c m - 1 ) Brass in 1 M HCl with BFC ( c m - 1 ) 3732.61 ---- ---- υ O-H  ---- 3265.23 3329.56,3216.55 20 Amine  ---- 3058.43,3029.27 3045.61 C-H asymmetric stretch  ---- ----- ---- C-H symmetric stretch  2901.86 2942.37,2808.24, 2757.98, 2698.24 2926.13,2854.75 δ HOH  1695.73 1601.77 ---- 1602.11 Absorbed moisture  ---- 1663.37 ---- C=O  ---- 1591.86 1560.35 Amide I band  ---- 1534.85,1472.72  Amide II band  1394.65 ----- 1382.62 δ OH  ---- 1335.60 ------ Furan ring  1268.12 1188.58  S O 4 2 -  ---- 1138.76  C-H  1027.34 1032.87  800.14 ----- ---- γ OH  ---- 841.92 688.81,582.77 Amine wagFigure 11 (a)
FT-IR peak values of brass in 1 M HCl (b)
FT-IR peak values of brass in 1 M HCl with BFC


#### 3.8.2. SEM Analysis

The brass specimen was polished with various grades of emery sheet, rinsed with distilled water, degreased with acetone. The SEM images of brass were recorded using a scanning electron microscope (standard JEOL 6280 JXXA and LEO 435 VP model electron).The surface morphology of brass sample in 1M HCl solution in the absence and presence of BFC at optimum concentration of 1.81 mM was shown in Figures12(b) and 12(c). The surface of brass metal was badly damaged in HCl solution for 2 hours indicating that there is significant corrosion. However in presence of BFC the surface of brass is smooth, implying that the corrosion rate is controlled. This improvement in surface morphology is due to the formation of a stable protective layer of BFC on brass surface.Figure 12
(a) SEM image of brass before immersion (polished); (b) SEM image of brass in IM HCl; (c) SEM image of brass in IM HCl with BFC.
(a) (b) (c)


### 3.9. Quantum Chemical Calculations

To study the effect of molecular structure on inhibition efficiency, quantum chemical calculation was performed using RB3LYP/6-311G method and the calculations were carried out by the geometrical optimization of BFC. According to Fukui’s frontier molecular orbital theory the ability of the inhibitor is associated with frontier molecular orbital, highest molecular orbital (HOMO), lowest unoccupied molecular orbital (LUMO), and dipole moment (I). The optimization structure of BFC,EHOMO, ELUMO, and Mulliken charges was shown in Figures 13(a), 13(b), 13(c), and 13(d). The energies of frontier orbital theory (EHOMO and ELUMO) are the most important parameters to predict the reactivity of chemical species. It has been observed that EHOMO is associated with electron donating ability of a molecule. The inhibition efficiency of BFC increases with increase in EHOMO. High EHOMO value indicates that the molecule has a tendency to donate electrons to an appropriate acceptor molecule. In addition to that if the value of ELUMO is less, it easily accepts electrons from the donar molecules [30–33].Figure 13 (a)
Optimized molecular structure of BFC (b)
Frontier molecular orbital density distribution of BFC (HOMO) (c)
Frontier molecular orbital density distribution of BFC (LUMO) (d)
Mulliken charges for BFC moleculeComputed parameters such asEHOMO, ELUMO, energy gap (ΔE= ELUMO - EHOMO), dipole moment (μ), absolute electronegativity (χ), global hardness (η), and global softness (σ) were calculated and shown in Table 5. To calculate the quantum chemical parameters χ and η the following equation was used [34–36]:(20)χ=ELUMO+EHOMO2(21)η=ELUMO-EHOMO2The inverse of global hardness (η) is designated as global softness (σ) and it is calculated by the following equation. By calculating these hardness and softness properties, the stability and reactivity of inhibitor molecule are measured:(22)σ=1ηThe energy band gap betweenEHOMO and ELUMO (ΔE) of the molecule is used to expand theoretical models that are qualitatively able to explain the structure and conformation barriers in molecular system. Hard molecule has large energy gap, whereas soft molecule has low gap. Soft molecules are more reactive than hard ones due to the donation of electrons to the acceptors. It is eminent that smaller the value of ΔE of an inhibitor, the higher the inhibition efficiency of molecule [37, 38].From Table8 it is obvious that BFC has higher EHOMO value (-0.0627 eV) which indicates that it donates electrons and the value of ELUMO is less (-0.0282 eV) which implies that it accepts the electrons. The energy band gap value for BFC is low (0.0345 eV) due to the stable nature on the metal surface which affirmed the corrosion resistance of brass in 1M HCl. The dipole moment (μ) value of BFC is 4.9349 which is bigger than the dipole moment of water (1.88 Debye), indicating that there is a strong dipole-dipole interaction between the inhibitor molecule and brass surface. Molecule exhibiting lower energy difference (ΔE) value readily undergoes charge transfer interface on the metal surface, thereby increasing the inhibition efficiency [39–42].Table 8
Quantum chemical parameters for BFC.
Inhibitor E H O M O (eV) E L U M O (eV) ΔE (eV) µ(D) η (eV) σ (eV) χ ω BFC -0.0627 -0.0282 0.0345 4.9349 0.0172 58.13 0.0454 0.2094In this present work the value ofσ is (58.13) high, thereby increasing the inhibition efficiency of BFC, which is in good agreement compared with experimental values. The absolute electronegativity (χ) and global electrophilicity (ω) of BFC were 0.0454 and 0.2094 which indicated the stability and reactivity of inhibitor molecule.The adsorption centers of inhibitor molecules were analysed by using Mulliken charges. The Mulliken charges of BFC molecule reveal that the heteroatom (N) has more negative charge compared with other atoms, which implies that the adsorption of brass metal is due to the electron donation of an electronegative atom (N) to the metal surface.


