Dear Bahman,

In principle yes, it is possible. The following publications demonstrate the use of FTIR along with other analytical methods to unravel the adsorption mechanisms of some chemical entities using fresh and old samples:

1-FTIR, UV-Vis, and HRTEM Study of Au/ZrO2 Catalyst: Reduced Reactivity in the CO-O2 Reaction of Electron-Deficient Gold Sites Present on the Used Samples

F. Boccuzzi,*,† G. Cerrato,† F. Pinna,‡ and G. Strukul‡

J. Phys. Chem. B, Vol. 102, No. 30, 1998

A Fourier transform infrared (FTIR), UV-vis, and high-resolution transmission electron microscopy (HRTEM) study of fresh and used Au/ZrO2 catalyst is reported. FTIR data show that on a fresh sample CO is adsorbed on regular gold metallic sites, while on the used sample the adsorption sites are bidimensional gold clusters

made positive by interaction with the support. NIR-UV-vis reflectance spectra show that the gold plasmonic peak appears broader and the ZrO2 absorption edge weaker on the used sample with respect to the fresh one. HRTEM indicates the disappearance of the gold metallic particles in the used catalysts. Moreover, a strong reduction in the CO oxidation activity has been evidenced on the used sample and ascribed to the positivization of gold and/or to the decrease of the number of highly uncoordinated gold sites, consistently with the spreading

of gold at the support surface.

http://pubs.acs.org/doi/pdfplus/10.1021/jp980890t?src=recsys

2-Application of FTIR Spectroscopy in Environmental Studies

Claudia Maria Simonescu 

http://cdn.intechopen.com/pdfs/38543/InTech-Application_of_ftir_spectroscopy_in_environmental_studies.pdf

3-A Comparison Study of Mechanism: Cu2+ Adsorption on Different Adsorbents and Their Surface-Modified Adsorbents

Yaqin Yu, Xinrui Li, and Jiemin Cheng

Journal of Chemistry

Volume 2016 (2016), Article ID 7936258, 8 pages

http://dx.doi.org/10.1155/2016/7936258

Abstract

The isothermal adsorption kinetics of Cu2+ onto Carbon Black (CB) and Oxidized Carbon Black (OCB) were studied under different solution conditions and compared with bentonite and organic bentonite with the hexadecyltrimethylammonium bromide (HDTMA). The adsorption capacities followed the order of OCB > CB > organic bentonite > bentonite, which was consistent with the orders of their surface roughness and specific surface area. The Fourier transmission infrared (FT-IR) spectroscopy, scanning electron microscopy (SEM), and transmission electron microscope (TEM) were used to explore the adsorption mechanism at molecular level. The adsorption process onto CB was physical adsorption. However, with the increase of oxygen-containing functional groups (C=O, C-O, and CNO), the chelation adsorption onto OCB became gradually dominant except physical adsorption. The ion exchange adsorption was the major adsorption mechanism of bentonite. The compounds were introduced into clay interlayer by complexing reaction with Cu2+, which improved the adsorption capacity of organic bentonite. The results present a significant implication for the environmental fate assessment of heavy metal pollution.

http://www.hindawi.com/journals/jchem/2016/7936258/

4-Biosorption of cadmium and lead from aqueous solution by fresh water alga Anabaena sphaerica biomass

Azza M. Abdel -Aty, Nabila S. Ammar, Hany H. Abdel Ghafar,⁎ and Rizka K. Ali

J Adv Res. 2013 Jul; 4(4): 367–374.

Published online 2012 Aug 14. doi: 10.1016/j.jare.2012.07.004

The present work represents the biosorption of Cd(II) and Pb(II) from aqueous solution onto the biomass of the blue green alga Anabaena sphaerica as a function of pH, biosorbent dosage, contact time, and initial metal ion concentrations. Freundlich, Langmuir, and Dubinin–Radushkevich (D–R) models were applied to describe the biosorption isotherm of both metals by A. sphaerica biomass. The biosorption isotherms studies indicated that the biosorption of Cd(II) and Pb(II) follows the Langmuir and Freundlish models. The maximum biosorption capacities (qmax) were 111.1 and 121.95 mg/g, respectively, at the optimum conditions for each metal. From the D–R isotherm model, the mean free energy was calculated to be 11.7 and 14.3 kJ/mol indicating that the biosorption mechanism of Cd(II) and Pb(II) by A. sphaerica was chemisorption. The FTIR analysis for surface function group of algal biomass revealed the existence of amino, carboxyl, hydroxyl, and carbonyl groups, which are responsible for the biosorption of Cd(II) and Pb(II). The results suggested that the biomass of A. sphaerica is an extremely efficient biosorbent for the removal of Cd(II) and Pb(II) from aqueous solutions.

http://www.ncbi.nlm.nih.gov/pmc/articles/PMC4293879/

Hoping this will be helpful,

Rafik

Thanks, Rafik

I would say in principle yes, but in practice NO! 

The following problems may happen:

-because the amount of the adsorbed fluoride in comparison with the amount of the adsorbent is not so significant, the FTIR peaks overlaps.

-Even if you physically mix fluoride with the adsorbent you will see the same peaks as for the chemically adsorbed fluoride FTIR peaks.

So, I suggest to use pseudo-first-order and pseudo-second-order kinetic models. If the pseudo-first-order model fitted well the experimental data, you can say that the adsorption was physically controlled, otherwise (pseudo-second-order) it was chemically adsorbed.

Dear Bahman

Adsorption mechanism predicted from UV is common and easy one . 

I hope FTIR is not that much help in your adsorption study. FTIR basically help to find the functional group from your materials . Not able to find the adsorption efficiency. 

FTIR consider one of the tools to confirm , however , the adsorption process ix physcial or chemical . If the vibration is low or the the peaks is slightley shifted or ovelaping this process physcial . if the peak dislocation or significant shiffted , the process will be chemical . in addition , langmiuer , Frundlich , pesudo first order , pesudo second order and interparticle defusion will be extra confirmation

Thank you Nasser.

i think you can use Dubinin-Radushkevich (D-R) isotherm model

The free energy change per mole of ion transferred to the composite surface from endless is known as the mean free energy (E). It can be calculated from β values using the following equation:

E=(2* beta)^-1/2

The calculated value of E can be identifying the reaction mechanism, if

the value of E is less than 8.0 (kJ/mole); the sorption mechanism is

physically forced. If the value of E in the range of 8-16 (kJ/mole), the

sorption is governed by ion exchange. If the value of E is in the range of 16-40 (kJ/mole), the sorption process is controlled by chemisorption

process.

you can find further details in my publication:

Article Evaluation of synthetic aluminum silicate modified by magnes...