Calculate the concentrations of each aqueous cobalt-containing species in a solution saturated with Co(OH)2(s), and having a fixed OH− concentration of 3.02×10−4 M. The equilibrium constants for the equilibria that occur in the solution are given in the table. d) [Co(OH)−3] = _________________________________ M e) [Co(OH)2−4] = ___________________________________ M

A 100.-mL sample of solution contains 10.0 mmol of Ca 2+ ion. How many mmol of solid Na 2SO 4 must be added in order to cause precipitation of 99.9% of the calcium as CaSO 4? The K sp of CaSO 4 is 6.1  × 10 –5. Assume the volume remains constant.   a. 10.0   b. 17.4   c. 71.0   d. 6.1   e. 61.0

2. Calculate the molar solubility of lead(II) phosphate in a pH 10 solution. Pb3(PO4)2(s) 3 Pb²+ (aq) + 2 PO4³- (aq) Pb²+ (aq) + 3 OH(aq) Pb(OH)3(aq) Ksp = 1.0 x 10-54 Kf = 8.0 x 1013 Pb3(PO4)2(s) + 9 OH(aq) 3 Pb(OH)3 (aq) + 2 PO4³- (aq)

2H2O → H3O+ + OH- To decrease the concentration of H3O+ ions in the iquilibrium above, you could a. add an acid to the solution b. add a base to the solution c. add a catalyst to the solution d. more than one choice is correct

Silver carbonate has a Ksp = 3.33×10-12 and a solubility of 0.00009407 M in water. Solid silver carbonate is placed into a silver nitrate solution. What concentration of silver nitrate is necessary to reduce the solubility of the silver carbonate to 1×10-8 M? [AgNO3] = _____ M

QUESTION 7 In the following scenarios, determine whether the reaction will proceed forward, reverse, or if equilibrium is reached: CaC204(0) Ca (aq) +C₂O4(q) The ion product constant is 2.5 x 10-10. The solubility product constant is 2.3 x 10" a. b. C. PbCl2 Pb² + 2Cl The ion product constant is 5.0 x 10. The solubility product constant is 1.6 x 10-5 BaSO4) Ba²+ SO4² The ion product constant is 2,5 x 10. The solubility product constant is 1.1 x 10-10

Write the solubility equilibrium constant expression for silver phosphate Show the ICE Table and calculate the solubility product constant of silver phosphate, given the molar solubility is 1.80 x 10-5. Ksp silver phosphate = _________

A 15.0 mL sample of a 0.437 M aqueous nitrous acid solution is titrated with a 0.441 M aqueous potassium hydroxide solution. What is the pH at the start of the titration, before any potassium hydroxide has been added?pH = __________

How many moles of Ca2+ and OH-ions are produced for every one mole of Ca(OH)2 that dissolves in solution? Ca(OH)2(s)↔Ca2+(aq) + 2OH–(aq)

1]  A student titrates a 20.00 mL sample of a solution of HBr with unknown molarity. The titration requires 20.05 mL of a 0.1819 M solution of NaOH. What is the molarity of the HBr solution? Solution:                                                                                            Final answer:____________   2]  Vinegar can be assayed to determine its acetic acid content. Determine the %(w/v) of acetic acid in a 15.00 mL sample of vinegar that requires 22.70 mL of a 0.5500 M solution of NaOH to reach the equivalence. Solution:                                                                                            Final answer:____________   3]  The calcium in a 5.00-mL serum sample is precipitated as CaC2O4 with ammonium oxalate. The filtered precipitate is dissolved in acid, the solution is heated, and the oxalate is titrated with 0.00100 M KMnO4, requiring 4.94 mL. Calculate the concentration of calcium in the serum in meq/L (equivalents based on charge). Solution:…