1. A mixture of the 8-hydroxyquinoline complexes of Al and Mg weighed 1.084 3 g. When ignited in a furnace open to the air, the mixture decomposed, leaving a residue of Al2O3 and MgO weighing 0.134 4 g. Find the weight percent of Al(C₂H6NO); in the original mixture. AIQ3 FM 459.43 Al + MgQ₂ FM 312.61 Mg heat Al2O3 + MgO FM 101.96 FM 40.304

1. A mixture of the 8-hydroxyquinoline complexes of Al and Mg weighed 1.084 3 g. When ignited in a furnace open to the air, the mixture decomposed, leaving a residue of Al2O3 and MgO weighing 0.134 4 g. Find the weight percent of Al(C₂H6NO); in the original mixture. AIQ3 FM 459.43 Al + MgQ₂ FM 312.61 Mg heat Al2O3 + MgO FM 101.96 FM 40.304

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.1QAP

See similar textbooks

Similar questions

Two different compounds are known with the formula Pd(py)2Cl2, but there is only one compound with the formula Zn(py)2Cl2. The symbol py is for pyridine, a mono-dentate ligand. Explain the differences in the Pd and Zncompounds.
Q 2. Comment on the Kinetic and thermodynamic stability of metal complexes? (2 marks) (a) Which complex is kinetically labile or inert according to crystal field theory? H₂O OH2 OH2 * H₂O NECHI Mn OH2 OH2 4- 2+ [+] NEC CEN CEN (b) Which complex is most thermodynamically stable and why? Calculate log ẞ to determine stability? H3N 2+ _NH3] 2 [NC-Ag-CN]] NH3 3+ H3N... H3N ,,NH3 Cr NH3 H3N NH3 NH3 K 1.0 x10¹² K 5.4 x 1018 K=2.0 × 105
In trilonometric (“complexonometric") titration as a titrant is used: EDTA solution Hg(NO3)2 solution; KĄ[Fe(CN)6] solution; Hg(CN)2 solution;
A 0.4755-g sample containing (NH4)2C2O4 and inert compounds was dissolved in water and made alkaline with KOH. The liberated NH3 was distilled into 50.00 mL of 0.1007 N H2SO4. The excess H2SO4 was back-titrated with 11.13 mL of 0.1214 N NaOH. Calculate the percentage of N (14.007 g/mol) and of (NH4)2C2O4 (124.10 g/mol) in the sample.
A mixture of the 8-hydroxyquinoline complexes of Al and Mg weighed 1.0843 g. When ignited in a furnace open to the air, the mixture decomposed, leacing a residue of Al2O3 and MgO weighing 0.1344 g. Find the weight percent of Al(C9H6NO)3 in the original mixture
A mixture of the 8-hydroxyquinoline complexes of Al and Mg weighed 1.0843 g.When ignited in a furnace open to the air, the mixture decomposed, leaving a residue of Al2O3and MgO weighing 0.1344 g. Find the weight percent of Al(C9H6NO)3 in the original mixture.
After titration, weight percent of oxalate in K3[Fe(C2O4)3] (MW: 437.2 g/mol) sample was determined to be 55.8%. What is the percent error of oxalate content determination?
The amount of Fe (AW 55.85) in a 0.4891-g sample of an ore was determined by a redox titration with K2Cr2O7 (FW 294.20). The sample was dissolved in HCl and the iron brought into the +2 oxidation state using a Jones reductor. Titration to the diphenylamine sulfonic acid end point required 36.92 mL of 0.02153 M K2Cr2O7. Report the iron content of the ore as %w/w Fe2O3 (FW 159.70). a. 54.46 % b. 12.98 % c. 77.86 % d. 31.45 %
Draw a reasonable structure for a complex between Fe3+ and nitrilotriacetic acid, N(CH2CO2H)3.
If 21.70 mL of 0.0500 M KMnO4 is required to titrate a 0.450 g sample of K3[Fe(C2O4)3]⋅3H2O, what is the percent C2O2−4C2O42− in the complex?
Question. The determination of K;[Al(C₂O4)3] content in a sample after preparation in the inorganic chemistry laboratory is described by the following equations: Dissolution of oxalato ligand: K3[Al(C₂0₂)3] + exess HCI Titration against KMnO₂: 2 KMnO4(aq) +5 C₂04² (aq) + 16 Ha (aq) ↓ Purple 1.0040 1.1303 1.0923 1.1139 1.0642 Use the following data to determine the average of %K [Al(C₂O₂),] in samples prepared by students. Mass sample Volume of 0.1M KMnO4 added (mL) 22.5 24.5 20.3 22.7 21.1 3 H₂C₂O + AICI, +3KCI Hint: M.wt of K[Al(C₂0)]=408 g/mol 10 CO)+2 Mn² (aq) +8 H₂0) colorless Mass of % K₁[Al(C₂O4)3] Average K3[Al(C₂O4)3]
Chromel is an alloy composed of nickel, iron, and chromium. A 0.6392-g sample was dissolved and diluted to 250.0 mL. When a 50.00-mL aliquot of 0.05173 M EDTA was mixed with an equal volume of the diluted sample, all three ions were chelated, and a 5.15-mL back-titration with 0.06139 M copper(II) was required. The chromium in a second 50.0-mL aliquot was masked through the addition of hexamethylenetetramine; titration of the Fe and Ni required 34.27 mL of 0.05173 M EDTA. Iron and chromium were masked with pyrophosphate in a third 50.0-mL aliquot, and the nickel was titrated with 24.31 mL of the EDTA solution. Calculate the percentages of nickel, chromium, and iron in the alloy. Percentage of nickel = % Percentage of iron = Percentage of chromium = % 10