## 3.1. Weight Loss Method

Table1 indicates the effect of concentration of BFC on the corrosion of brass in 1M HCl. From the table the inhibition efficiency (IE) of BFC increases with an increase in the concentration of inhibitor and temperature [8]. The maximum inhibition efficiency obtained by this method was found to be 77.37 % at a concentration of 1.41 mM and further increase in the concentration and temperature of inhibitor (1.61 to 2.01 mM, 60°C) did not cause any appreciable change in the efficiency of BFC. This is due to the surface blocking effect of inhibitor on the metal by adsorption and film formation mechanism and also due to the presence of protonated nitrogen and the oxygen atom of BFC. The presence of nitrogen and oxygen atom present in BFC absorbs quickly on the metal surface with formation of an insoluble stable film; this makes the inhibitor more effective.Table 1
Weight loss measurements of brass in IM HCl with BFC from 30°C to 60°C.
S.No. Temp. (°C) Con. of inhibitor (mM) Corrosion rate (mmpy) Surface coverage(θ) Inhibition efficiency (I.E)% 1 30°C Blank 35.781 - -  0.20 15.742 0.4278 42.78  0.40 13.552 0.4566 45.66  0.60 9.840 0.4610 46.10  0.80 7.174 0.5052 50.52  1.01 6.711 0.5676 56.76  1.21 5.061 0.6018 60.18  1.41 4.770 0.6149 61.49  2 40°C Blank 65.517 - -  0.20 18.731 0.4681 46.81  0.40 16.874 0.4707 47.07  0.60 15.364 0.4935 49.35  0.80 12.809 0.5309 53.09  1.01 9.781 0.5866 58.66  1.21 6.846 0.6211 62.11  1.41 5.224 0.6324 63.24  3 50°C Blank 98.182 - -  0.20 50.175 0.4920 49.20  0.40 48.011 0.5013 50.13  0.60 43.521 0.5367 53.67  0.80 37.540 0.5671 56.71  1.01 35.839 0.5930 59.30  1.21 29.743 0.6388 63.88  1.41 22.585 0.6500 65.00  4 60°C Blank 468.822 - -  0.20 62.743 0.5486 54.86  0.40 58.770 0.5637 56.37  0.60 50.982 0.6053 60.53  0.80 46.418 0.6652 66.50  1.01 44.730 0.7192 71.92  1.21 36.641 0.7632 76.32  1.41 30.150 0.7737 77.37


