Calculate the conditional formation constant of the complex [CuY]*, KNry, in a buffer containing 0.050 M NH3 and 0.090 M NH,Cl given that the%3Dsuccessive formation constants of the copper amines are: K1 = 1.9 x 10, K2 = 3.6 x 10°, K3 = 7.9 x 10- and Ka = 1,5 x 102.Cu2' (aq) + NH3(aq)[Cu(NH,))|Cu(NH3)) + NH3(aq) = [Cu(NH; )2) K2(aq)21|Cu(NH,)2) + NH3(4)[Cu(NH,)s + NH,(a4)[Cu(NH, )3 nc) K3[Cu(NH,)4) K,(aq)213 (aq)(aq)

Given, consecutive formation constant of copper amine. K1 ,K2,K3 and K4.

Answered: Calculate the conditional formation…

Appl Of Ms Excel In Analytical Chemistry

2nd Edition

ISBN:9781285686691

Author:Crouch

Publisher:Crouch

Chapter9: Complexometric And Precipitation Titrations

Section: Chapter Questions

Problem 9P

See similar textbooks

Similar questions

The accompanying data (1.00-cm cells) were obtained for the spectrophotometric titration 10.00 mL of Pd(II) with 2.44 10-4 M Nitroso R(O. W Rollins and M. M. Oldham, Anal. chem .,1971, 43, 262, DOI: 10.1021/ac60297a026). Calculate the concentration of the Pd(II) solution, given that the ligand-to-cation ratio in the colored product is 2:1
Calculate the conditional formation constant (K'' NiY) of the [NiY]2- complex in 0.050 M NH3 and 0.090 M NH4Cl buffer solution. The formation constants of nickel amine complexes are respectively K1 = 102.75, K2 = 102.20, K3 = 101.69, K4 = 101.15, K5 = 100.71, K6 = 10-0.01. (KNiY = 4.2x1018, KNH3 = 1.74x10-5)
The formation constant for the complexation of Mg2+ by EDTA is logKflogKf = 8.79. The conditional formation constant (Kf’) at pH 8 (αY4−αY4−= 4.2 x 10-3) is: 0.037 2.6 x 106 5.14 1.5 x 1011 6.4
The red color of soil is often due to the presence of iron. Metal ions are extracted from soil by stirring the soil in acid and then filtering the solution. One method for the analysis of Fe2+ is to form the highly colored Fe2+–thioglycolic acid complex. The complex absorbs strongly at 535 nm. Calibration standards of 1.00, 2.00, 3.00, 4.00, and 5.00 ppm are prepared by transferring appropriate amounts of a 10.0 ppm working solution of Fe2+ into separate 50-mL volumetric flasks, each of which contains 5 mL of thioglycolic acid, 2 mL of 20% w/v ammonium citrate, and 5 mL of 0.22 M NH3. After diluting to volume and mixing, the absorbances of the standards are measured. a)What is the effect on the reported concentration of iron in the sample if there is a trace impurity of Fe2+in the ammonium citrate?
The red color of soil is often due to the presence of iron. Metal ions are extracted from soil by stirring the soil in acid and then filtering the solution. One method for the analysis of Fe2+ is to form the highly colored Fe2+–thioglycolic acid complex. The complex absorbs strongly at 535 nm. Calibration standards of 1.00, 2.00, 3.00, 4.00, and 5.00 ppm are prepared by transferring appropriate amounts of a 10.0 ppm working solution of Fe2+ into separate 50-mL volumetric flasks, each of which contains 5 mL of thioglycolic acid, 2 mL of 20% w/v ammonium citrate, and 5 mL of 0.22 M NH3. After diluting to volume and mixing, the absorbances of the standards are measured. a)Use the data table below to prepare a calibration curve (absorbance versus concentration in ppm). Fit the data to straight line and find the equation for the straight line and the R2 value. (Hint: Think about what to do with the absorbance of the blank.)
A dual beam UV-visible spectroscopy was used to determine the levels of Fe(II) in the run-off water of a local mine using the ferrozine assay (i) During a check of the instrument a step-like feature at 360 nm was observed in spectrum of the standard. Suggest what may give rise to this with reference to the instrument configuration and comment on how it may be remedied. (ii) The molar absorptivity of the [Fe(Ferrozine)3]2+ complex is 27900 cm−1 M−1 at 562 nm in aqueous solution (pH 5.5). If the EU maximum contaminant level for Fe is 200 ug /L and the contract required detection limit is 100 ug/L, comment on the suitability of the assay for the detection of iron. (iii) Determine the sample range, in terms of concentration and ppm, of Fe(II) that can be confidently analysed by UV-visible spectroscopy using a 1 cm cuvette. Explain with reference to an appropriate equation and solution phenomena, the origin of the limitations that define this range
Describe main features of the evidence of M-CºC characterization and corresponding techniques of this complex (COCL(PPh3)2-III(CF3)2)...?
Give a lab cation separation scheme for Al3+, Ca2+, Ni2+ cations based on Ksp values and complex ion formations (if any).
Find 3 typical organic complexing agents in the environment and describe in which environments (in the widest sense) they are found and which elements are particularly taken up.
Mention 3 typical organic complexing agents in the environment and describe in which environments (in the widest sense) they are found and which elements are particularly taken up.
(i) You have been provided with a sample collected from a water pool beside a slag heap at the iron ore mine. 35 uL of the sample is added to 1165 uL of buffered ferrozine (excess). If the %T recorded at 562 nm in a 2 mm cuvette is found to be 25%, calculate the concentration of Fe(II) in the sample in mol L−1 and ppm. Comment on the contamination level. (ii) Comment on a possible contaminant that could interfere with the assay and suggest an approach that could be used to account for its presence.
The potassium ion in 250 ml of a water sample was first precipitated as potassium tetraphenylborate: K +(aq) + (C6H5)B- (aq)- KB(C6H5)4 (s). washed, dried and dissolved in an organic solvent. treatment of the organic solution with an excess of aqueous solution of the Hg(ii)-edta complex generated the following reaction: 4HgY2- (aq) +KB(C6H5)4(s) + 4H2O ➜H3BO3, (aq) +4C6H5Hg+(aq) + 4HY3- (aq) + K+ (aq) + OH -(aq) The released edta (in the form of HY3-) was fully titrated with 28.73 ml of 0.04xy mol/l zncl2 solution. Determine the concentration in mg/l of potassium in the water sample. xy is 11

SEE MORE QUESTIONS

Recommended textbooks for you

Appl Of Ms Excel In Analytical Chemistry

Chemistry

ISBN:

9781285686691

Author:

Crouch

Publisher:

Cengage

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

Appl Of Ms Excel In Analytical Chemistry

Chemistry

ISBN:

9781285686691

Author:

Crouch

Publisher:

Cengage

Fundamentals Of Analytical Chemistry

Chemistry

ISBN:

9781285640686

Author:

Skoog

Publisher:

Cengage

Principles of Instrumental Analysis

Chemistry

ISBN:

9781305577213

Author:

Douglas A. Skoog, F. James Holler, Stanley R. Crouch

Publisher:

Cengage Learning

SEE MORE TEXTBOOKS