JESSIREGSIDEFORDSMODans les ESESEMESTEConsider the reversible formation of the Cu(NH3)42+ complex ion.Cu²+ (aq) + 4NH3(aq) Cu(NH3)4²+ (aq)Suppose you have a solution at equilibrium in which [Cu²+] = 0.005 M.0.005[Cu(NH3)42+] = 0.500 MWhat is the value of the formation constant for the system at these conditions?Type answer:SISUSTUTTOBIESDEEStandarTESTERREGISTRAREAUTESES33134maatscremeGENETEXERFEEDEESECRESamoresionatDESSERSetmanENESSTOSScarcaseBesteroERSETSESUATORES DE 150MENGEDERESTEDSEREGETCRESCEATORED PendinSESTRANGERS WOODLADOSmangGAY BEBES BEDARFEDGELEHANDEanses[NH,M. [NH3] = 0.00148 M. and

Consider the reversible formation of the Cu(NH3)42+ complex ion. Cu²+ (aq) + 4NH3 (aq) = Cu(NH3)4²+ (aq) Suppose you have a solution at equilibrium in which [Cu²+] = 0.005 M. [NH3] = 0.00148 M, and [Cu(NH3)42+] = 0.500 M. What is the value of the formation constant for the system at these conditions? Type answer:

Consider the reversible formation of the Cu(NH3)42+ complex ion. Cu²+ (aq) + 4NH3 (aq) = Cu(NH3)4²+ (aq) Suppose you have a solution at equilibrium in which [Cu²+] = 0.005 M. [NH3] = 0.00148 M, and [Cu(NH3)42+] = 0.500 M. What is the value of the formation constant for the system at these conditions? Type answer:

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

A solution contains 2.2 × 10-3 M in Cu2+ and 0.33 M in LiCN. If the K+ for Cu(CN)4²- is 1.0 × 1025, how much copper ion remains at equilibrium? 1.9 × 10-26 M 6.7 × 10-28 M 2.9 × 10-27 × M 4.6 × 10-25 M 3.8 × 10-24 M
The complex ion Cu(NH3)42+ is formed in a solution made of 0.0200 M Cu(NO3)2 and 0.400 M NH3. What are the concentrations of Cu2+, NH3, and Cu(NH3)42+ at equilibrium? The formation constant*, Kf, of Cu(NH3)42+ is 1.70 × 1013.
The formation constant of a complex ion [M(NH3)4]2+(aq) is 8.8E8. If a solution is prepared by adding 0.4 mol of [M(NH3)4]Cl2 to 525.0 mL of water, what is the equilibrium concentration of free M2+(aq) ions? Include 3 significant figures
Determine the equilibrium concentration of nickel(II) ion in a solution that contains 2.3 M ammonia and 0.040 M nickel(II) nitrate. The formation constant for the complex [Ni(NH,) ] - 5.5×10® is 3.65×10-37 M 1.26×10-12 M 1.32×1054 M 3.65×10-10 M
The equilibrium constant for the formation of Cu(CN)42- is 2.0 x 1030. Calculate the value of pCu2+, or -log[Cu2+], if 2.21 g of CuCl2 is dissolved in 1.000 L of a 0.926 M solution by NaCN. The addition of CuCl2 does not affect the volume (the final volume is always 1,000 L).
7.00 grams of Cobalt (II) nitrate are dissolved in 1.00 liter of water. What is the initial concentration of CO (2+) in moles per liter? Then, 0.22 moles of solid KOH are added to this solution. The solution volume remains 1.00 liter. Given that Kf = 5.0 x 10^9 for the complex ion, Co(OH)4 (2-) find the final concentrations of Co (2+), Co(OH)4 (2-), and OH-. Also find the pH of this final solution.
write the reaction for the complex ion Cu(NH2)4SO4
What is the driving force in the following reaction Ni(NO3)2(aq) +K2S(aq) -> NiS(s)+ 2KNO3(aq)
Consider the insoluble compound nickel (II) hydroxide, Ni(OH)2. The nickel ion also forms a complex with cyanide ions. Write a balanced net ionic equation to show why the solubility of Ni(OH)2 (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction. For Ni(CN)4²-, Kf = 1.0×10³¹ . Be sure to specify states such as (aq) or (s). K = + Submit Answer + Retry Entire Group No more group attempts remain
For the aqueous [Ag (NH3)₂ complex K₁=1.12 × 107 at 25 °C. + Suppose equal volumes of 0.0042M AgNO3 solution and 0.86M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Ag ion. Round your answer to 2 significant digits. M x10 Times 10 to an exponent
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
A solution is prepared such that the initial concentration of A2+ is 1.50x103 M and the initial concentration of X is 4.60x10-3 M. A2+ and X are allowed to react as shown below to establish equilibrium with the complex AX2+. In a colorimetry experiment, the equilibrium concentration of the complex AX2+ is determined to be 8.9x10-4 M. A2* (aq) + X (aq) =Ax2+ (aq) %3D Complete the ICE table below by selecting the correct value or expression to place in the ICE table from the drop-down menu. A2+ (aq) X (ад) АХ2+ (aq) Initial concentration Change in concentration Equilibrium concentration expression Equilibrium concentration value