Consider the insoluble compound copper (II) carbonate, CuCO3. The copper(II) ion also forms a complex with ammonia. Write a balanced net ionic equation to show why the solubility of CuCO3 (s) increases in the presence of ammonia and calculate the equilibrium constant for this reaction. For Cu(NH3)42+ , K = 6.8x10¹2. Be sure to specify states such as (aq) or (s). K= + ?

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 = ________

The generic metal A forms an insoluble salt AB(s) and a complex AC, (aq). The equilibrium concentrations in a solution of AC, were found to be [A] = 0.100 M, [C] = 0.0270 M, and [AC5] = 0.100 M. Determine the formation constant, Kf, of AC5. K₁ = x100 The solubility of AB(s) in a 1.000 M solution of C(aq) is found to be 0.174 M. What is the Ksp of AB? Ksp= 6.59 x10-8

Consider the insoluble compound zinc carbonate, ZnCO3. The zinc ion also forms a complex with hydroxide ions. Write a balanced net ionic equation to show why the solubility of ZnCO3 (s) in presence of hydroxide ions and calculate the equilibrium constant for this reaction. For Zn(OH)42, K₁= 2.9x1015. Be sure to specify states such as (aq) or (s). K=

The equilibrium constant for the formation of Cu(CN)42- is 2.0 x 1030. Calculate the value of pCu2+, or -log[Cu2+], if 2.21 g of CuCl2 is dissolved in 1.000 L of a 0.926 M solution by NaCN. The addition of CuCl2 does not affect the volume (the final volume is always 1,000 L).

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

Write a balanced net ionic equation to show why the solubility of Zn(OH)₂(s) increases in the presence of a strong acid and calculate the equilibrium constant for the reaction of this sparingly soluble salt with acid. Be sure to specify states such as (aq) or (s). K= + +

0.268 mol AGNO, and 3.10 mol NH, were added to enough water to give 1.00 L of solution at 25 °C. Calculate the equilibrium concentration of free silver ion , [Ag*), in this solution. The formation constant for Ag(NH3),* (K,) = 1.50x107 at 25 °C. O 0x10° M O 2.23×10° M O 2.73x10° M 4.85x10° M 6.97x10° M

Consider the insoluble compound zinc carbonate, ZnCO3. The zinc ion also forms a complex with hydroxide ions. Write a balanced net ionic equation to show why the solubility of ZnCO3 (s) increases in the presence of hydroxide ions and calculate the equilibrium constant for this reaction. For Zn(OH)4²-, Kf = 2.9×10¹5. Be sure to specify states such as (aq) or (s). K = + Submit Answer + Retry Entire Group 2 more group attempts remaining

Upon analyzing a seawater sample, it was found that the concentration of bicarbonate ions (HCO3-) is 0.09 m, the activity of calcium ions (Ca2+) is 10^-6, and the pH of the seawater sample is 8.0. (a) Will calcite precipitate in this seawater sample? (b) Calculate the required activity of Mg2+ ions for dolomite to precipitate.