Article

Synergistic Effect of Cinnamon (Cinnamomum burmannii) Leaves Extract and

Potassium Iodide on Mild Steel in HCl

Rohil¹, Yeni Stiadi², Emriadi^3*

^1,2,3Department of Chemistry, Faculty of Mathematics and Natural Sciences, Andalas University, Padang,

25163, Indonesia

Abstract

The synergistic impact of potassium iodide with cinnamon leaf extract (CLE) on hindering gentle steel

corrosion in a HCl arrangement was examined utilizing weight loss measurement, UV-Vis spectroscopy,

and X-ray diffraction (XRD) analysis. At an inhibitor concentration of 10 g/L CLE coupled with 0.04 g/L

potassium iodide, the inhibition efficiency increased from 92.8% to 97.06% as the temperature and

concentration increased. The Langmuir adsorption isotherm was followed by the inhibitor's adsorption

on the mild steel surface. The synergistic interaction between CLE and potassium iodide was validated

when the synergistic parameter (S) was greater than 1. The inhibitor components and the steel surface

formed a coordination complex, according to UV-Vis analysis. When CLE was present, a defensive layer

formed on the mild steel surface that prevented the corrosive medium from interacting with the metal,

as confirmed by XRD analysis. These results imply that potassium iodide and CLE may be useful and

sustainable corrosion inhibitors for mild steel in acidic environments.

Keywords: Mild Steel; corrosion inhibitor; cinnamon; weight loss; synergistic effect

Graphical Abstract

*

Corresponding author

Email addresses: emriadi@sci.unand.ac.id

DOI: https://doi.org/10.22437/chp.v9i1.42334

Received March 08^th2025; Accepted May 01^st2025; Available online June 01^st2025

(https://creativecommons.org/licenses/by/4.0 )

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Introduction

mild steel seeks to explore the combined effects

of CLE and iodide inhibitors on steel corrosion in

acidic solutions, employing weight loss methods,

XRD analysis, and UV-Vis spectroscopy.

Mild steel is commonly utilized in mechanical

applications because of its excellent mechanical

properties

and

cost-effective

production.

Nonetheless, mild steel is particularly prone to

corrosion, especially when exposed to acidic

environments like HCl solutions commonly used

in metal cleaning and processing industries [1].

Therefore, preventive measures must be taken to

reduce rust. Here are some other materials that

can be used as anti-rust agents, such as

Gleichenia linearis burm. leaf extract [2] and

Melastoma candidum D. leaf extract [3]. The

presence of hetero atoms like sulfuric, oxygen, or

nitrogen in relevant molecules, along with

Materials and Methods

Materials

Cinnamon leaf samples, mild steel (AISI 1020),

hydrochloric acid (Smart Lab) p.a, potassium

iodide (EMILD STEELURE® ACS, ISO, Reag. Ph

Eur), deionized water (H₂O), methanol (CH3OH)

p.a, and acetone.

Preparation and Extraction

heterocyclic

compounds

and

π-electrons,

Preparation of cinnamon leaf and the making of

CLE. Fresh cinnamon leaves are taken in Koto Tuo

Pulau Tengah, Kerinci, Jambi, as much as 5 kg,

chopped into pieces and dried at room

temperature until dry, then weighed to obtain

dry powder. 500 g of dried cinnamon leaf powder

is drenched in 3000 mL of methanol p.a for 3

days, at that point sifted. The extract gotten is

influences the effectiveness of inhibitors. These

chemical inhibitors can adhere to the metal

surface and obstruct active sites, which in turn

lowers the corrosion rate [4]. One example of an

effective natural inhibitor is cinnamon leaves.

Cinnamon is a perennial plant that takes a long

time to yield results. The bark of the branches

and trunk steel is the main product of the

cinnamon plant, while the twigs and leaves are

by-products [5]. The bark of cinnamon is widely

utilized by the community, whereas the leaves

have not been optimally utilized. Cinnamon

leaves are rich in various compounds, including

vanished

employing

a

revolving

evaporator (HEIDOLPH w200).

