1) The amount of warfarin, used for anticoagulant medications, in a sample was calculated as follows. A 13.96 g sample was first treated with an alkaline I2 solution to convert C19H16O4 to CHI3. This treatment gives one mole of CHI3 for every mole of C19H1604 that was initially present in the sample. The iodine in CHI3 is then precipitated as AgI(s) by treatment with excess AgNO3(aq): CHI3(aq) + 3AGNO3(aq) + H2O(1)→ 3AgI(s) + 3HNO3(aq) + CO(g) If 0.1386 g solid AgI were obtained, then what is the percentage by mass of warfarin in the sample analyzed?

1) The amount of warfarin, used for anticoagulant medications, in a sample was calculated as follows. A 13.96 g sample was first treated with an alkaline I2 solution to convert C19H16O4 to CHI3. This treatment gives one mole of CHI3 for every mole of C19H1604 that was initially present in the sample. The iodine in CHI3 is then precipitated as AgI(s) by treatment with excess AgNO3(aq): CHI3(aq) + 3AGNO3(aq) + H2O(1)→ 3AgI(s) + 3HNO3(aq) + CO(g) If 0.1386 g solid AgI were obtained, then what is the percentage by mass of warfarin in the sample analyzed?

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter20: Transition Metals And Coordination Chemistry

Section: Chapter Questions

Problem 1ALQ

See similar textbooks

Similar questions

You want to separate Cd2* and Fe2+ (initial concentration 103 mol/L) by means ofprecipitation of the corresponding sulphides. Is therea pH range in which one of the two metals is precipitated quantitatively(concentration in the solution less than or equal to 10" mol/L) is precipitatedwhile the other is still completely_in solution?Calculate and name this pH range where pH values below 0are set equal to O. Illustrate the situation graphically by drawing
What products would you expect to form in the reaction between BrF3 and Fe2O3? Br2(l), O2(g), and an iron fluoride salt F2(g), O2(g), and an iron bromide salt OF2 and an iron bromide salt OBr2 and an iron fluoride salt
Account for the following observations: (a) Phosphorusforms a pentachloride, but nitrogen does not. (b) H3PO2 isa monoprotic acid. (c) Phosphonium salts, such as PH4Cl,can be formed under anhydrous conditions, but they cannotbe made in aqueous solution. (d) White phosphorus ismore reactive than red phosphorus.
Give an example of a double salt that can be formed via ligand exchange and give the reactions involved
The Latimer diagram for nitrogen in acidic solution at 25 °C is shown. Classify each species based on whether it is stable with respect to disproportionation or unstable with respect to disproportionation in acidic solution under standard conditions at 25 °C.
Describe the general trends in the following properties of first series 3d of transition elements: (i) number of oxidation states exhibited (ii) formation of oxometal ions.
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.
A pink solid has the formula CoCl3·5NH3·H2O. A solution of this solid is also pink in color and when titrated with silver nitrate quickly forms 3 mol of AgCl. Upon heating the pink solid, it loses 1 mole of water and forms a purple solid with the same NH3:Cl:Co ratio. Dissolving and titrating with AgNO3, the purple solid slowly releases one of its chlorides. a) Derive the formulas of the two octahedral complexes.b) draw and name them.c) write the chemical equations of all described reactions.
The periodic trend which is responsible for the observation that the maximum oxidation state of the transition-metal elements peaks near groups 7B and 8B?
Hem‎oglobin is sai‎d to be an examp‎le of coordination compou‎nd. This is because a. T‎he molec‎ule is ab‎le to bi‎nd Oxygen us‎ing heme stru‎cture. b. It cont‎ains a tra‎nsition metal Fe +2 and it is solu‎ble in w‎ater. c. It cont‎ains a ligand (heme) that is coordi‎nated to Fe +2, which is a Lewis acid. d. It is a colo‎red comp‎lex because of the presen‎ce of the he‎me.
When solid CrO3is dissolved in water, the solution is or-ange rather than the yellow of H2CrO4. How does this observa-tion indicate that CrO3is an acidic oxide?
Calculate the pH of a 0.10M solution of NaHSO4 solution taking into account activity (Ka2 = 1.92 for H2SO4).