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 14.7QAP
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.
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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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- Platinum(II) forms many complexes, among them those with the following ligands. Give the formula and charge of each complex. (a) two ammonia molecules and one oxalate ion (C2O42-) (b) two ammonia molecules, one thiocyanate ion (SCN-), and one bromide ion (c) one ethylenediamine molecule and two nitrite ionsarrow_forwardOne of the following nitrogen compounds or ions is not capable of serving as a ligand: NH4+, NH3, NH2. Identify this species, and explain your answer.arrow_forwardTwo different coordination compounds containing one cobalt(III) ion, five ammonia molecules, one bromide ion, and one sulfate ion exist. The dark violet form (A) gives a precipitate upon addition of aqueous BaCl2. No reaction is seen upon addition of aqueous BaCl2 to the violet-red form (B). Suggest structures for these two compounds, and write a chemical equation for the reaction of (A) with aqueous BaCl2.arrow_forward
- 3a) The nitrosyl ion, NO*, is a very rare case of a cationic ligand that can function as a Lewis base. Draw the Lewis structure of this ligand under consideration of the VSEPR rules and indicate any formal charges on the constituent atoms. 3b) How many electrons does the NO* ligand contribute on the ionic model and the neutral model, respectively? Assume that the Metal-N-O bonding angle is 180° upon coordination.arrow_forwardgive an example of hexadentate ligand.arrow_forward(b) Consider the oxalate (ox) ligand and answer the following questions:(i) Draw the structure of the ox ligand.(ii) Identify all the donor atoms of the ligand.(iii) What is the denticity of the ligand?(iv) What is the charge of the ligand?(v) Draw the structure of a homoleptic octahedral complex with ox as the ligand.Clearly show the geometry at the metal centre.(vi) Identify the stereoisomer in the structure drawn.arrow_forward
- A coordination compound has been determined to be composed of 18.4% Co, 26.6% NH3, 30.0% SO4 , and 25.0% Br–, by mass. The compound was also determined to have two different isomers, A and B, such that the solution of isomer-A was found to react with AgNO3(aq) to produce AgBr precipitate, but the reaction with Ba(NO3)2(aq) did not produce any precipitate. While the solution of isomer-B did not produce any precipitate when reacted with AgNO3(aq), but it produced BaSO4 precipitated when the solution is reacted with Ba(NO3)2(aq). (a) Determine the empirical formula of the compound written in the form of Co(NH3)x(SO4)yBrz. (b) Assuming that all of NH3 molecules in the formula are ligands, deduce the Werner’s formula for isomers A and B, respectively, and give the systemic name for each isomer.(c) Write molecular equations for the reaction of each isomer with AgNO3(aq) and Ba(NO3)2(aq).arrow_forwardThe complex [Fe(CO)6]+2 exhibits π-acceptor behavior. Using ligand field theory, draw the molecular orbital diagram mixing the d-orbitals on the metal and the molecular orbitals on the ligands and fill in the available electrons. What is the nature of the t2g orbitals that are part of Δo, bonding, antibonding, or non-bonding? Explain your answer. Is this molecule high spin or low spin? Explain your answer.arrow_forwardUse the data provided for stock concentration and mass to calculate the concentrations of each solution. Solution A) A stock solution of 0.0100 M solution of K3[Fe(CN)6] is provided. Calculate the volume of the stock solution needed to prepare 100.0 ml of .00200 M K3[Fe(CN)6]. Deionized water should be used to dilute the solution. Solution B) Calculate the volume of solution A needed to prepare 50.0 ml of .0010 M K3[Fe(CN)6]. Deionized water should be used to dilute this solution.arrow_forward
- Balance this equation and balanced reaction equation and the quantities included in the procedure to calculate the theoretical yield of K[Cr(C2O4)2(H2O)2]·2H2O.arrow_forwardA coordination compound has the following composition (by mass %): 23.53% Co; 42.47% Cl, and 34.00% NH3. When 4.91 g of the compound is dissolved in 75.0 mL of deionized water, and the solution is reacted with an excess of AGNO; solution, it yields 5.60 g of AgCl precipitate. (a) Determine the empirical formula of the compound and write in the form of Co(NH;),Cl, (where x and 24. y are simple integers), and calculate its molar mass. (Assume the compound contains only one Co atom). (b) Deduce the number of chloride (Cl) as counter ions and as ligand, respectively. (c) Write the Werner's formula of the compound and give its systematic name. (Answers: (a) Co(NH3);C13; molar mass = 250.43 g/mol; (b) 2 Cl are counter ions and one is ligand; (c) [Co(NH3);CI]Cl2 = pentaammonechlorocobalt(III) chloride)arrow_forward
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