Principles of Instrumental Analysis
7th Edition
ISBN: 9781305577213
Author: Douglas A. Skoog, F. James Holler, Stanley R. Crouch
Publisher: Cengage Learning
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Chapter 14, Problem 14.22QAP
Mixing the chelating reagent B with Ni(II) forms the highly colored NiB22+, whose solutions obey Beer’s lawat 395 nm overa wide range. Provided the analytical concentration of the chelating reagent exceeds that of Ni(II) by a factor of 5 (or more), the cation exists, within the limits of observation, entirely in the form of the complex. Use the accompanying data to evaluate the formation constant Kf for the process
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Chapter 14 Solutions
Principles of Instrumental Analysis
Ch. 14 - Prob. 14.1QAPCh. 14 - A 0.4740-g pesticide sample was decomposed by wet...Ch. 14 - Sketch a photometric titration curve for the...Ch. 14 - Prob. 14.4QAPCh. 14 - Prob. 14.5QAPCh. 14 - The accompanying data (1.00-cm cells) were...Ch. 14 - A 3.03-g petroleum specimen was decomposed by wet...Ch. 14 - Prob. 14.8QAPCh. 14 - Prob. 14.9QAPCh. 14 - The acid-base indicator HIn undergoes the...
Ch. 14 - Prob. 14.11QAPCh. 14 - Prob. 14.12QAPCh. 14 - Copper(II) forms a 1:1 complex with the organic...Ch. 14 - Aluminum forms a 1:1 complex with...Ch. 14 - Prob. 14.15QAPCh. 14 - Prob. 14.16QAPCh. 14 - Prob. 14.17QAPCh. 14 - Prob. 14.18QAPCh. 14 - Prob. 14.19QAPCh. 14 - Given the Information that...Ch. 14 - Prob. 14.21QAPCh. 14 - Mixing the chelating reagent B with Ni(II) forms...Ch. 14 - Prob. 14.23QAP
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- A 3.03-g petroleum specimen was decomposed by wet ashing and subsequently diluted to 500 mL in a volumetric flask. Cobalt was determined by treating 25.00-mL aliquots of this diluted solution as follows: Assume that the Co(II)-ligand chelate obeys Beer’s law, and calculate the percentage of cobalt in the original sample.arrow_forwardCalculate 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 10-11arrow_forwardA 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?arrow_forward
- A transition metal ion, M, forms a coloured complex with a monodentate ligand L. Portions of a 0.05 mol dm-³ solution of M are mixed with portions of a solution containing 0.05 mol dm-³ of L so that the total volume of the resulting mixture is always 10 cm³. The colour intensity of the complex in each mixture is measured using a colorimeter. The graph of the results is 0 1 2 3 3 4 5 6 7 8 9 10 cm³ of M 10 9 8 7 6 5 4 3 2 1 0 - cm³ of L What is the formula of the complex? A ML B ML₂ C ML₂ с D D ML4 Colour intensity 7:2arrow_forward(a) Write the electronic configuration of Ce3+ ion, and calculate the magnetic moment on the basis of ‘spin-only’ formula. [Atomic No. of Ce = 58] (b) Account for the following: (i) Thf enthalpies of atomisation of the transition metals are high. (ii) The lowest oxide of a transition metal is basic, the highest is amphoteric/ acidic. (iii) Cobalt (II) is stable in aqueous solution but in the presence of complexing agents, it is easily oxidised.arrow_forwardThe 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.<arrow_forward
- (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 cmarrow_forwardThe observed absorption band of the M2+ ion in the electronic spectrum of the hexaaqua complex is 7500 cm-1. How many kJ / mol is the crystal field cleavage of the tetraaqua complex of the same ion? (h = 6,626x10-34Js, c = 3x108ms-1)arrow_forwardA method different from the method of Job to determine the coordination number of a complex is to measure the shift in polarographic half-wave potential Ex of a metal ion M²* to more negative values during complex formation as a function of the concentration of the added ligand L. A good example is complex formation between Cd²+ and NH3 to which the equation E-(E), = 0.0591 2 [NH3J/mol L-1 0 Ey/V log [NH3] {Ex-(Ex)s}/V n= applies, where (E₁), is the half-wave potential of the free Cd²+ metal ion (i.e. in the absence of the ligand NH3), and K and n, as before, are the formation constant and coordination number of the resulting complex Cd (NH3)², respectively. Use the tabled values below and the supplied graph paper to determine the coordination number and molecular formula of the complex by plotting E-(E), versus log[NH3] and calculating n from the slope of the straight line graph. formula: 0.0592 2 log K-n- -log[NH,] -0.752 3.14 -0.840 3.86 -0.856 4.75 -0.872 7.20 -0.904 8.86 -0.920arrow_forward
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