Titanium(IV) and vanadium(V) 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 × 103 M solution of the titanium complex exhibits an absorbance of 0.805 at 415 nm and of 0.465 at 455 nm, while a 1.00 x 10-2 M solution of the vanadium complex exhibits absorbances of 0.400 and 0.600 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 final volume of 100 mL. The absorbance of the solution was 0.685 at 415nm and 0.513 at 455nm. What were the percentages of titanium and vanadium in the alloy?

Titanium(IV) and vanadium(V) 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 × 103 M solution of the titanium complex exhibits an absorbance of 0.805 at 415 nm and of 0.465 at 455 nm, while a 1.00 x 10-2 M solution of the vanadium complex exhibits absorbances of 0.400 and 0.600 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 final volume of 100 mL. The absorbance of the solution was 0.685 at 415nm and 0.513 at 455nm. What were the percentages of titanium and vanadium in the alloy?

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter8: Bonding In Transition Metal Compounds And Coordination Complexes

Section: Chapter Questions

Problem 41P

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Titanium(IV) and vanadium(V) form colored complexes when treated with hydrogen peroxide in 1 M Sulphuric acid. The titanium complex has an absorption maximum at 415 nm, and the vanadium complex has an absorption maximum at 455 nm. A 0.00100 M solution of the titanium complex exhibits an absorbance of 0.805 at 415 nm and of 0.465 at 455 nm, while a 0.0100 M solution of the vanadium complex exhibits absorbances of 0.400 and 0.600 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 final volume of 50.0 mL. The absorbance of the solution was 0.685 at 415 nm and 0.513 at 455 nm. a) Calculate the parts per thousand (ppt) concentration of vanadium (MW=50.94 g/mol) in the mixture. b) Calculate the parts per thousand (ppt) concentration of titanium (MW=47.87 g/mol) in the mixture.
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.
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 of the titanium complex exhibits an 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 final volume of 1000 mL. The absorbance of the solution was 0.697 at 415 nm and 0.533 at 455 nm. Calculate: a) The concentration of titanium and vanadium in the sample. b) The percentages of titanium and vanadium in the
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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…