Solubility & Net Ionic review Multiple Choice Identify the choice that best completes the statement or answers the question. 1. Which of the following statements is/are correct? 1. All ionic compounds that are soluble in water are electrolytes. 2. All ionic compounds dissolve in water. 3. Molecular compounds are never soluble in water. e. 2 and 3 2. Which of the following statements is/are correct? 1. Water soluble ionic compounds, such as NaCl, are strong electrolytes. 2. Some molecular compounds, such as HCl, are strong electrolytes. 3. Some molecular compounds, such as acetic acid, are weak electrolytes. 3. Which one of the following compounds is a nonelectrolyte when dissolved in water? a. HCl b. MgBr 2 c. Cl 2 d. Zn(NO 3) 2 e. KI 4. Which of the following statements is/are correct? 1. Most ionic compounds containing ammonium ion are insoluble in water. 2. Most ionic compounds containing nitrate ion are insoluble in water. 3. Most ionic compounds containing carbonate ion are insoluble in water. 5. Which of the following statements is/are correct? 1. Most ionic compounds containing phosphate ion are soluble in water. 2. Most ionic compounds containing chloride ion are soluble in water. 3. Most ionic compounds containing hydroxide ion are soluble in water.
6. Which of the following compounds are soluble in water: K 2CO 3, CaCO 3, NiCO 3, and Fe 2(CO 3) 3? a. K 2CO 3 only b. K 2CO 3 and CaCO 3 c. CaCO 3 and NiCO 3 d. NiCO 3 and Fe 2(CO 3) 3 e. CaCO 3, NiCO 3, and Fe 2(CO 3) 3 7. Which of the following compounds are soluble in water: Cu(NO 3) 2, Al 2S 3, Ba 3(PO 4) 2, and CaBr 2? a. Cu(NO 3) 2 only b. Cu(NO 3) 2 and Al 2S 3 c. Al 2S 3 and Ba 3(PO 4) 2 d. Ba 3(PO 4) 2 and CaBr 2 e. Cu(NO 3) 2 and CaBr 2 8. All of the following compounds are insoluble in water except. a. BaSO 4 b. AgI c. CuS d. Ca(ClO 4) 2 e. PbCrO 4 9. A precipitate will form when aqueous Pb(NO 3) 2 is added to an aqueous solution of. a. Cu(NO 3) 2 b. CaBr 2 c. NaCH 3CO 2 d. Ca(ClO 4) 2 e. NaNO 3 10. A precipitate will form when aqueous nickel(ii) chloride is added to an aqueous solution of. a. SrI 2 b. Cu(NO 3) 2 c. KOH d. Na 2SO 4 e. NaF 11. If an aqueous solution of is added to a mixture of Ba 2 and Fe 3, the barium ion will precipitate, but the iron ion will remain in solution. a. NaOH b. Na 2SO 4 c. K 3PO 4 d. KCl e. Pb(NO 3) 2 12. If an aqueous solution of is added to a mixture of F and SO 4 2, the fluoride ion will precipitate, but the sulfate ion will remain in solution. a. LiBr b. HNO 3 c. Pb(ClO 4) 2
