VIEWS: 10 PAGES: 7 POSTED ON: 1/5/2012
3rd Nine-Weeks Week # 06 AP Chemistry CW 04: Solubility Product Name: ______________________________________ Date: _________ Period: __________ 1. Given the following reaction: Bi2S3 (s) 2 Bi3+ (aq) + 3 S2- (aq) a. Write the solubility product constant expression. b. If the solubility of Bi2S3 is 1.00 x 10-15 M at 25 ºC, calculate the Ksp. 2. Given the following reaction: Ag2Cl2O7 (s) 2 Ag1+ (aq) + Cl2O72- (aq) a. Write the solubility product constant expression. b. If the solubility of the substance is 3.68 x 10-3 M, calculate the Ksp. c. What is the concentration of Cl2O72- ions, if 0.1 moles of AgNO3 is added to the solution? 3. Given the following reaction: Al(OH)3 (s) Al3+ (aq) + 3 OH1- (aq) a. Write the solubility expression. b. Given the Ksp = 2.00 x 10-32, calculate the concentration of aluminum ions and hydroxide ions at equilibrium. 4. Given the following reaction: Ba3(PO4)2 (s) 3 Ba2+ (aq) + 2 PO43- (aq) a. Write the solubility expression. b. Given a Ksp = 6.00 x 10-39, calculate the solubility of the compound. c. Calculate the barium ion concentration if 2.05 x 10-5 moles of K3PO4 is added to the solution. 5. Determine if the following solutions will form a precipitate. a. 250. mL of 0.057 M Ba(NO3)2 and 500. mL of 0.0337 M Na3PO4 The Ksp for Ba3(PO4)2 is 6.00 x 10-39 . b. 500. mL of 1.02 x 10-5 M CaCl2 and 750. mL of 2.03 x 10-7 M NaOH The Ksp for Ca(OH)2 is 1.30 x 10-6. 6. Given the following reaction: Fe(OH)2 (s) Fe3+ (aq) + 3 OH1- (aq) a. Write the Ksp expression. b. If the solubility of Fe(OH)3 is 4.49 x 10-10 M, calculate the Ksp. c. If 0.035 moles of NaOH are added to 1 L of the Fe(OH)3 solution, calculate the concentration of [Fe3+]. 7. Given the following reaction: PbBr2 (s) Pb2+ (aq) + 2 Br1- (aq) a. Write the Ksp expression. b. Calculate the [Pb2+] and [Br1-] if Ksp = 2.1 x 10-6. c. If 0.154 moles of Pb(NO3)2 are added to 1 L of PbBr2 solution, calculate the [Br1-]. 8. Given the following reaction: Ag3PO4 (s) 3 Ag1+ (aq) + PO43- (aq) a. Write the Ksp expression. b. Calculate the molar solubility of Ag3PO4 if the Ksp = 2.8 x 10-18. c. If 0.25 moles of AgNO3 are added to 1 L of the Ag3PO4 solution, what is the [PO43-]? 9. Determine if the following solutions will form a precipitate. a. 500. mL of 2.15 x 10-4 M Ca(NO3)2 is added to 850. mL of 3.05 x 10-3 M NaOH. The Ksp for Ca(OH)2 is 6.5 x 10-6. b. 400. mL of 0.025 M Au(NO3)3 is added to 950. mL of 0.00375 M NaCl. The Ksp for AuCl3 is 3.2 x 10-25. 10. Fe(OH)2 (s) Fe2+(aq) + 2 OH1- (aq) a. Write the solubility-equilibrium expression. b. The molar solubility for Fe(OH)2 is 1.26 x 10-2 M. Calculate the Ksp. c. Using the Ksp from part b, calculate the [Fe2+] after 0.0357 moles of KOH is added to 1-liter of the iron (II) hydroxide solution? 11. Ca3(PO4)2 (s) 3 Ca2+ (aq) + 2 PO43- (aq) a. Write the solubility-equilibrium expression. b. If the Ksp is 2.10 x 10-33, calculate the molar solubility of Ca3(PO4)2. c. Using the Ksp in part b, determine the effect in the concentration of the calcium ion if 0.0155 moles of Na3PO4 is added to 1-liter of the solution. 12. Zn(OH)2 (s) Zn2+ (aq) + 2 OH1- (aq) a. Write the solubility-equilibrium expression. b. The Ksp for Zn(OH)2 is 3.00 x 10-17. Calculate the [Zn2+] and the [OH1-]. c. Using the Ksp from part b, calculate the changes in concentration to the hydroxide ion, OH1-, if 0.00345 moles of Zn(NO3)2 is added to 1-liter of the solution. 13. (a). Predict whether a precipitate of PbCl2 will form if 100. mL of 0.0100 M NaCl is added to 250. mL of 0.0200 M Pb(NO3)2. The Ksp for PbCl2 is 1.70 x 10-5. (b) Will a precipitate from when 1.00 L of 0.150 M MgCl2 solution is mixed with 2.00 L of 0.0333 M Na3PO4 solution? The Ksp for Mg3(PO4)2 is 1.00 x 10-24.