If dissociation for a complex ion is 6.3 x 10-5 what is Kf ?
Sometimes equilibria for complex ions are described in terms of dissociation constants, Kd. For the complex ion AlF63− the dissociation reaction is: AlF63− ⇌ Al3+ + 6F− and Kd = [Al3+][F−]6 divided by [AlF63−] =2×10−24 Calculate the value of the formation constant, Kf, for AlF63−.
Cu(OH)2 has Ksp = 2.2 x 10^–20. The complex ion Cu(NH3)4 2+ has Kf = 2.1 x 10^13 . What concentration of [NH3] can dissolve 0.01mol/L Cu(OH)2 to become Cu(NH3)4 2+ in 1L solution?
The Kf for the formation of the complex ion between Pb2+ and EDTA4− is 1.0 × 1018 at 25° C. Pb2+ + EDTA4− ⇌ Pb(EDTA)2− Calculate the [ Pb2+ ] at equilibrium in a solution containing 2.50 × 10−3 M Pb2+ and 3.50 × 10−3 M EDTA4
Question 5: The cation, Co2+, is able to form a complex ion, [Co(SCN)4] 2–, with the thiocyanate anion, SCN–. (a) Write the chemical equation for the (a) Write the chemical equation for the formation of this complex ion with the corresponding expression for the formation constant, Kf, and (b) Given Kf for [Co(SCN)4] 2– = 1 x103, explain how having SCN– in solution would affect the solubility of Co(OH)2 (Ksp for Co(OH)2 = 1.3 x 10–15).
A metal ion M forms a stable complex with the ligand X: M + (aq) + 4 X (aq) ⇌ M (X) 4+ (aq) Kf = 1.0 ∙ 10^20 In a solution where [M +] = 0.100 M and [X] = 0.800 M before reaction, what is [X] at equilibrium?
Question 5 2 pts What is the crystal field spitting energy for a complex ion that absorbs light at 530 nm? 3.75 x 10-19) 2.15 x 10-15 4.53 x 10-21) 5.42 x 10-12
O KINETICS AND EQUILIBRIUM Using Kf to calculate the equilibrium molarity of a complex For the aqueous ( Ni(NH3)672* complex K,=2.0 x 108 at 25 °C. Suppose equal volumes of 0.0064 M Ni ) solution and 0.96 M NH, solution are mixed. Calculate the equilibrium molarity of aqueous Ni“ ion. Round your answer to 2 significant digits. | |м x 6 ?
For the complex ion [AgBr)' K,-1.7 x 107 and Ksp for AgBr= 5.0 x 10". Use this information to calculate Kc for the reaction AgBr Br AgBr2 5.
O KINETICS AND EQUILIBRIUM Using Kf to calculate the equilibrium molarity of a complex an For the aqueous [Ag(CN)complex K-3.0x 102° at 25 °C. Suppose equal volumes of 0.0040 MAgNO solution and 0.96 MNaCN solution are mixed. Calculate the equilibrium molarity of aqeous Ag ion Round your answer to 2 significant digits. Џи x10
O KINETICS AND EQUILIBRIUM Using Kf to calculate the equilibrium molarity of a complex an For the aqueous [Ag(CN)complex K-3.0x 102° at 25 °C. Suppose equal...
What concentration of Cl- is required to form a complex ion of [AgCl2-](aq) whose concentration is 0.2M? Assume the concentration of [Ag+] is 0.1M. Your answer should be listed as a molar concentration. Kf for AgCl2- is 1.8x10^5 Please thorougly explain work, I want to understand.