Weight Loss Method

The corrosion rate was decided utilizing weight

loss method, considering the influence of

temperature, by immersing steel in 50 mL of 1 M

HCl medium solution with various concentrations

of CLE and addition of potassium iodide with

temperature variation (30, 40, 50, and 60^oC). Steel

was soaked using a water bath for 7 hr. Then

cleaned, cleaned and dried using an oven. After

drying, the steel is weighed and the weighing

result was communicated as the ultimate weight

(m₂). The corrosion rate was calculated according

to equation 1.

flavonoids,

phenolics,

alkaloids,

and hydroquinone

saponins,

[6].

tannins,

These

compounds have demonstrated the ability to

inhibit corrosion, as evidenced by previous

studies of Mikania micrantha extract [7] and

Cardaria draba extract [8]. The synergistic effect

for halides is ordered as follows: I⁻ > Br⁻ > F⁻ > Cl⁻.

Combining iodide with organic inhibitors can

improve the effectiveness of corrosion inhibition

for mild steel in harsh conditions, as iodide ions

offer benefits like larger atomic size and easier

polarization [9]. This study aims to see how

effective small amounts of potassium iodide and

CLE are at preventing corrosion on mild steel, as

well as their synergistic effects that provide

valuable insights into strategies for inhibiting

corrosion of mild steel in acidic environments.

This research focuses on the synergistic effects of

potassium iodide and CLE in HCl media, aiming to

m₁- m₂

A. t

(1)

V_corr

=

Where m₁and m₂are the sample weights prior to

and following immersion in the corrosive

solution, and V_corrstands for the corrosion rate.

Respectively, A denotes

and t is the immersion time in hours. The

inhibitor efficiency (IE%) was determined

according to equation 2.

the

exposed

area,

develop

practical

methods

for

corrosion

inhibition in mild steel applications. This study on

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Rohil et al.

Chempublish Journal, 9(1) 2025, 65-73

V_corr(blank)-V

^corr(inh)×100%

(2)

10 g/L CLE for 7 days, as well as with the addition

of 0.4 g/L potassium iodide. After soaking, the

steel was dried, and the adhered layer was

scraped off the surface. This measurement aims

to confirm the nearness of a defensive layer

formed by CLE on the steel surface, which makes

a difference avoid the destructive medium from

association with the metal.

(

)

EI % =

V_corr(blank)

Where V_corr(blank)and V_corr(inh)represent the

corrosion rate without and with the inhibitor in

the HCl solution, respectively.

Spectroscopy UV-Vis Analysis

The steel was submerged in a 1 M HCl corrosive

Result and Discussion

liquid

in

order

to

perform

UV-Vis

spectrophotometric

measurement

with or

Analysis Using Weight Loss Method

without 10 g/L CLE and 0.4 g/L potassium iodide,

for 7 days. After soaking in the solution, it was

then taken and measured at wavelengths

between 200 and 800 nm using a UV-Vis

spectrophotometer. This measurement was also

carried out for 1 M HCl only by soaking without

adding CLE. The purpose of these measurements

is to see how the inhibitor components (CLE and

potassium iodide) form coordination complexes

with the steel surface.

Weight loss data for different CLE concentrations

at various temperatures can be utilized to

determine the corrosion rate and inhibition

efficiency values. Figures 1 and 2 show that the

corrosion

rate

decreases

as

the

CLE

concentration increases. However, with the

addition of potassium iodide, the corrosion rate

increases with rising temperature during the 7

hours immersion period. This decrease in

corrosion rate indicates that CLE is effective in

inhibiting corrosion in an HCl acid medium. This

inhibitory effect occurs because the CLE extract

adheres to the steel surface [10].

X-Ray Diffraction (XRD) Analysis

XRD

measurements

were

conducted

by

immersing the mild steel in a 1 M HCl corrosive

medium, both without and with the addition of

6

5

4

3

2

1

0

100

80

303 K

313 K

323 K

333 K

60

40

20

0

2

4

6

8

10

CCLE (g/L)

Figure 1. Effect of CLE concentration on inhibition efficiency (%) and corrosion rate (V_corr) in 1 M HCl at

diverse temperatures.

