Ans:) Due to very high value of Kf the concentration of Pb2+ is very low at equilibrium. If there is any doubt regarding the solution please ask in the comment section.
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1. The K for the complex ion formation between Pb2+ and EDTA is 1.4x1018 at 25°C....
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
Kc is 2.35 × 1018 at 25 °C for the formation of iron(III) oxalate complex ion. If 0.0450 mol L‐1 Fe3+ is initially mixed with 2.00 mol L‐1 oxalate ion, what is the concentration of Fe3+ ion at equilibrium? a) complete the concentration summary below. Fe3+(aq) + 3C2O42‐(aq) ⇌ [Fe(C2O4)3]3‐(aq) Initial concentrations 0.0450M 2.00M 0 Change is Concentrations due to stoichiometric Reaction Initial Conc. After stoichiometric reaction Change in concentration to reach equilibrum Equilibrium Conc. The concentration of Fe3+ at...
Please help with chemistry 17. Find the new K value for the combined solubility equilibrium and formation equilibrium reactions when the Ksp for PbCO, is 7.4x10M and the K, for the [Pb(GOJ2]2-complex ion is 3.5x106. (C2042-?S the bidentate oxalate ligand.) The K, for the complexion Pb(EDTA)2-is 2.0x108. Analysis shows a solution at equilibrium contains [Pb(EDTA?] = 0.0011 M, [EDTA"] = 0.88 M, and [Pb2+]s 6.25×10-22 M. what concentration of sulfide ion will just start the precipitation of PbS(s) from the...
10) Kc is 1.67 1020 at 25°C for the formation of iron(III) oxalate complex ion: Fe3+(aq) + 3 C2042-(aq) = [Fe(C204)3β-(aq). If 0.160 M Fe3+ is initially mixed with 1.00 M oxalate ion, what is the concentration of Fe3+ ion at equilibrium? D) 6.81x 10-21 M A) 1.47 x 1020 M C) 1.04 x 1021 M B) 0.0100 M 11) Cyclohexane, C6H12, undergoes a molecular rearrangement in the presence of AlCl3 to form methylcyclopentane, CH3C5H9, according to the equation: C6H12-...
In aqueous solution the Pb2+ ion forms a complex with four chloride anions. Write the formation constant expression for the equilibrium between the hydrated metal ion and the aqueous complex. Under that, write the balanced chemical equation for the first step in the formation of the complex.
The molecular complex PbCl4 2- dissociates in water by the process PbCl4 2- (aq) = Pb2+(aq) + 4 Cl KC = 4.1 x 10-16 The initial concentration of PbCl4 2- in an aqueous solution is 0.0220 M. No Pb2+ or Cl- ions are initially present. What is the concentration of Pb2+ ion present when equilibrium is achieved?
5) The molecular complex PbC142-dissociates in water by the process PbC142"(aq) = Pb2+ (aq) + 4 CI Kc - 4.1 x 10-16 The initial concentration of PbCl2- in an aqueous solution is 0.0220 M. No Pb2+ or C ions are initially present. What is the concentration of Pb2+ ion present when equilibrium is achieved? [12 points]
1. A solution is made from 125.0 mL of 0.200 M Pb2+ and 375.0 mL of 0.100 MI PbIfs) ¢, Pb?"(aq) + 2 1-(aq) K,-8.5 x10-9 (10 pts) Does a precipitate form? Show all calculations. (10 pts) Calculate the concentration of each ion at equilibrium.
urgent 5) The molecular complex PbCh? dissociates in water by the process PbCk?"(aq) = Pb2+ (aq) + 4 CH Kc = 4.1 x 10-16 I The initial concentration of PbCl2 in an aqueous solution is 0.0220 M. No Pb2+ or C ions are initially present. What is the concentration of Pb2+ ion present when equilibrium is achieved? [12 points)
5) The molecular complex PbCl2- dissociates in water by the process PbCl²(aq) = Pb²+(aq) +4 CH Kc = 4.1 x 10-16 The initial concentration of PbC142- in an aqueous solution is 0.0220 M. No Pb2+ or C ions are initially present. What is the concentration of Pb2+ ion present when equilibrium is achieved? [12 points]