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 =     K sp / K a =

4. Unlike most silver salts, silver fluoride is very soluble in water. AgF(s) Ag (aq) + F(aq) AgCl(s) Ag (aq) + Cl(aq) a) Calculate the molar solubility of silver fluoride. Keq = 183.8 Keq = 1.8 x 10-10 b) What is the pH of a concentrated solution of silver fluoride? c) Provide an explanation for the difference in solubility between silver fluoride and silver chloride.

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

What is the molar solubility of Fe(OH)3 in a solution buffered at pH = 4.29? See the Solubility Product Constant Table. 4.0 8.1e-9 What is the molar solubility at pH = 9.00? 4.0 6.00-23 X M Substance Ksp at 25 °C Aluminum Al(OH)3 1.9 x 10-33 Barium Ba(OH)2 BaCO3 BaSO4 XM 5.0 x 10-3 8.1 x 10-9 1.1 x 10-10 Ba3(PO4)2 3.4 x 10-23 Cadmium Cd(OH)2 CdCO3 CdS Calcium 2.5 x 10-14 5.2 x 10-12 8.0 x 10-27 Ca(OH)2 5.5 x 10-6 CaCO3 4.8 x 10-⁹ Ca3(PO4)2 1.0 x 10-26 CaF2 3.9 x 10-11 Chromium CO(OH)2 COS Cr(OH)3 6.3 x 10-31 Cobalt 1.6 × 10-15 4.0 x 10-21 Copper Cu(OH)2 Cu₂S CUCO3 CuS Iron Fe(OH)2 FeS Fe(OH)3 FePO4 Lead Pb(OH)2 PbF2 PbCl₂ PbBr₂ Pbl2 PbCrO4 PbSO4 PbS 2.2 x 10-20 1.6 x 10-48 1.4 x 10-10 6.3 x 10-36 Mg(OH)2 8.0 x 10-16 6.3 x 10-18 2.5 x 10-39 9.9 x 10-29 2.8 x 10-16 3.7 x 10-8 1.7 x 10-5 6.3 x 10-6 6.5 x 10-⁹ 1.8 x 10-14 1.7 x 10-8 8.4 x 10-28 Magnesium 1.8 × 10-11 Manganese Mn(OH)2 MnCO3 MnS Nickel Ni(OH)2 Silver AgCl AgBr Agl AgCN Ag₂S Ag₂ CrO4 Ag3PO4 Tin Sn(OH)2 SnS Zinc ZnCO3 Zn(OH)2…