Consider the data for the determination of phosphorus in urine as the phosphomolybdate complex, which has a maximum absorbance at 650 nm. 43 1.2 1 0.8 0.6 0.4 0.2 1 2 3 4 6 conc. of P. Dom Below is the generated titration curve from an external standard calibration method in the analysis of phosphorus in soil. Identify the concentration of phosphorus in a gram of sample that has an absorbance of 0.500 at a wavelength of 650 nm. absorbance

Consider the data for the determination of phosphorus in urine as the phosphomolybdate complex, which has a maximum absorbance at 650 nm. 43 1.2 1 0.8 0.6 0.4 0.2 1 2 3 4 6 conc. of P. Dom Below is the generated titration curve from an external standard calibration method in the analysis of phosphorus in soil. Identify the concentration of phosphorus in a gram of sample that has an absorbance of 0.500 at a wavelength of 650 nm. absorbance

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter26: Molecular Absorption Spectrometry

Section: Chapter Questions

Problem 26.5QAP

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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.)
the spectrochemical series allows us to explain the variety ofcolors observed in transition metal complexes. But in practice, someone attempting to predictthe properties of compounds can occasionally be frustrated by various complicating factors.For instance, the nitrite ligand is presented as having a high field strength, but that is only whenit is the nitrogen of the nitrite that is coordinating to the metal center. Nitrite is also capable ofbinding to the metal center through an oxygen, and when this happens, nitrite is a low fieldstrength ligand. Furthermore, many metals initially precipitate as simple ionic salts before theyhave a chance to form more soluble complex ions. And occasionally, unexpected redoxreactions can lead to complex mixtures. Despite these complications, the spectrochemical series remains a powerful predictivetool for inorganic chemists. New ligands are being developed all the time, and each new ligandneeds to be placed, at least approximately, on the…
the spectrochemical series allows us to explain the variety ofcolors observed in transition metal complexes. But in practice, someone attempting to predictthe properties of compounds can occasionally be frustrated by various complicating factors.For instance, the nitrite ligand is presented as having a high field strength, but that is only whenit is the nitrogen of the nitrite that is coordinating to the metal center. Nitrite is also capable ofbinding to the metal center through an oxygen, and when this happens, nitrite is a low fieldstrength ligand. Furthermore, many metals initially precipitate as simple ionic salts before theyhave a chance to form more soluble complex ions. And occasionally, unexpected redoxreactions can lead to complex mixtures. The complex that copper forms with chloride ions is tetrahedral. Write the chemical formula for this complex. Thoroughly describe the energy diagram for the d orbitals.
the spectrochemical series allows us to explain the variety ofcolors observed in transition metal complexes. But in practice, someone attempting to predictthe properties of compounds can occasionally be frustrated by various complicating factors.For instance, the nitrite ligand is presented as having a high field strength, but that is only whenit is the nitrogen of the nitrite that is coordinating to the metal center. Nitrite is also capable ofbinding to the metal center through an oxygen, and when this happens, nitrite is a low fieldstrength ligand. Furthermore, many metals initially precipitate as simple ionic salts before theyhave a chance to form more soluble complex ions. And occasionally, unexpected redoxreactions can lead to complex mixtures. Despite these complications, the spectrochemical series remains a powerful predictivetool for inorganic chemists. New ligands are being developed all the time, and each new ligandneeds to be placed, at least approximately, on the…
By using the given 1) electronic absorption spectrum, 2) the Tanabo-Sugano diagram for d3 complex in octahedral ligand field and 3) the absorption/emission spectra, explain the following: a) Ligand field states (to support your explanation show the filling of the orbitals) b) Radiative transitions (to support your explanation refer to fluorescence, phosphorescence and Stokes’ shift)
An aqueous solution of compound X was placed in a cuvette 1 cm thick and its light absorption (lambda=366 nm) was determined in 04 different concentrations. Experimental data are presented in the Table below: Determine the coefficient of molar extinction.
Describe main features of the evidence of M-CºC characterization and corresponding techniques of this complex (COCL(PPh3)2-III(CF3)2)...?
palladium complexes containing the thiocyanate anion as a ligand were studied. Initially, the square planar [Pd(AsPh3)2(SCN)2] complex was synthesized and this was isomerized to [Pd(AsPh3)2(NCS)2] at elevated temperatures and these two complexes were characterized by infrared spectroscopy. To prove with absolute certainty that the changes they observed in the infrared spectra were due to the linkage isomerism of the thiocyanate ligands, they also synthesized and characterized [Pd(bipy)(SCN)2] and [Pd(bipy)(NCS)2], as well as [Pd(bipy)2][Pd(SCN)4] a. Why was it important that they used the bipy ligand instead of the AsPh3 ligands in this study? What type of isomerism would it prohibit from occurring? b. What type of isomerism is observed when comparing [Pd(bipy)(SCN)2] and [Pd(bipy)2][Pd(SCN)4]? Please draw both of the complexes as part of the explanation of your answer.
How does the coordination geometry of a metal center influence its reactivity in bioinorganic chemistry? Provide an example to illustrate your answer. asap give correctly or else downvote
When Alfred Werner was developing the field of coordinationchemistry, it was argued by some that the opticalactivity he observed in the chiral complexes he hadprepared was due to the presence of carbon atoms in themolecule. To disprove this argument, Werner synthesizeda chiral complex of cobalt that had no carbon atoms in it,and he was able to resolve it into its enantiomers. Design acobalt(III) complex that would be chiral if it could be synthesizedand that contains no carbon atoms. (It may not bepossible to synthesize the complex you design, but we willnot worry about that for now.)
Titanium and vanadium form colored complexes when treated with hydrogen peroxide in 1 M sulfuric acid. The titanium complex has an absorption maximum at 415 nm, and the vanadium complex has an absorption maximum at 455 nm. A 1.00 × 10−3 M solution ofthe titanium complex exhibits absorbance of 0.816 at 415 nm and of 0.485 at 455 nm while a 2.00 × 10−3 M solution of the vanadium complex exhibits absorbances of 0.425 and 0.608 at 415 and 455 nm, respectively. A 1.000-g sample of an alloy containing titanium and vanadium was dissolved, treated with excess hydrogen peroxide, and diluted to a finalvolume of 1000 mL. The absorbance of the solution was 0.697 at 415 nm and 0.533 at 455nm. Calculate: a) The concentration of titanium and vanadium in the sample. b) The percentages of titanium and vanadium in the alloy.