## 3.2. Tafel Polarization Measurements

Figures5(a), 5(b), 5(c), and 5(d) indicate the potentiodynamic polarization curves for the brass electrode in 1M HCl solution with and without different concentrations of BFC at 60°C, 50°C, 40°C, and 30°C. It was clear that the current density decreases with the presence of BFC which indicates that inhibitor is adsorbed on the surface of metal. The values of corrosion potential (Ecorr) and corrosion current density (icorr) are obtained by Tafel extrapolation method, anodic (ba) and cathodic (bc) These polarization curves indicate that there is a clear reduction of both anodic and cathodic currents in the presence of BFC compared with Blank solution.Figure 5 (a)
Potentiodynamic polarization curves of BFC for brass in 1M HCl at 60°C (b)
Potentiodynamic polarization curves of BFC for brass in 1M HCl at 50°C (c)
Potentiodynamic polarization curves of BFC for brass in 1M HCl at 40°C (d)
Potentiodynamic polarization curves of BFC for brass in 1M HCl at 30°CThe rate of corrosion for brass decreases as the concentration of BFC increases with respect to temperature. The presence of inhibitor decreases the rate of corrosion andicorr prominently with an increase in the concentration of inhibitor related to a shift of corrosion potential (Ecorr) to more positive [9–11].Further, the inhibition efficiency of BFC increases with an increase in concentration and temperature. It is due to physisorption of BFC molecule adsorbed at low temperature on brass surface, which is altered to chemisorptions at higher temperature. The maximum inhibition efficiency of BFC was found to be 86.79% in 1.41 mM at 60°C.The corrosion kinetic parameters like corrosion potential (Ecorr), corrosion current density (icorr), and anodic (ba) and cathodic (bc) slopes in the presence and absence of inhibitor obtained from polarization curves were summarized in Table 2. The corrosion current density (icorr) is more compared with the inhibitor, because in HCl there is no inhibitor to cover brass surface. Hence dissolution of metal occurs on the surface of brass. The presence of inhibitor minimizes the acid attack due to the formation of compact and coherent layer on the surface of copper. The addition of inhibitor manifests the shift Ecorr to a positive direction, which suppresses hydrogen evolution and metal dissolution reaction [12].Table 2
Tafel polarization parameters for brass in 1M HCl with BFC from 30°C to 60°C.
S.No. Temp. (°C) Conc. of inhibitor (mM) E c o r r (V/SCE) -ba (mV dec−1) -bc (mV dec−1) i c o r r (mA cm−2) IE% 1 30°C Blank -0.483 6.85 6.78 3.846 -  0.20 -0.516 11.63 5.94 1.882 51.06  0.40 -0.548 10.54 5.70 1.723 55.20  0.60 -0.549 11.77 4.88 1.570 59.17  0.80 -0.546 11.10 4.17 1.401 63.57  1.01 -0.550 11.62 6.72 1.398 63.65  1.21 -0.566 11.82 6.87 1.354 64.79  1.41 -0.599 12.68 6.11 1.136 70.46  2 40°C Blank -0.466 5.663 6.36 5.728 -  0.20 -0.468 6.631 6.77 2.457 57.10  0.40 -0.470 6.178 8.82 2.280 60.19  0.60 -0.466 8.817 8.70 2.161 62.27  0.80 -0.474 8.875 8.97 1.986 65.32  1.01 -0.478 9.957 8.18 1.804 68.50  1.21 -0.482 13.25 8.50 1.629 71.56  1.41 -0.493 11.50 6.90 1.472 74.30  3 50°C Blank -0.433 6.307 6.09 8.532 -  0.20 -0.446 6.128 8.51 3.428 59.82  0.40 -0.451 8.695 7.62 3.276 61.60  0.60 -0.459 13.30 7.84 3.174 62.79  0.80 -0.466 13.81 6.81 2.862 66.45  1.01 -0.472 11..68 6.22 2.650 68.94  1.21 -0.473 8.105 8.90 2.266 73.44  1.41 -0.461 11.73 6.78 1.951 77.13  4 60°C Blank -0.423 5.681 6.36 9.578 -  0.20 -0.436 7.897 7.45 3.773 60.60  0.40 -0.437 11.32 6.95 3.562 62.81  0.60 -0.442 12.92 7.98 3.118 67.44  0.80 -0.448 10.91 7.44 3.046 68.19  1.01 -0.451 10.17 6.76 2.852 70.22  1.21 -0.457 10.33 9.06 2.312 75.86  1.41 -0.478 13.42 7.63 1.268 86.79Many researchers discussed about the corrosion potential of inhibitor, if the potential shift exceeds with ±85mV with respect to the potential of uninhibited solution, the inhibitor acts as either anodic or cathodic type, in addition to thatEcorr vary within ±50mV, and then the inhibitor is mixed type inhibitor. In this present study, BFC acts as a mixed type inhibitor and undergoes both cathodic reaction (hydrogen evolution) and anodic reaction (metal dissolution) [13]. There was no definite trend observed for cathodic Tafel slope and anodic Tafel slope indicates that BFC was first adsorbed on the surface and impeded by merely blocking the reaction sites of the metal without affecting the reaction mechanism [14, 15]. The result obtained from polarization technique was in good agreement with conventional weight loss method.


## 3.3. Electrochemical Impedance Spectroscopy.

Nyquist plot of brass in 1M HCl solution in the absence and presence of different concentration of BFC at 60°C, 50°C, 40°C, and 30°C was shown in Figures6(a), 6(b), 6(c), and 6(d). The Nyquist plot consists of a large capacitive loop at high frequency followed by a small inductive loop at low frequency value. The high frequency capacitive loop is due to charge transfer resistance of the corrosion process and electrical double layer [16]. At lower frequency the loop is attributed to the relaxation process of the adsorbed intermediates by controlling the anodic process [17]. The impedance spectra of BFC were deviated from perfect semicircle due to frequency dispersion effect as a result of roughness and in-homogeneity on the metal surface [18, 19]. Furthermore, the diameter of the capacitive loop in presence of BFC is higher than in HCl and its magnitude is a function of the inhibitor concentration.Figure 6 (a)
AC impedance curves of BFC for brass in 1M HCl at 60°C (b)
AC impedance curves of BFC for brass in 1M HCl at 50°C (c)
AC impedance curves of BFC for brass in 1M HCl at 40°C (d)
AC impedance curves of BFC for brass in 1M HCl at 30°C (e)
Randle’s Equivalent circuit used to fit the impedance spectraThe values of charge transfer resistance (Rct) and double layer capacitance (Cdl) obtained from the Nyquist plot and the calculated inhibition efficiency value were reported in Table3. From the table it is obvious that the value of Cdl decreases as the concentration of inhibitor increases. The decrease in Cdl value is due to increase in local dielectric constant and increase in electrical double layer, suggesting that the inhibitor undergoes adsorption by forming a protective layer on the metal surface with dissolution [20, 21]. The maximum inhibition efficiency of BFC was found to be 91.07% at 60°C for 1.41 Mm of BFC.Table 3
AC impedance parameters for brass in 1M HCl with BFC from 30°C to 60°C.
S.No. Temp. (°C) Conc.of inhibitor (mM) Rct(ohm cm2) Cdl(ohm µF/cm2) I.E % 1. 30°C Blank 28.9 298.0 -  0.20 62.6 167.5 53.83  0.40 68.7 155.0 57.93  0.60 73.5 149.3 60.68  0.80 79.4 141.7 63.60  1.01 86.3 136.2 66.51  1.21 94.1 135.4 69.28  1.41 103.6 113.9 72.10  2. 40°C Blank 21.7 382.0 -  0.20 51.8 268.7 58.10  0.40 58.3 229.0 62.77  0.60 66.5 215.0 67.36  0.80 74.3 209.0 70.74  1.01 78.9 195.7 72.49  1.21 85.2 191.6 74.53  1.41 89.5 177.0 75.78  3. 50°C Blank 10.67 975.0 -  0.20 28.1 582.4 62.02  0.40 30.5 570.0 65.01  0.60 37.2 559.8 71.31  0.80 40.9 533.0 73.91  1.01 45.3 517.9 76.44  1.21 47.6 507.5 77.58  1.41 59.8 480.2 82.15  4. 60°C Blank 7.5 1126 -  0.20 24.8 954.0 62.09  0.40 27.9 922.8 63.74  0.60 35.4 879.0 68.37  0.80 39.7 823.0 71.73  1.01 47.5 760.5 73.51  1.21 56.3 731.0 80.57  1.41 84.0 674.4 91.07To fit the experimental impedance data of brass a simple Randle’s equivalent circuit was shown in Figure6(e) in the absence and presence of BFC. In Figure 6(e) (Rs) is solution resistance, (Rct1) is charge transfer resistance with porous structure on brass surface, (Rct2) is charge transfer resistance with adsorption of inhibitor on brass surface and it acts as a resistor, (W) is Warburg impedance, (CPE1) is first constant phase element, and (CPE2) is second constant phase element. In this Randle’s equivalent circuit, (CPE) is used instead of a pure capacitor owing the frequency dispersion of semicircle.The rough solid electrode, a constant phase element and (ZCPE) were described by the following:(7)ZCPE=Y0-1iω–nwhere Y0 is a proportionality factor, ω is the angular frequency, and n is the CPE exponent whose value lies between 0 and 1 and it is used as a gauge of in-homogeneity or roughness on the brass surface. The n-values of first constant phase element (CPE 1) lie between 0.47 to 0.76 representing double layer capacitance. Addition of inhibitor increases the n value thereby decreasing the CPE. The second constant phase element (CPE 2) is nearly Warburg impedance [22].


