Calculate the solubility-product constant for each of the following substances, given that the molar concentrations of their saturated solutions are as indicated: a. CuSeO3 (1.42 X 10-4 M). b. Pb(IO3)2 (4.3 X 10-5M). c. SrF2 (8.6 X 10-4 M). d. Th(OH)4 (3.3 X 10-4 M)

Answer the following questions about CaCO3. At 25°C the value of the solubility product constant, Ksp, for calcium carbonate is 3.4 X 10-9. b. Consider the solubility of CaCO3in the following aqueous solutions. i. Is the solubility of CaCO3in 0.10 M CaCl2 greater than, less than or equal to the solubility of CaCO3in pure water? Justify your answer.

Hydrofluoric acid is important in both pharmaceutical synthesis and the synthesis of Teflon. It can be produced by reacting H2 with F2, H2(g) + F2(g)-> 2 HF(g). If you ran the reaction with initial concentrations of H2 and F2 2.00M, what would the concentration of HF be at equilibrium? The Kc =115. a. 3.37 M Ob. 0.85 M Oc. C. 1.69 M Od. 4.00 M le. 2.85 M

Question 19 of 25 The molar solubility of Mg(CN)2 is 1.4 x 10-5 M at a certain temperature. Determine the value of Ksp for Mg(CN). NEXT Based on the given values, fill in the ICE table to determine concentrations of all reactants and products. Mg(CN) (s) Mg (aq) 2 CN-(aq) Initial (M) Change (M) Equilibrium (M) O RESET 1.4 x 105 -1.4 x 10-5 2.8 x 10-5 -2.8 x 10-5 +x +2x -2x 1.4 x 10-5 + x 1.4 x 10- + 2x 1.4 x 10-5 - x 1.4 x 10 - 2x 2.8 x 10-5 + x 2.8 x 10+ 2r -x 2.8 x 10-5 - x 2.8 x 10 - 2x