Figures 1 and 2 show that the higher the

concentration, the higher the efficiency. and the

higher temperature, the higher the efficiency.

The addition of iodide synergistically increases an

inhibition efficiency with an addition of 10 g/L of

CLE as an inhibitor, the inhibition efficiency

reaches 92.8% at a temperature of 60°C, adding

0.04 g/L of iodide boosts the inhibition efficiency

to 97.06%. Higher iodide concentrations lead to

more molecules being adsorbed onto the metal

surface [11,12].

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Chempublish Journal, 9(1) 2025, 65-73

Figure 2. Effect of CLE and potassium iodide concentration on inhibition efficiency (%) and corrosion rate

(V_corr) in 1 M HCl at different temperatures.

Adsorption Isotherm

The Langmuir isotherm condition as illustrated in

equation 3.

Adsorption isotherm mild steel explains how the

inhibitor engages with the carbon steel surface.

Among the various adsorption isotherm models

examined, counting Temkin, Freundlich, and

Langmuir, the Langmuir model seems to be the

most suitable which can be seen in Table 1.

Because, the coefficient of determination (R²)

values approaching 1 clearly demonstrate this.

C

θ

1

K_ads

(3)

=

+ C

where K_adsadvertisements speaks to The

harmony consistent for the adsorption prepare,

where C speaks to the inhibitor concentration

and θ demonstrates the surface scope [2,13].

Table 1. Determination coefficient (R²) values for different adsorption isotherms.

Coefficient of determination (R²)

Temperature

(K)

Langmuir

0.9997

0.9992

0.9999

Freundlich

0.9975

Temkin

0.9970

0.9713

0.7301

0.9710

303

313

323

333

0.9998

0.9996

0.9999

Figure 3. Exhibits a linear correlation between

C/θ and C in the 303–333 K temperature range.

As seen by Table 1, this linear relationship implies

that the adsorption of inhibitor compounds is

more consistent with the Langmuir adsorption

model than with alternative isotherm models.

The Langmuir adsorption isotherm is employed

because the coefficient of determination (R²) is

near 1. This shows that the molecules stick to the

mild steel surface in a single layer, implying that

the produced layer is a single layer (monolayer).

Moreover, the connection between the CLE and

potassium iodide compounds and the mild steel

is stronger [14].

The K_adsvalue is derived from the captured of the

linear condition delineated in Figure 3. The

adsorption strength of potassium iodide and CLE

on the mild steel surface is indicated by this

number. The calculation of ∆G_adscan be derived

from the K_adsconstants, which were observed

according to the formulation described in

equation 4.

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Chempublish Journal, 9(1) 2025, 65-73

Figure 3. The inhibitor is Langmuir adsorption graphs at various temperatures on a mild steel surface in

a 1 M HCl solution.

∆G_ads=RTln (C_{H O}K_ads

)

(4)

In this context, ∆H_adsrepresents the enthalpy of

adsorption (kJ/mol), ∆Gads represents the Gibbs

free energy (kJ/mol), ∆Sads indicates the entropy

of adsorption (J/mol), and T stands for the

temperature (K). Table 2. Show that the

∆H_adswhich is probably why the adsorption

entropy has a positive sign. The adsorption

process is characterized by its endothermic

nature indicates the dominance of chemical

adsorption. The positive ∆S_adsvalue indicates a

decrease in disorder. When the inhibitor adsorbs

onto the steel surface in an acidic solution, the

2

Where, R is the molar gas constant (8.314 J

mol⁻¹K⁻¹) C_{H O}is the water content (1000 g/L),

2

and. A negative ∆Gads value between from -20 to

-40 kJ/mol indicates that both physisorption and

chemisorption processes are involved in are

involved in the spontaneous adsorption process.

During the adsorption process at the solid-liquid

interface, molecules of the solute and solvent can

both stick to the CLE surface [15]. The value

of ∆G_adscan be used to determine the enthalpy

( ∆H_ads) and entropy ( ∆S_ads) of adsorption, as

calculated using equation 5.

number

of

adsorbed

inhibitor

molecules

increases relative to the number of water

molecules that leave the surface [8,16,17].

