500.0 mL of 0.020 M Mn(NO3)2 are mixed with 1.0 L of 1.0 M Na2C204. The oxalate ion, C2042-, acts as a ligand to form complex ions with the Mn2+ ion. Mn2+ + C2042- MnC204 K1 = 7.9 x 103 [Mn(C204)2]2-2 MnC204 + C2042- K2 = 1.26 x 10-2 What is the equilibrium constant for the reaction below? Mn2+ + 2C2042-2 [Mn(C204)2]2-

500.0 mL of 0.020 M Mn(NO3)2 are mixed with 1.0 L of 1.0 M Na2C204. The oxalate ion, C2042-, acts as a ligand to form complex ions with the Mn2+ ion. Mn2+ + C2042- MnC204 K1 = 7.9 x 103 [Mn(C204)2]2-2 MnC204 + C2042- K2 = 1.26 x 10-2 What is the equilibrium constant for the reaction below? Mn2+ + 2C2042-2 [Mn(C204)2]2-

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

31 For the aqueous [Ni(CN)4] complex K₁=2.00 × 10³¹ at 25 °C. .2+ Suppose equal volumes of 0.0052M Ni (NO3), solution and 1.0M KCN solution are mixed. Calculate the equilibrium molarity of aqueous Ni²+ ion. Round your answer to 2 significant digits. M x10 × Ś
14. The complex ion [Ni(TAP)(CN)]+ has a distorted trigonal bipyramidal structure, the complex ion has a coordination number… A. 4B. 6C. 5D. 7
The ligand bpy forms complexes with Ru³+ and Ru²+. The standard potential of the couple is +1.26 V. Does bpy bind preferentially to Ru³+ or Ru²+? Why? [Ru(bpy)3]³+/[Ru(bpy)3]²+ 3+
For the complexes: 2- (1){Co(NO)6} Splitting patterm: octahedral of tetrahedral? (II) {Co(H2O)6}* Splitting pattern: octahedral of tetrahedral Strong or weak field ligand? Strong or weak field ligand? Number of unpaired electrons? Number of unpaired electrons? Which is more paramagnetic; (I) or (II)?
Please help solve the table.
Name the following complex ions. formula name ¬3+ Sc 2 Ag (NH,), 3+ Fe(NH, 4
For the coordination compound [Pd(CN)2(en)2][PtCl4]: How many unpaired d electrons are present in the cation and anion? What is the standard reduction potential in V of the complex anion (E° [PtCl4]2-/Pt) at 298.15 K? Given: E° Pt2+/Pt = +1.188V, Kf for the complex anion = 1.1 x 1016
Consider the coordination complex [Cr(OH₂)3C13] Br3 Identify the ligands by name (include the word "ion" at the end for all ions): What is the charge on the coordination complex? Enter the sign then the numeric value (+2, -2, etc.) What is the oxidation state of the Cr ion? Enter the sign then the numeric value (+2, -2, etc.) What is the coordination number for the complex ion? Enter your answer as a number.
Cr(aq) + 3 e Cr(s) Zn²(aq) + 2 e → Zn(s) 2 H₂O() +2 e → H₂(g) + 2 OH(aq) Mn2(aq) + 2 e A(an) + 3 e Mn(s) Al(s) 7. All of the following statements concerning ligand field theory are true EXCEPT A. in low-spin complexes, electrons are concentrated in the day, dys, and dr orbitals. B. in an isolated atom or ion, the five d orbitals have identical energy. C. low-spin complexes contain the maximum number of unpaired electrons. D. the crystal field splitting is larger in low-spin complexes than high-spin complexes. E. the energy difference between d orbitals often corresponds to an energy of visible light. 8. All of the following complexes will be colored (in the visible) EXCEPT A. [Co(en)]2+ B. [Fe(CN)6] C. [Ni(H₂O)]²+ D. [Cd(NH3)4]2+ 9. A positron has a mass number of a(n) a. 0; 1+; proton b. 1; 2+; proton c. 0; 1+; electron d. 1; 2+; electron e. 0; 0; proton -0.76 -0.83 -1.18 -1.66 a. [Cr(CO)6]C13 b. [Cu(OH)4(NH3)2] c. K4[Mn(CN)6] d. [Pt(en)3] (NO3)4 e. [Pt(NH3)2(OH₂)CIJ3PO4 10. In which…
How do I find the electronic configuration of an unknown transition metal? For instance I am given [M(H2O)6]+2, where M is the unknown first row transition metal with a magnetic moment of 2.83. I know it's oxidation state is 2+
Give the systematic name for the following coordination compound or complex ion: