5.00 mL of 0.0200 M Fe(NO3)3 was mixed with 5.00 mL of 0.00200 M KSCN to form the FeSCN²+ complex. The equilibrium molar concentration of the FeSCN²+ complex was determined to be 1.00 X 104 M Moles of Fe³+, initial Moles of SCN, initial Moles of FeSCN²+ a) b) c)

5.00 mL of 0.0200 M Fe(NO3)3 was mixed with 5.00 mL of 0.00200 M KSCN to form the FeSCN²+ complex. The equilibrium molar concentration of the FeSCN²+ complex was determined to be 1.00 X 104 M Moles of Fe³+, initial Moles of SCN, initial Moles of FeSCN²+ a) b) c)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Similar questions

Determine the equilibrium concentration of the complex ion formed by a solution with 10.0 mL of 0.100 M FeCl3, 1.00 mL of 0.00100 M KSCN, and 9.00 mL of water.
After completing the experiment, a student finds that the equilibrium concentrations of the reactants and product are as follows. Calculate the equilibrium constant for the complex ion formation. [SCN¯]eg= 6.45x10-4 M %3D [Fe3+]eg = 8.42x10-4 M leq [FENCS2+]eg = 1.50x10-4 M %3D
Spotify - 2Pa X2 www.shakes x * OWLV2 | Onli x + .com/ilrn/takeAssignment/takeCovalentActivity.do?locator=assignment-take [References] Cu2+ ions from copper(II) sulfate combine with Br ions from potassium bromide to form the yellow CuBra complex ion in the equilibrium shown below: (aq) + 4 Br" (aq)CuBr (aq) + 4 H,O (1) yellow Cu(H,O),+ blue When the blue diluted solution was heated, it turned yellow. This color change indicates that the are favored, K v with increased temperature, and the reaction is
a. A lab student analyzed a cooled Ni-en complex to determine the ethylenediamine, en, content. A 0.334 g sample of the synthesized Ni-en complex was dissolved in about 50 mL of water and titrated with 0.243 M HCI (aq). Endpoint required 21.01 mL of the HCI (aq). What is the mass (in grams) of en (MW of en = 60.10 g/mole) in the Ni-en complex analyzed? g en + 2 HCI H₂en²+ + 2 CI™ b. Continuing on with the analysis of the Ni-en complex as found in part a, 30 mL of dimethylglyoxime (DMG) solution was added to the 0.334 g of the titrated Ni-en complex solution. The resulting beautiful red complex, Ni(DMG)2 (MW = 288.94 g/mole) was collected by filtration and found to weigh 0.233 g after 20 minutes in the oven. What is the mass (in grams) of Ni in the Ni-en complex analyzed? Ni²+ + 2 DMG → Ni(DMG)2 (s) CD. [Ni(en)3]SO4.7H₂O CE. [Ni(en) (H20)4]SO4-4H₂0 9 c. Determine the empirical formula of the complex synthesized in parts a and b. A. [Ni(en)3]SO4-4H₂0 B. [Ni(en)2(H₂O)₂]SO4-3H₂0 C.…
Metallic cadmium is added to 0.350 L of an aqueous solution in which [Cr³+]o is 1.00 mol/L. What is the [Cr³+] eq concentration of the chromium(III) species at equilibrium? Kc=0.288 2Cr3+(ac)+Cd(s)<------->2Cr2+(ac)+Cd2+
The equilibrium constant for the following reaction is 1.0 x 1023. Cr+ (aq) + H₂EDTA² (aq) CrEDTA (aq) + 2H+ (aq) O₂C-CH₂ CH, CO, O₂C-CH₂ CH, C, EDTA- N-CH₂-CH₂-N) Ethylenediaminetetraacetate EDTA is used as a complexing agent in chemical analysis. Solutions of EDTA, usually containing the disodium salt Na₂H₂ EDTA, are used to treat heavy metal poisoning. Calculate [Cr] at equilibrium in a solution originally 0.0050 M in Cr³+ and 0.040 M in H₂EDTA and buffered at pH 6.00. Assume that H₂ EDTA form dominates at this pH. = [Cr³+) | M
In 0.15m Cu2 (03 (aq) Solution, Write the chemical equation of the reaction With the ksp expression: KSp= [Fe²] ³- [Pou] ²
Which of the following will increase the solubility of calcium silicate, CaSiO3? a) The additions of calcium chloride, CaCl b) The addition of oxygen gas c) The formation of ferricyanide, [Fe(CN)6]3- d) The formation of [Ca(EDTA)]2-
Taking the activity coefficient effect into consideration, please calculate the concentration of Fe in a solution that is saturated with Fe4[Fe(CN)6]3 (Iron(III) ferrocyanide). The overall ionic strength of the solution is 0.001 M. Notes: Kap of [Fea[Fe(CN)6]3] = 3.3×1041. At 0.001 M, the gFe3+ and g[Fe(CN)6] are 0.738 and 0.570, respectively. Format BIU ... Ea h Add a File Record Audio Record Video of
The citrate ion is a tridentate ligand that forms a strong complex with ferric ion: Fe^3+ + 2Cit^3- <=> Fe(Cit)2^3- A metal ion buffer solution was prepared by adding 2.5g of Na3Cit.2H2O (MW = 294.1) and 1 g of Fe(NO3)3.9H2O (MW=404.01) to a 500ml volumetric flask. The flask was filled to the mark and mixed throughly after the reagents dissolved. The pFe = 18.56, Calculate Kf.
The chemical reaction for the formation of the red-orange iron(III) thiocyanate complex ion is Fe3+ (aq) + SCN- (aq) <==> [FeSCN2+] (aq) What is the source of the Fe3+ ions? What is the source of the SCN- ions? The equilibrium constant for this reaction is given by what
The formation constant for [Cu(CN)2]- is 1.0 x 1016, what is the value of the dissociation constant for this complex? Your answer should have 2 sig figs.