## 3.4. Cyclic Voltammetry Measurements

The mechanism of copper corrosion in HCl solution has been studied by many researchers and the main reaction that can take place in the acidic medium is given as follows [23, 24]:(8)Cus+Cl-aq⇌CuClaq+e(9)CuClaq+Cl-aq⇌CuCl2-aq(10)CuCl2-aq⇌Cu2+aq+2Cl-aq+e-(11)2CuCl2-aq+2OH-l⟶Cu2Os+4Cl-aq+H2Oaq(12)Cu2Os+12O2aq+Cl-aq+2H2Oaq⟶Cu2OH3+OH-In this mechanism,CuClaq is adsorbed on the surface of copper electrode. In acidic medium the presence of CuClaq layer is destroyed and the rate of corrosion is more. In presence of inhibitor the CuClaq layer adsorption is strong which is formed on the surface of copper acts as protective layer thereby preventing the oxidation of copper. The dissolution of CuCl2-aq takes place from CuClaq occurring according to (10). Further there is an opportunity of oxidation reaction (11) and (12).The cyclic voltammogram for brass in 1M HCl in the absence and presence of inhibitor was shown in Figures7(a), 7(b), 7(c), and 7(d) at 60°C, 50°C, 40°C, and 30°C. It was observed that bare brass shows an oxidation peaks at the forward scan of 0.289V (SCE). The formation of oxidation peak is due to the Cu2+ or due to the formation of an insoluble Cu2O or due to hydroxychloride reactions from (9)-(12). In reverse sweep also there is a reduction peak occurring at -0.468V (SCE) which is due to the reduction of Cu2+ and insoluble Cu2O layer formed during the oxidation process.Figure 7 (a)
CV for brass in 1M HCl in the absence and presence BFC at 60°C (b)
CV for brass in 1M HCl in the absence and presence BFC at 50°C (c)
CV for brass in 1M HCl in the absence and presence BFC at 40°C (d)
CV for brass in 1M HCl in the absence and presence BFC at 30°CThe cyclic voltammogram as shown in Figures shows the effect of the addition of various concentrations of the inhibitor. It is interesting to note that two main changes have occurred with the addition of the inhibitor. First one exhibits only one peak for brass in both forward and reverse sweep at around -0.12V(SCE) for the forward scan and +0.214 for the reverse sweep. The reduction in the Volt is attributed to adsorption of the inhibitor on the brass surface. The second change is the reduction of the oxidation and reduction peak, which diminishes drastically with the addition of the inhibitor. This observation indicates that the inhibitor added to the solution is adsorbed on the brass surface effectively and reduces the oxidation of the copper in the brass.By comparing the cyclic voltammogram of brass and BFC modified brass, the addition of inhibitor diminishes the oxidation and reduction peak drastically and there are shifts of peak potential from positive to negative direction, respectively. These observations reveal that the addition of inhibitor is adsorbed on the surface of brass effectively and reduces the oxidation of the copper in the brass.The cyclic voltammogram of brass and various concentrations of the inhibitor was carried out at the voltage range of -1.2V to 1V and scan rate was 0.05V. These range was fixed to carry out the oxidation and reduction potential of Zn and copper ions in various oxidation state.