ΔH_ads- ΔG_ads

T

(5)

ΔS_ads

=

Table 2. The Langmuir isotherm is used to calculate the thermodynamic parameters for the adsorption

of CLE on mild steel in a 1 M HCl setup at various temperatures.

Temperature(K)

K_ads

ΔG^o_ads(kJ/mol)

-31.632

ΔH^o_ads(kJ/mol)

ΔS^o_ads(J/mol.K)

303

313

323

333

284.284

185.410

241.558

627.963

-31.564

-33.283

-36.958

21.966

174.010

Thermodynamic Parameters Activation

plotting the relationship between 1/T and ln V_corr

of steel at various temperatures.

The Arrhenius condition (equation 6) can be

utilized to decide the activation energy by

E_a

(6)

ln V_corr= ln A -

RT

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Chempublish Journal, 9(1) 2025, 65-73

Where A speaks to the recurrence figure,

E_adenotes the activation energy (kJmol^-1), and T

stands for temperature (K).

acidic conditions that are suppressed and those

that are not are shown in Table 3. In the absence

of CLE and with potassium iodide present, the

activation energy is greater than that observed in

the inhibited solution. As temperatures rise, the

amount of surface area occupied by CLE

increases, and the presence of potassium iodide

may lead to an imprecise reduction in E_a,

modifying the erosion energy by advertising

elective chemical pathways that have lower

enactment energies ⁸.

In Figure 4, the natural logarithm of the corrosion

rate (ln (CR/T)) is plotted against the inverse of

the absolute temperature (1/T). The slopes of the

Arrhenius and transition state conditions can be

used to determine the activation energy (E_a) and

activation

enthalpy

(∆H_ads).

The

findings

pertaining to metal corrosion mechanisms in

Figure 4. Charts of Arrhenius plots outlining the disintegration rates of mild steel in a 1 M HCl

arrangement, both within the nonappearance and nearness of CLE with potassium iodide at distinctive

concentrations.

To find the values of ∆H* and ∆S*, the Arrhenius

condition can be utilized (7).

endothermic response. This recommends that

the erosion prepare requests a significant sum of

energy³. Meanwhile, the ΔS* values watched both

with and without the tested extract were found

to be negative, demonstrating that the rate-

determining step including the actuated complex

is characterized by affiliation instead of

separation. This suggests that the activated

molecules exist in a more disordered state

V

R

Nh

∆S*

R

∆H*

RT

(7)

ln ^corr= [ln (

) +

] -

T

Where N is Avogadro's number (6.023 × 10²³), h is

Planck's consistent (6.63 × 10⁻³⁴), ∆S* represents

the

variation

in

entropy

(J

mol⁻¹

K⁻¹),

and ∆H* denotes the enthalpy variation (J mol⁻¹

K⁻¹).^{18 19}. Table 3. show that the positive ΔH*

esteem shows that the method was an

relative to their initial condition⁴¹¹

.

Table 3. Values for activation energy (Ea), activation enthalpy (ΔH*), and activation entropy (ΔS*).

Potassium Iodide

concentration (g/L)

Activation Energy

(Ea) (kJ/mol)

55.481

Activation Enthalpy

(ΔH*) (kJ/mol)

55.481

Activation Entropy

(ΔS*) (J/mol.K)

-63.956

0

0.1

0.2

0.3

0.4

19.851

18.816

17.024

11.362

19.851

18.816

17.024

11.362

-194.448

-198.855

-205.520

-225.399

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Chempublish Journal, 9(1) 2025, 65-73

Synergistic Effect. With adding potassium iodide

results

in

increased

inhibition

efficiency

Table 4. Synergistic effect values of MLE

increases compared to using CLE by itself. The

equation below is used to determine the

synergistic effect, as shown in equation 8 [14].

combined with potassium iodide at 60^oC

Potassium iodide

Concentration (g/L)

