You have found the following: Pb+2(aq) + 4 I-(aq) <=> [PbI4]-2(aq) K = (2.853x10^4) What is the value of K for the following reaction? 3 Pb+2(aq) + 12 I-(aq) <=> 3 [PbI4]-2(aq)
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You have found the following:
Pb+2(aq) + 4 I-(aq) <=> [PbI4]-2(aq)
K = (2.853x10^4)
What is the value of K for the following reaction?
3 Pb+2(aq) + 12 I-(aq) <=> 3 [PbI4]-2(aq)
Step by step
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- Express the equilibrium constant for this reaction: 2 NH3(g) <=> N2(g) + 3 H2(g) K = [NH3]2 / ([NH3]2 x [N2]) K = ([NH3]2 x [N2]) / [H2]3 K = ([N2] x [H2]3) / [NH3]2Calculate the molar solubility of zinc carbonate in ZnCO3(s) Zn2+(aq) + CO32-(aq) Kps=3.10-8 Water: solubility = [ ] mol.L-1 • Zn (NO3) 2 solution 0.0500 mol.L-1: solubility = [ ] mol.L-1 • K2CO3 solution 0.0500 mol.L-1; solubility = [ ] mol.L-1The solubility of aqueous PbCr2O7 at 25 oC is 1.55 x 10–2 g/L at 25.0 oC. Calculate the Ksp of PbCr2O7 at this temperature. MM PbCr2O7 = 423.188 g/mol
- The Ksp value for magnesium arsenate [Mg3(AsO4)2] is 2.00 X 10-20 so if a chemist added 1.19 x 10-2 M of Pb3(AsO4)2(aq) which is a common ion then what would be the concentration of the Arsenate ion AsO43-(aq) in Molarity at equilibrium? 1.97 x 10-2 2.78 x 10-2 2.38 x 10-2 1.74 x 10-2 3.24 x 10-2 2.99 x 10-2 2.57 x 10-2 2.11 x 10-2 1.55 x 10-2 1.35 x 10-2Consider the following aqueous chemical equilibrium of benzoic acid, a weak acid: C6H5COOH(aq) + H2O(l) is in equilibrium with H3O+(aq) + C6H5COO-(aq) a. The addition of H3O+(aq) to the chemical equilibrium will have what effect on the amount (moles) of C6H5COO-(aq) in the system? b. Addition of OH-(aq) to the chemical equilibrium will have what effect on the amount (moles) of C6H5COOH(aq) in the system? c. Removal of C6H5COO-(aq) from the chemical equilibrium will have what effect on the amount of (moles) H3O+(aq) in the system? d. Increasing the pH of the solution will have what effect on the amount (moles) of C6H5COOH(aq) in the system?At 25oC, the ΔH o andΔH o for the following reaction is -24.7 kJ/mol and -49.9 J/mol-K, respectively. H2S (aq) + CN- (aq) ⇋ HS- (aq) + HCN (aq) If you mix 100 mL of 0.0450 M NaCN with 100 mL of 0.0450 M H2S, the reaction will proceed as indicated in the equation and will reach an equilibrium in the end. What will be the molar concentration of HCN at equilibrium?
- Consider the following equilibria:Ca(OH)2(s) ⇌⇌ Ca2+(aq) + 2 OH-(aq) K1 = 6.5 x 10-6 H2O(l) ⇌⇌ H+(aq) + OH-(aq) K2 = 1.0 x 10-14Given these equilibria, what is the equilibrium constant, K, for the following reaction?Ca(OH)2(s) + 2 H+(aq) ⇌⇌ Ca2+(aq) + 2 H2O(l)FeS has a Ksp of 3.72 x 10-19. What is the molar solubility of FeS? Write your answer to 3 sig figs, in the format 1.23E-4.1.1The Ksp of Ca3 (PO4 ) 2 is 1.3 × 10−26 . Estimate the solubility of this salt in units of g. L −1 . You must show any reaction equation(s) that you may think are necessary. 1.2 If a sample of solid Ca3(PO4)2 is stirred into exactly one litre of a 0.550M solution of Na3PO4, how will the solubility of the salt compare with the answer that you have obtained in question 1.1? Explain you answer in a short sentence.
- The concentration of a pure solid is left out of a equilibrium constant expression but a pure liquid is includedGiven the following reactions and their equilibrium constants,calculate the value for the overall formation constant forAg(NH3)2+. In addition, write the equilibrium expression forthe formation of Ag(NH3)2+.½Ag+(aq) + ½Cl–(aq) ⇋ ½AgCl(s) K1 = 7.45 x 104Ag(NH3)2+(aq) + Cl–⇋ AgCl(s) + 2NH3(aq) K2 = 323Ag+(aq) + 2NH3(aq) ⇋ Ag(NH3)2+(aq) Kf = ?If the equilibrium constants for the two reactions 2 HCl(g) H2(g) + Cl2(g) K1 = 4.36x10-2 and I2(g) + Cl2(g) 2 ICl(g) K2 = 8.92x10-6 are denoted K1 and K2 respectively, then the equilibrium constant, K3, for the reaction below is 2 HCl(g) + I2(g) 2 ICl(g) + H2(g) K3= ?