## 3.5. Dezincification Factor by AAS

Dezincification factor is used to measure the percentage of copper and zinc ion present in the HCl solution from weight loss method using atomic absorption spectroscopy (AAS) (Elico-India). Dezincification factor is calculated by the following equation where the concentration of zinc and copper is in ppm [25].(13)Dezincification factorZ=Zn/CusolutionZn/CUAlloyDezincification of 1M HCl and the optimum concentration of the inhibitor (700ppm) were shown in Table4. From the table it was observed that copper and zinc both are leached in the HCl solution. The ratio of copper to zinc ion present in the HCl solution was much lesser than in the alloy.Table 4
Solution analysis by AAS for brass in 1M HCl with BFC.
Conc. of inhibitor (ppm) Solution Analysis Dezincification factor Inhibition (%) Cu (ppm) Zn (ppm) Cu Zn 1 M HCl 0.1170 8.179 62.16 - -  BFC (700 ppm) 0.0524 0.804 34.22 81.07 92.11This is due to the diffusion of ion and it is mainly controlled by the dissolution of the alloy. Copper is less leached than zinc in HCl solution, becauseEo(cu2+/Cu) for copper (+0.34V) has a positive value and Eo(Zn2+/Zn) for Zn is (-0.76) negative. The diffusion of ion is very much related to the size of the ion; zinc (II) ion having an atomic radius of 0.074nm diffuses faster than the copper (II) ion which has atomic radius of 0.096nm. The leaching of copper and zinc ion was minimized by the addition of the inhibitor. But the percentage of the zinc present in inhibitor was much higher than the copper. The dezincification factor of BFC is 34.22 compared with 1M HCl which was 62.16. This indicates that the dezincification factor is reduced by the addition of inhibitor by 27.94%. Results reveal that BFC inhibits the dezincification of brass in 1M HCl at optimum concentration efficiently [26].


## 3.6. Langmuir Adsorption Isotherm

The corrosion action of BFC was characterized by various adsorption isotherm like Langmuir, Freundlich, Temkin, Flory-Huggins, and El-Awady. All these adsorption isotherms follow a general expression as given in the following:(14)fθ,xe-2aθ=KCwhere f(θ,x) is the configurational factor, θ is the surface coverage, K is the constant of the adsorption process and can be equated to equilibrium constant, C is the inhibitors concentration expressed in molarity, and a is the molecular interaction parameter. By careful examination of the R2 value of the various isotherm, Langmuir isotherm was found to fit well with the data of corrosion inhibition. Langmuir isotherm model for the adsorption of BFC on the Brass surface can be represented as follows [27]:(15)Cθ=1K+CPlot of C/θ versus C for various temperatures of BFC is shown in Figure 8 Table 5 shows the values of R2, slope, ΔG, and Kads. The table implies that the slope of the line for the adsorption isotherm is greater than 1.12 at all temperatures which shows that each molecule of BFC occupies more than one site of adsorption in the brass metal. Higher adsorption capacity of BFC means there would be higher corrosion efficiency on the brass.Table 5
Equilibrium and statistical parameter for adsorption of MFC on Brass surface in 1M HCl.
Temperature (K) R2 K a d s slope ΔG 303 0.979 3276 1.452 -30.5087  313 0.984 3839 1.345 -31.931  323 0.991 4735 1.294 -33.514  333 0.983 4135 1.124 -34.17Figure 8
Plot of C/θ versus C for various temperature with BFC.The inhibition of corrosion mechanism of the BFC on the surface of brass was monitored using the surface coverage. Tafel polarization was used for the measurement of the surface coverageθ at different inhibitor concentration. Calculation of surface coverage (θ) calculation was given in the following formula:(16)θ=Vo-VVo(17)ΔGoads=-RTln⁡55.5Kadswhere Vo is the corrosion rate without inhibitor and V is the corrosion rate with inhibitor. Various isotherms were tried with the value ofθ and the best fit was found and as described earlier Langmuir isotherm showed the best fit.Δ G o a d s was calculated using (17) and is give in Table 5 and the value at 60°C was found to be -34.17kJ/mol. Table 5 shows a high value of Kads and the negative sign of ΔGoads which indicates the, as already discussed, strong adsorption of BFC and surface of alloy. ΔGoads values can be used to determine whether physical or chemical adsorption has occurred on the surface of the alloy. When ΔGoads value is less than -20 kJ/mol, physical adsorption (physisorption) is considered to be the major contributor to the adsorption process because of the Vander walls forces of attraction between the alloy and the inhibitor and when ΔGoads value is lesser than -30 kJ/mol; then contribution by chemical adsorption is high. From the table it can be seen BFC shows ΔGoads value more negative than -30kJ/mol at all temperature, so it can be seen that chemical adsorption contributes to higher percentage of adsorption of BFC on the alloy surface. At high temperature ΔGoads becomes more negative which suggest that chemical bond formation takes place to a larger extent at high temperature compared to low temperature.


