The formation constant of a complex ion [M(NH3)4]2+(aq) is 8.8E8. If a solution is prepared by adding 0.4 mol of [M(NH3)4]Cl2 to 525.0 mL of water, what is the equilibrium concentration of free M2+(aq) ions? Include 3 significant figures

Consider the insoluble compound silver hydroxide , AgOH . The silver ion also forms a complex with cyanide ions . Write a balanced net ionic equation to show why the solubility of AgOH (s) increases in the presence of cyanide ions and calculate the equilibrium constant for this reaction.For Ag(CN)2- , Kf = 5.6×1018 . Be sure to specify states such as (aq) or (s).   Net Equation= _________ K = ________

What is the concentration of [Ag(S2O3)2]3- in a solution which contains 7.5 x 10-7 M Ag+ ions and 1.5 x 10-6 M S2O32- ions?   The Kf for [Ag(S2O3)2]3- is 4.7 x 1013.

The formation constant of a silver cyano complex is 5.6 x 1018 Ag+ + 2 CN Ag(CN)," If a certain solution have the equilibrium concentrations of 5.0 x 10-3 M and 0.20 M for Ag+ and CN", respectively, then what is the equilibrium concentration for the silver cyano complex? O1.1 x 1015 O5.6 x 1015 02.8 x 1016 02.4 x 109

For the aqueous [HgI4]complex Ky = 6.76 × 1029 at 25 °C. Suppose equal volumes of 0.0062 M Hg (NO3)2 solution and 0.42M Nal solution are mixed. Calculate the equilibrium molarity of aqueous Hg** ion. Round your answer to 2 significant digits. ☐ M

7.00 grams of Cobalt (II) nitrate are dissolved in 1.00 liter of water. What is the initial concentration of CO (2+) in moles per liter? Then, 0.22 moles of solid KOH are added to this solution. The solution volume remains 1.00 liter. Given that Kf = 5.0 x 10^9 for the complex ion, Co(OH)4 (2-) find the final concentrations of Co (2+), Co(OH)4 (2-), and OH-. Also find the pH of this final solution.

The generic metal A forms an insoluble salt AB(s) and a complex AC5(aq). The equilibrium concentrations in a solution of AC5 were found to be [A]=0.100 M, [C]=0.0230 M, and [AC5]=0.100 M. Determine the formation constant, Kf, of AC5. Kf = 155367729.8   The solubility of AB(s) in a 1.000 M solution of C(aq) is found to be 0.152 M. What is the Ksp of AB? Ksp = ?

For the aqueous [Ag (NH3)₂ complex K₁=1.12 × 107 at 25 °C. + Suppose equal volumes of 0.0042M AgNO3 solution and 0.86M NH3 solution are mixed. Calculate the equilibrium molarity of aqueous Ag ion. Round your answer to 2 significant digits. M x10 Times 10 to an exponent

The chemical reaction for the formation of the red-orange iron(III) thiocyanate complex ion is Fe3+ (aq) +  SCN- (aq)  <==> [FeSCN2+] (aq)   What is the source of the Fe3+ ions?   What is the source of the SCN- ions?   The equilibrium constant for this reaction is given by what