1. Calculate a predominance diagram showing the solubility of Ferric hydroxide [Fe(OH)3(s)] as a function of solution pH by plotting the logarithm of the concentration of each iron species against pH assuming the solution is in contact with ferric hydroxide mineral. (10 pts) Before beginning, answer these questions: i) Is this solution open or closed with respect to iron? (2 pts) ii) If open, what is the reservoir for iron? (2 pts) ● ●

A 0.125-M solution of 0.075 Mn(NO3)2 is saturated with H2S([H2S]=0.10M). At what pH does Mns begin to precipitate?. MnS(s)Mn2+(aq)+S2(aq)Ksp=4.31022 H2S(aq)+2H2O(l)2H3O+(aq)+S2(aq)K=1.01026

1. (Total 20 pts) Calculate a predominance diagram showing the solubility of Spertiniite - a rare Cu(II) hydroxide mineral, Cu(OH)2(s) - as a function of pH by plotting the logarithm of the concentration of each copper species against pH assuming the solution is in contact with Spertiniite. Consider only the following aqueous species: Cu²+; CuOH+; Cu(OH)2; Cu(OH)3. A. Write the reactions that form the aqueous species from Cu(OH)2(s) and the corresponding equilibrium relations. The equilibrium constants for the formation of the 4 aqueous species listed above are 108.68; K₂ = 100.98; K3 = 10–5; K4 = 10-18.2. (10 pt) B. Write the mass balance equation for the solution. (3 pt) C. Plot the total concentration of the dissolved species in a predominance diagram and indicate on the diagram the regions where the solution is oversaturated and undersaturated with Cu(II). Hint: The diagram can be drawn by hand. (7 pt) K₁ =

Determine the molar solubility (S) of Ag, CO, in a buffered solution with a pH of 4.983 using the systematic treatment of equilibrium. K(Ag,co.) = 8.46 x 10-12; K(H,CO,) = 4.45 x 10-7; K2(H,CO,) = 4.69 x 10. M