## 3.7. Effect of Temperature

The effect of temperature on the inhibition action of BFC was studied at different temperature ranges from 30°C to 60°C using Tafel polarization method and EIS measurement. It was observed that change in temperature changes the rate of the corrosion and rate of adsorption of the BFC on the alloy surface. Increase in temperature increases both the chemical adsorption and also the corrosion rate. Increase in the corrosion rate was found to be high in blank compared to the alloy in the presence of the inhibitor as a result the corrosion inhibition efficiency of the BFC increases with increase in temperature. Rapid desorption of the inhibitor, etching of metal, chemisorption of the inhibitor, decomposition of the inhibitor, and rearrangement of the inhibitor are the various process that can take place when the temperature increases. At high temperature BFC forms strong covalent coordinate bond compared to the physical adsorption which dominates at low temperature. At each temperature there is an equilibrium between the adsorption and desorption of the inhibitor on the surface of the brass alloy. When the temperature changes the equilibrium is shifted and a new equilibrium is reached, with BFC the shift in equilibrium is towards the adsorption towards the alloys and an increase in the K value could be observed.Arrhenius equation and transition state equations can be used to calculate the activation energy, enthalpy of adsorption, and entropy of adsorption The Arrhenius and transition state plots are shown in Figures9 and 10. The equation for the calculation of activation energy and thermodynamic parameter is given in the following:(18)logIcorr=-Ea2.303RT+log⁡A(19)Icorr=RTNhexp⁡ΔS∗Rexp⁡-ΔH∗RTFigure 9
Arrhenius plot of logIcorr versus 1/T 10−3for the effect of temperature on the performance of BFC on brass in 1M HCl.Figure 10
Transition state plot for brass corrosion with and without BFC in 1 M HCl at 60°CIn these equationsIcorr represents the corrosion current, R is the universal gas constant, T is the absolute temperature, N is the Avogadro number, h is the plank’s constant, ΔS∗ is the entropy change for the adsorption process, and ΔH∗ is the enthalpy change.Figure9 represents the plot of log (Icorr) versus 1/ (T x 10−3K) for blank and various concentration of inhibitors. A straight line was obtained. Slope of the plot of (18) was used for the calculation of Ea, and Table 6 shows the results. An increase in Ea was observed when the temperature decreases. Radovici classification of the inhibitor was applied to BFC inhibition on Brass surface. Inhibitors were classified according to their behaviour at high temperature. There were three cases: when energy of activation of inhibitor is equal to energy of activation of blank, then with change in temperature there would not be any increase or decrease of inhibition. In the second case when the enthalpy of activation of the blank is greater than enthalpy of activation of inhibitor, then with increase in temperature there would be an increase in the corrosion inhibition; in the last condition when Ea of the blank is less than Ea of inhibitor then increase in temperature decreases the inhibition efficiency [28, 29].Table 6
Thermodynamic parameters for corrosion of brass in 1M HCl with BFC.
Concentration (ppm) E a(kJ/mol) A (A/cm2) Δ H o(kJ/mol) Δ S o(J/K.mol) Δ G o(kJ/mol) 303 313 323 333 Blank 32.824 157.20 20.71 -110.221 51.07 52.07 53.07 54.08  100 24.695 11.16 16.56 -128.532 51.97 53.14 54.31 55.48  300 20.152 10.20 15.75 -133.615 52.55 53.77 54.98 56.20  500 15.974 8.27 15.06 -137.39 52.90 54.15 55.40 56.65  700 11.542 6.11 14.93 -139.779 53.43 54.70 55.97 57.24BFC molecules has heteroatoms like oxygen and nitrogen which can form bonds with the brass surface and can form covalent coordinate bond. With increase in temperature the reaction rate increases as the number of covalent bond formations increases since the activation energy for the formation of the covalent bond decreases. Hence more attraction by the heteroatom of the BFC with the brass metal increases the surface coverage and decrease in the corrosion was observed.It can be inferred from the table that the activation energy is lowest at (11.542) 700 ppm for the adsorption of BFC on the brass surface. Table6 shows that at the inhibitor concentration of 700 ppm the activation energy value is the lowest which is also the optimum condition of inhibitor concentration.The plot of log (Icorr/T) versus 1000/T was shown in Figure 10. ΔHo and ΔSo are calculated from the slope and intercept of straight line is obtained and the values are given in Table 6. ΔHo and ΔSo values at optimum condition of inhibitor in 1M HCl on the brass surface (14.93 kJ/mol and -139.78 J/(mol K)) are less than the values in the absence of inhibitor. The desorption of the solvent molecule and the attraction of the inhibitor towards the surface of the brass makes ΔSo negative because one molecule of inhibitor desorbs more than 1 molecule of the solvent. So the randomness decreases on the surface of the brass, hence decreases in entropy are observed.


## 3.8. Surface Analysis

The surface morphology of the corroded and inhibited brass specimen was studied by the FT-IR and SEM analysis.


