Write a balanced net ionic equation to show why the solubility of BaF2(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 =

Calculate the solubility of Mn(OH), in grams per liter when buffered at pH = 9.7. Express your answer using two significant figures.

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

27) Assuming that no equilibria other than dissolution are involved, calculate the concentrations of ions in a saturated solution of each of the following (see Appendix J for solubility products): (a) AgI (b) Ag2SO4 (c) Mn(OH)2 (d) Sr(OH)2·8H2O (e) the mineral brucite, Mg(OH)2

By controlling the pH of an aqueous solution it is possible to control the formation of a precipitate (thesolid form) for a slightly soluble ionic compounds. As an example, consider an aqueous solution with[Zn2+] = 2.3 x 10^-4 M. Note that the solubility product for zinc hydroxide (Zn(OH)2) is Ksp = 4.1 x 10^-17.a) At what value for pH will Zn(OH)2 solid first form?b) What percent of the initial concentration of Zn2+ ion will have formed solid at pH = 9.00?

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

Calculate the pH for each case in the titration of 50.0 mL of 0.180 M HCIO(aq) with 0.180 M KOH(aq). Use the ionization constant for HC1O. What is the pH before addition of any KOH? КОН? pH = %3D What is the pH after addition of 25.0 mL KOH? pH = What is the pH after addition of 30.0 mL KOH? pH = What is the nH after addition of 50.0 ml. KOH? Question Source: McQuarrie, Rock, And Gallogly 4e General Chemsitry | Publisher: Ur

Write a balanced net ionic equation to show why the solubility of Mg(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). Mg(OH)2(s) + 2HCl(aq)   MgCl2(aq) + 2H2O(l) K =

In some natural systems the pH must be maintained within very narrow limits. e.g. in human blood the pH must remain close to 7.4 or cell deterioration occurs. Blood contains several weak acid/conjugate base equilibria called buffers, which control the pH.One weak acid present in blood is the dihydrogen phosphate ion, H2PO4-(aq), for which the equilibrium in aqueous solution is H2PO4-(aq) +H2O(l) <--> HPO42-(aq) + H3O+(aq). a) What would be the effect on this equillibrium of adding hydrochloric acid solution?b) Write the expression for the equilibrium constant of this reaction.c) If 0.5 mol H2PO4- and 0.5 mol HPO42- are in equilibrium in 1.0L of aqueous solution, calculate the pH of the solution. (Ka for H2PO4-= 6.4 x 10-8)d) 0.010 mol HCl is now added to the 1.0L of the solution in c). Assuming that all the added H+ ions are used up in the equilibrium shift, calculate the concentrations of H2PO4- and HPO42-. Hence calcuate the pH of this solution.e) 0.010 mol HCl has been added…

Consider the insoluble compound zinc sulfide, ZnS . The zinc ion also forms a complex with hydroxide ions. Write a balanced net ionic equation to show why the solubility of ZnS (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= + +