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- A certain coordination compound has the simplest formula PtN2H6Cl2. It has a molar mass of about 600 g/mol and contains both a complex cation and a complex anion. What is its structure?Which of the following is the correct Kf expression for the formation of the complex ion tetraiodoplumbate(II) ion, [PbI4]2–? Pb2+ (aq) + 4 I1- (aq) < === > [PbI4]2– (aq) Kf = [PbI4]2– / {[Pb2+] [4 I1-]} Kf = {[Pb2+] 4[I1-]} / [PbI4]2– Kf = {[Pb2+] [I1-]4} / [PbI4]2– Kf = [PbI4]2– / {[Pb2+] [I1-]4}For the 31 aqueous [Ni (CN)4] complex K, = 2.00 × 10³¹ at 25 °C. .2+ Suppose equal volumes of 0.0086M Ni (NO3)2 solution and 0.38M KCN solution are mixed. Calculate the equilibrium molarity of aqueous Ni**ion. Round your answer to 2 significant digits. M ☐x x10 X Ś
- A protein (P) binds a ligand (L) to form a complex (PL). a. Draw the equilibrium expression. b. Write the dissociation constant Ka, using [P], [L] or [PL], or some of them. c. Write the fraction bound of the ligand to the protein 0, using [P]. [L] or [PL], or some of them. d. From b and c, derive the equation of the fraction bound e in terms of [L] and Ka. Show the process. e. Sketch a hypothetical binding curve. Then, circle the Ka value. Explain why you chose this (L]. 10- 0.9- 08- 07- 06- e 05- 0.4- 0.3- 02- 01- 25 50 100 150 200What is the Kf expression for the following complexation reaction? Al3* (ag) + 6F (aq) [AIFP (aq) Select one: | AIF ° A1 А. | AP* ]| F |* | AIF3- | 6 KĘ = В. | AIF,3- | K = | AI* ]| F]° K = | AIF3- |6 D.A solution is prepared such that the initial concentration of A2+ is 1.50×10-3 M and the initial concentration of X is 4.60×10-3 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 8.9×10-4 M. A2+ (aq) + X (aq) AX2+ (aq) What is Kf, the formation constant, for this complex?
- What is the equilibrium constant expression for the Ksp of Fe2S3? a. Ksp = [2Fe3+]2 [3S2-]3 b. Ksp = [2Fe3+] [3S2-] c. Ksp = [Fe3+]2 [S2-]3 d. Ksp = [Fe3+] [ S2-]A solution is prepared such that the initial concentration of A2+ is 1.50×10-3 M and the initial concentration of X is 4.60×10-3 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 8.9×10-4 M. A2+ (aq) + X (aq) AX2+ (aq) Use your correct answers from #7 to answer this question. What is Kf, the formation constant, for this complex?The equilibrium equation for the formation of the complex PbBr42 is: Pb2+ + 4 Br = PbBr42. Since PbBr42- is a typical complex, which of the following would you expect to be true? 1. The Kf value is small (- power of 10) 2. At equilibrium, there will be more PbBr42- than free Pb2+ and Br- 3. The Kf value is large (+ power of 10) 4. At equilibrium, there will be more free Pb²+ and Br than PbBr,2- 3 and 4 only 2 and 3 only O 1 and 4 only O 2 only O 1 and 2 only
- Co(H2O)62+(aq) + 4 Cl–(aq)⇄CoCl42–(aq) + 6 H2O a) Would a saturated solution of ammonium chloride pordice a large enough concentration of chloride ion to form chloride complex? b) What is the effect of heating a soution? If heat were a reagent, where would it be in the cobalt complex equilibrium? Endo or exothermic?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 value13. Z²+ can form a hexaammonia complex ion in the presence of ammonia (K₁ = 1.3 x 105). Z³+ can also form a hexaammonia complex ion in the presence of ammonia (Kf = 2.3 x 102³). ZCl₂ has a Ksp value of 1.8 x108. ZCl3 has a Ksp value of 2.7 x 10-¹². Z is a transition metal. a. Which compound would be more soluble in an 0.100 M NH3 solution ZCl3 or ZCl₂? b. Calculate the molar solubility of ZCl3 in pure water. c. NH₂(CH3) is a better ligand with Z3+ than NH3. Would this increase or decrease the solubility of ZCl3 if the 0.100 M NH3 solution was replaced with a 0.100 M NH₂(CH3) solution (provided NH2(CH3) can also form a hexamine complex ion with Z³+)?