From the value Kf = 1.2 × 10º for Ni(NH3)62+ , calculate the concentration of NH3 required to just dissolve 0.014 mol of NiC2O4 (Ksp = 4 × 10-10 ) in 1.00 L 2- because the solution will of solution. (Hint: You can neglect the hydrolysis of C2 04 be quite basic.)
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- Given that the Ksp for silver chloride is 1.76 x 10-10, and the Kf of silver(I) diammine cation [Ag(NH3)2 +] is 1.7 x 107, calculate the maximum number of grams of silver chloride that will dissolve in 250.0 mL of a 3.25 M solution of ammonia.An aqueous solution is prepared in which 0.00113 mol Ni(NO3)2 and 0.484 mol NH3 are dissolved in a total volume of 1.00 L. Kf for Ni(NH3)62+ is equal to 5.5 × 108. Calculate the concentration of Ni(H2O)62+ ions at equilibrium in the solution formedThe value of Ksp for Cd(OH)2 is 2.5 x 10-14. (a) Whatis the molar solubility of Cd1OH22? (b) The solubilityof Cd(OH)2can be increased through formation of thecomplex ion CdBr42 - (Kf = 5 x 103). If solid Cd(OH)2 isadded to a NaBr solution, what is the initial concentrationof NaBr needed to increase the molar solubility of Cd(OH)2to 1.0 x 10-3 mol/L?
- Calculate the concentration of [Ag(S2O3)2]3- in a solution which contains 8.5E-6 M Ag+ ions and twice that molar concentration of thiosulfate ions at equilibrium? The Kf for [Ag(S2O3)2]3- is 4.7 x 1013. Your answer should have 2 sig figs.Calculate the (Ka) value for the reaction of CH3COOH with NH3 that the pH of the solution is (6.46) and the (Kb = 1.75 x 10 5).the overall equilibrium constant for the reaction of hexaaquairon(II) with 2 mol of acetate to form diacetatotetraaquairon(II) is 120, wheras that for the reaction with 1 mol of malonate, -OOCCH2COO-, is 630. Write equations representing these reactions and briefly rationalize the differences in the magnitudes of the equilibrium constants.
- Please answer with the work shown Ű Ċ 6. Using hard-soft concepts, indicate (by circling) whether the following reactions will have an equilibrium constant greater than or less than 1. a. R3PBBr3 + R3NBF3R3PBF3 + R3NBBr3 b. [AgCl₂] (aq) + 2CN- (aq) [Ag(CN)₂] (aq) + 2Cl(aq) Answer: Answer: K> 1 or K 1 or K <1Which of these expressions correctly expresses the solubilityproductconstant for Ag3PO4 in water?(a) [Ag][PO4] (b) [Ag+][PO43 - ] (c) [Ag+]3[PO43 - ](d) [Ag+[[PO43 - ]3 (e) [Ag+]3[PO43 - ]31. What mass of solid Lanthanum (II) oxalate nonahydrate { La2 ( C204 )3 9 H20 } can be obtained from 650 mL of 0.0170 M aqueous solution of LaCl3 by adding a stoichiometric amount of sodium oxalate ?
- Which of the following expression can be used to calculate the equilibrium constant involving the 3- 2+ 4- 3+ Fe(CN), + Cr = Fe(CN)," + Cr reaction: Select one: log Keq = (E°cr E"(Fe(CN)61)/0.0592 log Keq = {2(E°Fe(CNIGI - E°C, )}/0.0592 Cr· O log Keq = (E°, - E°C, )/0.0592 [Fe(CN)6] log Keq = {2(E°. Cr E"(Fe(CN)6)}/0.0592 E°,ΔG = -RT ln Ka, with Ka that represents the association constant for a complex. (a) Write an expression of ΔG as a function of Kd, the dissociation constant for the same process. (b) Calculate the change in ΔG (thus, the value of ΔΔG) if you consider a 10-fold stronger association for the complex (hint: you don’t need to know the actual values of Ka, Kd, or ΔG). Assume the temperature equal to 25°C.Given this series of equilibrium reactions. See Image(a) Which way should the reaction to “tend” at high pH? Why?(b) Which way should the reaction to “tend” at low pH? Why? (c) What Fe(III) species would be least soluble?