(4) Calculate the pH of a solution made from the following mixtures. Ka (HAc) = 1.8×10-5 (a) 50.0 mL of 0.10 M HAc and 10.0 mL of 0.10 M NaOH (b) 50.0 mL of 0.10 M HAc and 50.0 mL of 0.10 M NaOH (c) 10.0 mL of 0.10 M HAc, 5.0 mL of 0.10 M NaOH, and 10.0 mL of 0.10 M NaAc
(5) Calculate the pH at the equivalence point when titrating 0.200 M solutions of each of the following bases with 0.200 M HBr: (a) hydroxylamine, NH2OH; Kb = 1.1×10 -8 (b) aniline, C6H5NH2 ; Kb = 4.3×10 -10
(1) The molar solubility of CaF2 at 35 oC is found to be 1.24×10 -3 mol/L. Calculate the Ksp for CaF2 .
(2) The solubility of BaSO4 in water is found to be 9.0mg/L at 25 oC. Calculate the Ksp for BaSO4 .
(3) A saturated solution of Ca3 (PO4 )2 has [Ca2+ ] = 2.01×10 -8 and [PO43-] = 1.6×10 -5. Calculate the Ksp for Ca3 (PO4 )2 .
(4) A saturated solution of Ag2CrO4 in water has [CrO42-] = 6.5×10 -5. Calculate the Ksp for Ag2CrO4 .
(5) Calculate the molar solubility of each of the following slightly soluble compounds. (a) FeCO3 , Ksp = 2.1×10 -11 (b) Al(OH)3 , Ksp = 4.6×10 -33
(6) A 45.0 mL sample of 0.0015 M BaCl2 is added to a beaker containing 75.0 mL of 0.0025 M KF. Will a precipitate form?
(7) How many moles of calcium chloride, CaCl2 , can be added to 1.5 L of 0.020 M potassium sulfate, K2SO4 , before a precipitate is formed? Assume that the volume of the solution is not changed significantly by the addition of calcium chloride. Ksp (CaSO4 ) = 2.4×10 -5
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