### 3.8.1. FT-IR Analysis

The FT-IR spectrum of BFC was recorded by coating the inhibitors on the KBr disc. The FT-IR spectrum of the brass specimen in the presence and absence of inhibitor was immersed in 1M HCl solution. After the elapsed time the specimens were cleaned with double distilled water and dried at room temperature with cold air. Then it is characterized by Perkin Elmer Make–Model Spectrum RX (FT-IR).FT-IR spectrum of brass in 1 M HCl, BFC, and brass in 1 M HCl with BFC was shown in Figures11(a), 4(a), and 11(b). The corresponding peak values are presented in Table 7. The broad peak at 3732.61 cm−1 is assigned to superficial absorbed water stretching mode of an OH. The stretching frequency of secondary amine shifts from 3216.55 to 3329.56 cm−1 due to lone pair of electrons present in the nitrogen atom which coordinates with Cu2+ to form a complex. A peak between 1300 to 1602.11 cm−1 indicates the presence of secondary amide of BFC. The peak at 1032.87 cm-i indicates the formation of complex. The peaks between the ranges of 400 to 700 cm−1 were mainly due to ZnO2 and CuO2.Table 7
FT-IR analysis of brass in 1 M HCl, BFC, and brass in 1 M HCl with BFC.
FT-IR peak values Possible groups Brass in 1 M HCl ( c m - 1 ) BFC ( c m - 1 ) Brass in 1 M HCl with BFC ( c m - 1 ) 3732.61 ---- ---- υ O-H  ---- 3265.23 3329.56,3216.55 20 Amine  ---- 3058.43,3029.27 3045.61 C-H asymmetric stretch  ---- ----- ---- C-H symmetric stretch  2901.86 2942.37,2808.24, 2757.98, 2698.24 2926.13,2854.75 δ HOH  1695.73 1601.77 ---- 1602.11 Absorbed moisture  ---- 1663.37 ---- C=O  ---- 1591.86 1560.35 Amide I band  ---- 1534.85,1472.72  Amide II band  1394.65 ----- 1382.62 δ OH  ---- 1335.60 ------ Furan ring  1268.12 1188.58  S O 4 2 -  ---- 1138.76  C-H  1027.34 1032.87  800.14 ----- ---- γ OH  ---- 841.92 688.81,582.77 Amine wagFigure 11 (a)
FT-IR peak values of brass in 1 M HCl (b)
FT-IR peak values of brass in 1 M HCl with BFC


### 3.8.2. SEM Analysis

The brass specimen was polished with various grades of emery sheet, rinsed with distilled water, degreased with acetone. The SEM images of brass were recorded using a scanning electron microscope (standard JEOL 6280 JXXA and LEO 435 VP model electron).The surface morphology of brass sample in 1M HCl solution in the absence and presence of BFC at optimum concentration of 1.81 mM was shown in Figures12(b) and 12(c). The surface of brass metal was badly damaged in HCl solution for 2 hours indicating that there is significant corrosion. However in presence of BFC the surface of brass is smooth, implying that the corrosion rate is controlled. This improvement in surface morphology is due to the formation of a stable protective layer of BFC on brass surface.Figure 12
(a) SEM image of brass before immersion (polished); (b) SEM image of brass in IM HCl; (c) SEM image of brass in IM HCl with BFC.
(a) (b) (c)


## 3.8.1. FT-IR Analysis

The FT-IR spectrum of BFC was recorded by coating the inhibitors on the KBr disc. The FT-IR spectrum of the brass specimen in the presence and absence of inhibitor was immersed in 1M HCl solution. After the elapsed time the specimens were cleaned with double distilled water and dried at room temperature with cold air. Then it is characterized by Perkin Elmer Make–Model Spectrum RX (FT-IR).FT-IR spectrum of brass in 1 M HCl, BFC, and brass in 1 M HCl with BFC was shown in Figures11(a), 4(a), and 11(b). The corresponding peak values are presented in Table 7. The broad peak at 3732.61 cm−1 is assigned to superficial absorbed water stretching mode of an OH. The stretching frequency of secondary amine shifts from 3216.55 to 3329.56 cm−1 due to lone pair of electrons present in the nitrogen atom which coordinates with Cu2+ to form a complex. A peak between 1300 to 1602.11 cm−1 indicates the presence of secondary amide of BFC. The peak at 1032.87 cm-i indicates the formation of complex. The peaks between the ranges of 400 to 700 cm−1 were mainly due to ZnO2 and CuO2.Table 7
FT-IR analysis of brass in 1 M HCl, BFC, and brass in 1 M HCl with BFC.
FT-IR peak values Possible groups Brass in 1 M HCl ( c m - 1 ) BFC ( c m - 1 ) Brass in 1 M HCl with BFC ( c m - 1 ) 3732.61 ---- ---- υ O-H  ---- 3265.23 3329.56,3216.55 20 Amine  ---- 3058.43,3029.27 3045.61 C-H asymmetric stretch  ---- ----- ---- C-H symmetric stretch  2901.86 2942.37,2808.24, 2757.98, 2698.24 2926.13,2854.75 δ HOH  1695.73 1601.77 ---- 1602.11 Absorbed moisture  ---- 1663.37 ---- C=O  ---- 1591.86 1560.35 Amide I band  ---- 1534.85,1472.72  Amide II band  1394.65 ----- 1382.62 δ OH  ---- 1335.60 ------ Furan ring  1268.12 1188.58  S O 4 2 -  ---- 1138.76  C-H  1027.34 1032.87  800.14 ----- ---- γ OH  ---- 841.92 688.81,582.77 Amine wagFigure 11 (a)
FT-IR peak values of brass in 1 M HCl (b)
FT-IR peak values of brass in 1 M HCl with BFC


