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.

2. Determine the equilibrium concentrations for each of the products and determine the molar solubility of Ca3(PO4)2.

pls complete the table using given dataEffect of Common Ions on the Solubility of Ca(OH)21. Add Ca(OH)2 to 250.0 mL of 0.010 M CaCl2 with stirring until equilibrium is achieved.2. Filter the undissolved precipitate. Measure out 50.0 mL of the filtrate in a 250-mL Erlenmeyer flask. 3. Add a few drops of phenolphthalein indicator and titrate with standardized HCl solution until endpoint is achieved. 4. Record the volume of HCl solution used. Perform two more trials.

Consider a solution that is 0.035 M Ca2+ and 0.068 M Pb2*. When K,SO, is added to the solution, what will be the first precipitate and what minimum concentration of K,SO, is required for this precipitate? Compound Kp CaSO, 7.10 x 10-5 PBSO4 1.82 x 10-8 O Caso, will precipitate fırst when [K,SO,) - 2.68 x 10-7 M. %3D O PbSO, will precipitate first when [K,SOl = 5.20 x 10-7 M. O PBSO, will precipitate first when [K,SO] = 2.68 x 10-7 M. O PbSO, will precipitate first when [K,SO.) - 2.03 x 10-3 M. O CasO, will precipitate first when [K,SO] = 2.03 x 10-3 M. D Question 17 Which of the following statements regarding BCI3 is CORRECT? O BCI, is a Lewis acid because B can donate a pair of electrons. BCI, is a Lewis acid because can accept a pair of electrons. BCI, is a Lewis acid because Cl can accept a pair of electrons. O BCI, is a Lewis base because Cl can donate a pair of electrons. BCI, is a Lewis base because B can donate a pair of electrons.