Synergistic Effect

(S)

1 − θ₁₊₂

(8)

0

-

푆₁=

1 − θ`₁₊₂

0.1

0.2

1.553

1.550

Where, S represent synergism. θ₁indicates the

amount of surface coverage by iodide ions, θ₂

denotes the level of coverage on the surface by

CLE, and θ`₁₊₂reflects the total surface scope

combining iodide ions and CLE. A synergistic

effect value (S) exceeding 1 signifies a synergistic

interaction between CLE and potassium iodide,

as can be seen in Table 4. This suggests that the

combination of CLE wich potassium iodide is

more efficient in inhibiting corrosion compared

to when used separately [16,20]. An S value

greater than 1 signifies a synergistic relationship,

whereas an S value less than 1 signifies an

antagonistic relationship and an S value = 1

0.3

0.4

1.424

1.420

UV-Vis Analysis

UV-Vis analysis was conducted on mild steel to

determine the interaction of the inhibitor

complex with the steel surface. As shown in

Figure 5, the UV-Vis spectrum of the HCl solution

with steel (Figure 5a) exhibits a peak at 337 nm.

In contrast, the spectrum of the HCl solution with

CLE extract (Figure 5b) shows an absorption peak

at 314 nm. Meanwhile, the mixture of CLE extract

and steel (Figure 5c) displays a peak at 322 nm.

indicates

no

synergistic

or

antagonistic

relationship between the compounds [4,21].

2.5

c

2.0

1.5

1.0

0.5

0.0

d

b

a

200

400

600

800

1000

1200

Wavelength (nm)

Figure 5. UV-Vis Spectra (a) 1 M HCl + mild steel, (b) 1 M HCl + CLE 10 g/L, (c) 1 M HCl + CLE 10 g/L + mild

steel, and (d) 1 M HCl + CLE 10 g/L + potassium iodide 0,4 g/L + mild steel.

This absorption peak is associated with an n→π*

electronic transition of the C=O group present in

the CLE extract [22]. Additionally, the UV-Vis

range of the CLE extract arrangement with steel

and the expansion of potassium iodide (d)

appears a top at 317 nm. This top move

demonstrates the creation of a coordination

complex including the components of the CLE

extract with steel all through the dousing handle

[14]. XRD Analysis. X-Ray Diffraction (XRD) the

investigation was conducted on mild steel to

decide the compounds show within the detached

layer shaped on its surface. Figure 6 (a) shows

several peaks indicating the presence of iron

oxides, namely Fe₂O₃and Fe₃O₄. Additionally,

FeCl₂is also present, shaped as a result of the

interaction of chloride particles with the

substrate [23]. Figure 6 (c) shows no intensity

peaks of FeCl₂, indicating that CLE can reduce the

corrosion process by forming a protective layer

on the steel surface and preventing the corrosive

medium HCl from interacting with the mild steel

surface. Figure 6 (b) shows a small amount of iron

oxide and the appearance of FeI₂peaks.

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Chempublish Journal, 9(1) 2025, 65-73

a

b

c

0

20

40

60

80

100

2 (Degree)

Figure 6. XRD designs (a) mild steel submerged in 1 M HCl, (b) mild steel submerged in 1 M HCl + CLE 10

g/L + potassium iodide 0.4 g/L, and (c) mild steel submerged in 1 M HCl + CLE 10 g/L.

Conclusions

acquisition, critically reviewed, writing initial

draft, data analysis, editing, and revising.

Cinnamon leaf remove and potassium iodide mix

act has been showed up to be a practical

disintegration inhibitor for delicate steel in a 1 M

HCl course of action. An increment in

temperature and the incorporation of iodide

leads to progressed restraint productivity due to

a result of synergistic impact. The Langmuir

adsorption isotherm is used to alter the CLE is

adsorption behavior. The synergistic parameter

(S), analyzed at different iodide concentrations.

The esteem was decided to surpass one,

recommending that the improved hindrance

effectiveness watched with iodide particles is due

to their synergistic interaction.

Conflict of interest

The authors declare no conflict of interest.

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