In a dilute nitric acid solution, Fe" reacts with thiocyanate ion (SCN) to form a dark-red complex: Fe(H,0)J + SCN The equilibrium concentration of (Fe(H,O),NCS]** may be determined how darkly colored the solution is (measured by a spectrometer). In one such experiment, 1.0 mL of 0.20 M Fe(NO,), was mixed with 1.0 mL of 1.0 X 10M KSCN and 8.0 H,0 + [Fe(H,O),NCS]*

In a dilute nitric acid solution, Fe" reacts with thiocyanate ion (SCN) to form a dark-red complex: Fe(H,0)J + SCN The equilibrium concentration of (Fe(H,O),NCS]** may be determined how darkly colored the solution is (measured by a spectrometer). In one such experiment, 1.0 mL of 0.20 M Fe(NO,), was mixed with 1.0 mL of 1.0 X 10M KSCN and 8.0 H,0 + [Fe(H,O),NCS]*

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

The formation constant of a silver cyano complex is 5.6 x 1018 Ag+ + 2 CN Ag(CN)," If a certain solution have the equilibrium concentrations of 5.0 x 10-3 M and 0.20 M for Ag+ and CN", respectively, then what is the equilibrium concentration for the silver cyano complex? O1.1 x 1015 O5.6 x 1015 02.8 x 1016 02.4 x 109
the overall equilibrium constant for the reaction of hexaaquairon(II) with 2 mol of acetate to form diacetatotetraaquairon(II) is 120, wheras that for the reaction with 1 mol of malonate, -OOCCH2COO-, is 630. Write equations representing these reactions and briefly rationalize the differences in the magnitudes of the equilibrium constants.
Below is the chemical equation of the complex Ni(C4H7N2O2)2. What specie is responsible for the color of its solution and the precipitate?
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
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 formation constant for triethylenetetraamine - silver is 5.0x10^7. If the complex formed is 1:1 Ag + Trien, calculate the concentration of Ag + in equilibrium when 10.00 mL.0250 M of trien solution is added to 20.00mL of Ag+ .0120M. (Verify limiting reactant to help solve). Please show a step by step solving to better my understanding of the process
write the reaction for the complex ion Cu(NH2)4SO4
Please use the values in the resources listed below instead of the textbook values. Sometimes equilibria for complex ions are described in terms of dissociation constants, Ka. For the complex ion Cu(CN)4 3- the dissociation reaction is as follows. [Cu*]• [CN 14 Kd [Cu(CN)43-] Cu(CN)4 3- = Cu+ + 4 CN- = 5.0X10° n-31 = Calculate the value of the formation constant, Kf, for Cu(CN)4°¯. 4.0
What is the concentration of Cu2+ in a solution of the complex ion Cu(NH3)42+ formed by reaction of 0.0140 M Cu2+ and 1.05 M NH3? Kf = 1.0 × 107 [Cu2+] = ??? mol/L
Define a complex liquid