Gravimetric determination of Kp. Table 1 Trial Volume of solution used (ml) Mass of empty beaker (g) Mass of beaker with solid residue (g) Mass Ca(OH)₂ (g) 10mL Ksp for Ca(OH)₂= 92.808g 92.766g 0.042g 1 Determine the mass of dissolved solid that was in the saturated solution. Calculate the molar solubility of the solution (M) using the mass of dissolved solid, the volume of solution used in analysis, and the molar mass of calcium hydroxide. Substitute the molar solubility into a versi of equation 4.1 [Hint: use an ICE table] to determine the Kp. Provide an annotated calculatio below:

Calculate the solubility at 25 °C of PbCO3 in pure water and in a 0.0070M Pb(NO3)2 solution. You'll find K sp Round both of your answers to 2 significant digits. solubility in pure water: x10 solubility in 0.0070 M Pb(NO3)2 solution: 20 170 L Ox 00 믐 ? data in the ALEKS Data tab.

One mixes aqueous NaCl with aqueous AgNO3. NaCl. AgNO3and NaNO3all have appreciable solubility in water. AgCl has a solubility product constant Ksp of 1.6 x 10-10. If one mixes the NaCl solution with the AgNO3solution, one would suspect: a) no precipitate will form   b)  AgCl precipitate will form  c) NaNO3 precipitate will form    d) both AgCl and NaNO3 precipitates will form

19" 0.00014 m Na2 Coz are combined? Determine the solubility of Cul (s) (Ksp.= 1.1x1013 In 0.15m Cu₂ (03 (aq) Solution,