(III) adsorbent (b) Adsorption of the hexacyanoferrate (III) ion, [Fe(CN)6] ³, on y-Al2O3 from aqueous solution was examined. The adsorption was modelled using a modified Langmuir isotherm, yielding the following values of Kat pH = 6.5: (ii) T/K 10-10 K 280 2.505 295 1.819 310 1.364 325 1.050 Determine the enthalpy of adsorption, AadsHⓇ. If the reported value of entropy of adsorption, Aads Se = 146 J K-1 mol-1 under the above conditions, determine Aads Gº.
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- Explain the Coordination Chemistry and Chemical Speciation Utilized in the Analysis of Fluoride in Water Samples by Fluoride Ion-Selective Electrode.Ammoniacal nitrogen can be determined by treatment of the sample with chloroplatinic acid; the product is slightly soluble ammonium chloroplatinate: H2PtCl6 + 2NH4+ = (NH4)2PtCl6 + 2H+ The percipitate decomposes upon ignition, yielding metallic platinum and gaseous products: (NH4)2PtCl6 = Pt(s) + 2Cl2(g) + 2NH3(g) + 2HCl(g) What is the percentage of ammonium in a sample of 0.2213g of sample gave rise to 0.5881g of platinum?Give the formula of each of the following coordination entities :(i) Co3+ ion is bound to one Cl–, one NH3 molecule and two bidentate ethylene diamine (en) molecules.(ii) Ni2+ ion is bound to two water molecules and two oxalate ions.Write the name and magnetic behaviour of each of the above coordination entities.(At nos. Co = 27, Ni = 28)
- At 580 nm, the wavelength of its maximum absorption, the complex Fe(SCN)2+ has a molar absorptivity of 7.00x 103 L cm-1 mol-1. Calculate (a) the absorbance of a 3.40 x 10–5 M solution of the complex at 580 nm in a 1.00-cm cell. (b) the absorbance of a solution in which the concentration of the complex is twice that in (a). (c) the transmittance of the solutions described in (a) and (b). (d) the absorbance of a solution that has half the transmittance of that described in (a).At 580 nm, the wavelength of its maximum absorption, the complex Fe(SCN)2+ has a molar absorptivity of 7.00 X 103 L mol-1 cm-1. Calculate (a) the absorbance of a 2.50 X 10-5 M solution of the complex at 580 nm in a 1.00-cm cell. (b) the absorbance of the solution in which the concentration of the complex is twice that in part (a) (c) the transmittance of the solutions described in parts (a) and (b) (d) the absorbance of a solution that has half the transmittance of that described in part (a) answer letter d pleaseAt 580 nm, the wavelength of its maximum absorption, the complex Fe(SCN)2+ has a molar absorptivity of 7.00 X 103 L mol-1 cm-1. Calculate (a) the absorbance of a 2.50 X 10-5 M solution of the complex at 580 nm in a 1.00-cm cell. (b) the absorbance of the solution in which the concentration of the complex is twice that in part (a) (c) the transmittance of the solutions described in parts (a) and (b) (d) the absorbance of a solution that has half the transmittance of that described in part (a)
- (a) The spectrochemical series of (a) Fe³+, (b) Co²+ and (c) Mn²+ ions follow the order: (b) Benzene is a field ligand relative to NH3 in the spectrochemical series. (c) For an octahedral Co³* complex with A. = 24,000 cm¹ and pairing energy per electron pair, P = 14,000 cm¹, the CFSE is m-¹. (enter final answer only). OR cmA solution containing the complex formed between Bi(III) and thiourea has a molar absorptivity of 9.32 x 103 M-1 cm-1 at 470 nm. (a) Calculate the absorption of a 4.25x10-5 M solution of the complex at 470 nm in a 1-cm cell. (b) What is the molar concentration of the complex in a solution that has the calculated absorption in (a) when measured at 470 nm in a 2.50 cm cell?Calculate the equilibrium concentration of Ni²* in a solution with an analytical NİY2- concentration of 0.0100 M at pH 2.0 and pH 9.0. Kr of NIY2= 4.2 x 1018 HẠY Dissociation Constants: Ka1 =1.02 x 10² Ka2 =2.14 x 103 Ka3 =6.92 x 10-7 Ka4 =5.50 x 10-11
- The mineral magnetite has the formula Fe3O4 and has an inverse spinel structure. In the unit cell, there are two Fe ions in octahedral sites and one Fe ion in a tetrahedral site. (i) Are the Fe ions in magnetite low-spin or high-spin? Explain your reasoning. (ii) Draw d-orbital splitting diagrams for Fe(III) in tetrahedral and octahedral ligand fields and hence deduce the CFSE in each case. (iii) On the basis of your answer to part (ii) above, do you expect Fe(III) to have a preference for tetrahedral or octahedral sites? Explain your answer. (iv) Draw d-orbital splitting diagrams for Fe(II) in tetrahedral and octahedral ligand fields and hence deduce the CFSE in each case. (v) Assuming that Δt ~ 4/9 Δo and using your answer to part (iv) above, deduce the CFSE of Fe(II) in a tetrahedral field in terms of Δo. Hence decide whether the tetrahedral site is occupied by Fe(II) or Fe(III), explaining your reasoning.The equilibrium constant for the following reaction is 1.0 x 1023. Cr+ (aq) + H₂EDTA² (aq) CrEDTA (aq) + 2H+ (aq) O₂C-CH₂ CH, CO, O₂C-CH₂ CH, C, EDTA- N-CH₂-CH₂-N) Ethylenediaminetetraacetate EDTA is used as a complexing agent in chemical analysis. Solutions of EDTA, usually containing the disodium salt Na₂H₂ EDTA, are used to treat heavy metal poisoning. Calculate [Cr] at equilibrium in a solution originally 0.0050 M in Cr³+ and 0.040 M in H₂EDTA and buffered at pH 6.00. Assume that H₂ EDTA form dominates at this pH. = [Cr³+) | MThe stepwise formation constants for complexes of NH3 with [Cu(OH2)6]2+(aq) are log Kfl = 4.15, log Kf2 = 3.50, log Kf3 = 2.89, log Kf4 = 2.13, and log Kf5 = −0.52. Suggest a reason why Kf5 is so different.<