## 3.8.2. SEM Analysis

The brass specimen was polished with various grades of emery sheet, rinsed with distilled water, degreased with acetone. The SEM images of brass were recorded using a scanning electron microscope (standard JEOL 6280 JXXA and LEO 435 VP model electron).The surface morphology of brass sample in 1M HCl solution in the absence and presence of BFC at optimum concentration of 1.81 mM was shown in Figures12(b) and 12(c). The surface of brass metal was badly damaged in HCl solution for 2 hours indicating that there is significant corrosion. However in presence of BFC the surface of brass is smooth, implying that the corrosion rate is controlled. This improvement in surface morphology is due to the formation of a stable protective layer of BFC on brass surface.Figure 12
(a) SEM image of brass before immersion (polished); (b) SEM image of brass in IM HCl; (c) SEM image of brass in IM HCl with BFC.
(a) (b) (c)


## 3.9. Quantum Chemical Calculations

To study the effect of molecular structure on inhibition efficiency, quantum chemical calculation was performed using RB3LYP/6-311G method and the calculations were carried out by the geometrical optimization of BFC. According to Fukui’s frontier molecular orbital theory the ability of the inhibitor is associated with frontier molecular orbital, highest molecular orbital (HOMO), lowest unoccupied molecular orbital (LUMO), and dipole moment (I). The optimization structure of BFC,EHOMO, ELUMO, and Mulliken charges was shown in Figures 13(a), 13(b), 13(c), and 13(d). The energies of frontier orbital theory (EHOMO and ELUMO) are the most important parameters to predict the reactivity of chemical species. It has been observed that EHOMO is associated with electron donating ability of a molecule. The inhibition efficiency of BFC increases with increase in EHOMO. High EHOMO value indicates that the molecule has a tendency to donate electrons to an appropriate acceptor molecule. In addition to that if the value of ELUMO is less, it easily accepts electrons from the donar molecules [30–33].Figure 13 (a)
Optimized molecular structure of BFC (b)
Frontier molecular orbital density distribution of BFC (HOMO) (c)
Frontier molecular orbital density distribution of BFC (LUMO) (d)
Mulliken charges for BFC moleculeComputed parameters such asEHOMO, ELUMO, energy gap (ΔE= ELUMO - EHOMO), dipole moment (μ), absolute electronegativity (χ), global hardness (η), and global softness (σ) were calculated and shown in Table 5. To calculate the quantum chemical parameters χ and η the following equation was used [34–36]:(20)χ=ELUMO+EHOMO2(21)η=ELUMO-EHOMO2The inverse of global hardness (η) is designated as global softness (σ) and it is calculated by the following equation. By calculating these hardness and softness properties, the stability and reactivity of inhibitor molecule are measured:(22)σ=1ηThe energy band gap betweenEHOMO and ELUMO (ΔE) of the molecule is used to expand theoretical models that are qualitatively able to explain the structure and conformation barriers in molecular system. Hard molecule has large energy gap, whereas soft molecule has low gap. Soft molecules are more reactive than hard ones due to the donation of electrons to the acceptors. It is eminent that smaller the value of ΔE of an inhibitor, the higher the inhibition efficiency of molecule [37, 38].From Table8 it is obvious that BFC has higher EHOMO value (-0.0627 eV) which indicates that it donates electrons and the value of ELUMO is less (-0.0282 eV) which implies that it accepts the electrons. The energy band gap value for BFC is low (0.0345 eV) due to the stable nature on the metal surface which affirmed the corrosion resistance of brass in 1M HCl. The dipole moment (μ) value of BFC is 4.9349 which is bigger than the dipole moment of water (1.88 Debye), indicating that there is a strong dipole-dipole interaction between the inhibitor molecule and brass surface. Molecule exhibiting lower energy difference (ΔE) value readily undergoes charge transfer interface on the metal surface, thereby increasing the inhibition efficiency [39–42].Table 8
Quantum chemical parameters for BFC.
Inhibitor E H O M O (eV) E L U M O (eV) ΔE (eV) µ(D) η (eV) σ (eV) χ ω BFC -0.0627 -0.0282 0.0345 4.9349 0.0172 58.13 0.0454 0.2094In this present work the value ofσ is (58.13) high, thereby increasing the inhibition efficiency of BFC, which is in good agreement compared with experimental values. The absolute electronegativity (χ) and global electrophilicity (ω) of BFC were 0.0454 and 0.2094 which indicated the stability and reactivity of inhibitor molecule.The adsorption centers of inhibitor molecules were analysed by using Mulliken charges. The Mulliken charges of BFC molecule reveal that the heteroatom (N) has more negative charge compared with other atoms, which implies that the adsorption of brass metal is due to the electron donation of an electronegative atom (N) to the metal surface.


## 4. Conclusions

The structure of the synthesized compound BFC was confirmed by spectral data. Weight loss measurement indicates that the inhibition efficiency of BFC increases with an increase in concentration and temperature ranges from 30°C to 60°C. Polarization measurements imply that BFC acts as a mixed type inhibitor, and it controls both hydrogen evolution and metal dissolution process. The inhibition efficiency of BFC obtained from AC impedance is in good agreement compared with the conventional weight loss and polarization methods.Cyclic voltammetry study reveals that the addition of inhibitor reduces the oxidation of copper on the surface of brass. Adsorption isotherm shows that BFC obeys Langmuir adsorption isotherm and the reaction is exothermic. The inhibition efficiency of BFC was closely related to quantum chemical parameters. The purity of the inhibitor was confirmed by LC-MS.



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*Source: 9372804-2018-07-02.xml*