Answered: engine.html?ClassID=1746475745# Orie.…

engine.html?ClassID=1746475745# Orie. 3.08 x 10-3 mol FeCl3 was identified through titration from the 0.700 g impure sample. What is the percent FeCl3 in the original sample? [?]% FeCl3

Fundamentals Of Analytical Chemistry

9th Edition

ISBN:9781285640686

Author:Skoog

Publisher:Skoog

Chapter17: Complexation And Precipitation Reactions And Titrations

Section: Chapter Questions

Problem 17.25QAP

See similar textbooks

Similar questions

The Handbook of Chemistry and Physics (http://openstaxcollege.org/l/16Handbook) gives solubilities of the following compounds in grams per 100 mL of water. Because these compounds are only slightly soluble, assume that the volume does not change on dissolution and calculate the solubility product for each. (a) BaSiF6, 0.026 g/100 mL (contains SiF62- ions) (b) Ce(IO3)4, 1.5102 g/100 mL (c) Gd2(SO4)3, 3.98 g/100 mL (d) (NH4)2PtBr6, 0.59 g/100 mL (contains PtBr62- ions)
Nickel(II) formate [Ni(HCO2)2] is widely used as a catalyst precursor and to make metallic nickel. It can be prepared in the general chemistry laboratory by treating nickel(II) acetate with formic acid (HCO2H). Ni(CH3CO2)2(aq) + 2 HCO2H(aq) Ni(HCO2)2(aq) + 2 CH3CO2H(aq) Green crystalline Ni(HCO2)2 is precipitated after adding ethanol to the solution. (a) What is the theoretical yield of nickel(II) formate from 0.500 g of nickel(II) acetate and excess formic acid? (b) Is nickel(II) formate paramagnetic or diamagnetic? If it is paramagnetic, how many unpaired electrons would you expect? (c) If nickel(II) formate is heated to 300 C in the absence of air for 30 minutes, the salt decomposes to form pure nickel powder. What mass of nickel powder should be produced by heating 253 mg of nickel(II) formate? Are nickel atoms paramagnetic?
Both AgCl and Agl dissolve in NH3.. (a) What mass of AgI dissolves in 1.0 L of 1.0 M NH3?. (b) VNhat mass of AgCl dissolves in 1.0 L of 1.0 M NH3?
An artificial fruit beverage contains 12.0 g of tartaric acid, H2C4H4O6, to achieve tartness. It is titrated with a basic solution that has a density of 1.045 g/cm3 and contains 5.00 mass percent KOH. What volume of the basic solution is required? (One mole of tartaric acid reacts with two moles of hydroxide ion.)
The equilibrium constant for the reaction Hg2+(aq)+2Cl(aq)HgCl2(aq) is 1.61013, Is HgCl2 a strong electrolyte or a weak electrolyte? Mm are the concentrations of Hg2+ and Cl- in a 0.015-M solution of HgCl2?
The calcium ions in human blood serum are necessary for coagulation (Figure 15.5). Potassium oxalate, K2C2O4, is used as an anticoagulant when a blood sample is drawn for laboratory tests because it removes the calcium as a precipitate of CaC2O4H2O. It is necessary to remove all but 1.0% of the Ca2+ in serum in order to prevent coagulation. If normal blood serum with a buffered pH of 7.40 contains 9.5 mg of Ca2+ per 100 mL of serum, what mass of K2C2O4 is required to prevent the coagulation of a 10 mL blood sample that is 55% serum by volume? (All volumes are accurate to two significant figures. Note that the volume of serum in a 10-mL blood sample is 5.5 mL. Assume that the KSp value for CaC2O4 in serum is the same as in water.) Figure 15.5 Anticoagulants can be added to blood that will combine with the Ca2+ ions in blood serum and prevent the blood from clotting. (credit: modification of work by Neeta Lind)
Perform these calculations for nickel(II) carbonate. (a) With what volume of water must a precipitate containing NiCO3 be washed to dissolve 0.100 g of this compound? Assume that the wash water becomes saturated with NiCO3(Ksp=1.36107). (b) If the NiCO3 were a contaminant in a sample of COCO3(Ksp=1.01012), what mass of COCO3 would have been lost? Keep in mind that both NiCO3 and COCO3 dissolve in the same solution.
Tris(pentatluorophenyl)borane, commonly known by its aeronym BARF, is frequently used to initiate polymerization of ethylene or propylene in the presence of a catalytic transition metal compound. It is composed solely of C, F, and B; it is 42.23% C and 55.66% F by mass. a. What is the empirical formula of BARF? b. A 2.251-g sample of BARF dissolved in 347.0 mL of solution produces a 0.01267-M solution. What is the molecular formula of BARF?
According to the Resource Conservation and Recovery Act (RCRA), waste material is classified as toxic and must be handled as hazardous if the lead concentration exceeds 5 mg/L. By adding chloride ion, the lead ion will precipitate as PbCl2, which can be separated from the liquid portion. Once the lead has been removed, the rest of the waste can be sent to a conventional waste treatment facility. How many grams of sodium chloride must be added to 500 L of a waste solution to reduce the concentration of the Pb2+ ion from 10 to 5 mg/L?
o/index.html?deploymentld%=55750828934189288909969212&eiSBN=9781305657571&snapshotld%32199898&id%3... ☆ IDTAP Q Search this cou Use the References to access important values if needed for this question. The concentration of H3ASO3 in a solution is determined by titration with a 0.1945 M Ce+ solution. The balanced net ionic equation for the reaction is: 2Ce*(aq) + H3ASO3(aq) + 5H2O(1) 2Ce*(aq) + H3ASO4(aq) + 2H3O*(aq) (a) If 19.83 mL of the 0.1945 M Ce** solution are needed to react completely with 30.00 mL of the H3ASO3 solution, what is the concentration of the H3ASO3 solution? M (b) Which of the two solutions was in the buret during the titration? (c) Suppose at the end of the titration, the solution containing the Ce³* ion is transferred to a volumetric flask and diluted to 300. mL. What is the concentration of Ce3+In the diluted solution? Submit Answer 5 question attempts remaining
Moles SCN- used in titration (mol)Moles of Agt in 20.0 mL titrated (mol) [Ag*lequil (M)X= [Ag*Jinit - [Ag*lequil = Change (M) solve for flask d e and f
9. Solid sodium carbonate, Na,CO, is used to determine the concentration of a HBr(aq) by titration. What is the role of sodium carbonate in this titration? (A) Catalyst (B) IndicatorA8 (C) Primary standard (D)Proton donor euld bne el hotsolon (A) nielerd auld lom onolbni Vegnto nouloe s lo ophar Hq es Short Answer 1. Consider the following equilibrium for the chemical indicator phenol red, HInd, at pH = 7.3. 0.00 H,0 = H,O* + Ind red HInd + Yellow If 10.0 mL of 0.10 mol/L NAOH(aq) is added, how will the concentration of H,O* (aq) be affected, and what is the color of the resulting solution?