d. AgNO 3 e. AlCl 3 13. What is the net ionic equation for the reaction of aqueous calcium acetate and aqueous sodium carbonate? a. Ca 2 (aq) 2 CH 3CO 2 (aq) Ca(CH 3CO 2) 2(s) b. Na (aq) CH 3CO 2 (aq) NaCH 3CO 2(aq) c. Na (aq) CH 3CO 2 (aq) NaCH 3CO 2(s) d. Ca 2 (aq) CO 3 2 (aq) CaCO 3(s) e. Ca 2 (aq) 2 Na (aq) CaNa 2(s) 14. What is the net ionic equation for the reaction of aqueous sodium hydroxide and aqueous iron(ii) chloride? a. Na (aq) OH (aq) NaOH(s) b. Na (aq) Cl (aq) NaCl(s) c. Fe 2 (aq) 2 OH (aq) Fe(OH) 2(s) d. Fe 2 (aq) OH (aq) FeOH (s) e. Fe 2 (aq) 2 Cl (aq) FeCl 2(s) 15. Which of the following compounds is a weak acid? a. HCl b. CH 3CO 2H c. HNO 3 d. HClO 4 e. H 2SO 4 16. What are the spectator ions in the reaction between aqueous hydrobromic acid and aqueous sodium hydroxide? a. Na only b. H and OH c. Na and Br d. Br only e. H, Br, Na, and OH 17. What are the spectator ions in the reaction between aqueous hydrochloric acid and ammonia? a. H only b. Cl only c. H and NH 4 d. Cl and NH 4 e. H, Cl, and NH 4 18. Formic acid, HCO 2H, is a weak acid. Write a net ionic equation for the reaction of aqueous formic acid and aqueous potassium hydroxide. a. HCO 2H(aq) KOH(aq) K (aq) HCO 2 (aq) H 2O( ) b. HCO 2H(aq) H 2O(aq) HCO 2 (aq) H 3O ( ) c. H (aq) OH (aq) H 2O( ) d. HCO 2H(aq) OH (aq) HCO 2 (aq) H 2O( ) e. H (aq) KOH(aq) K (aq) H 2O( ) 19. How many liters of 0.2805 M C 6H 12O 6(aq) contain 1.000 g of C 6H 12O 6? a. 0.001557 L b. 0.01979 L c. 0.2805 L d. 3.565 L
e. 50.5 L 20. If 5.15 g Fe(NO 3) 3 is dissolved in enough water to make exactly 150.0 ml of solution, what is the molar concentration of nitrate ion? a. 0.00319 M b. 0.0343 M c. 0.142 M d. 0.313 M e. 0.426 M 21. What is the mass of sodium iodide in 50.0 ml of 2.63 10 2 M NaI(aq)? a. 0.00132 g b. 0.00877 g c. 0.0788 g d. 0.197 g e. 78.8 g 22. What volume of 0.200 M Na 2SO 4(aq) will completely react with 50.0 ml of 0.135 M Ba(NO 3) 2(aq)? Na 2SO 4(aq) Ba(NO 3) 2(aq) BaSO 4(s) 2 NaNO 3(aq) a. 33.8 ml b. 67.5 ml c. 74.1 ml d. 148 ml e. 540. ml 23. A 25.00 ml sample of KOH is titrated with 21.83 ml of 0.2120 M HCl(aq). What is the concentration of the KOH solution? a. 0.0006720 M b. 0.002574 M c. 0.1851 M d. 0.2428 M e. 4.119 M
Solubility & Net Ionic review Answer Section MULTIPLE CHOICE 1. ANS: A PTS: 1 TOP: 3.5 Ions and Molecules in Aqueous Solutions 2. ANS: E PTS: 1 TOP: 3.5 Ions and Molecules in Aqueous Solutions 3. ANS: C PTS: 1 TOP: 3.5 Ions and Molecules in Aqueous Solutions 4. ANS: C PTS: 1 TOP: 3.5 Ions and Molecules in Aqueous Solutions 5. ANS: B PTS: 1 TOP: 3.5 Ions and Molecules in Aqueous Solutions 6. ANS: A PTS: 1 TOP: 3.5 Ions and Molecules in Aqueous Solutions 7. ANS: E PTS: 1 TOP: 3.5 Ions and Molecules in Aqueous Solutions 8. ANS: D PTS: 1 TOP: 3.5 Ions and Molecules in Aqueous Solutions 9. ANS: B PTS: 1 TOP: 3.6 Precipitation Reactions 10. ANS: C PTS: 1 TOP: 3.6 Precipitation Reactions 11. ANS: B PTS: 1 TOP: 3.6 Precipitation Reactions 12. ANS: D PTS: 1 TOP: 3.6 Precipitation Reactions 13. ANS: D PTS: 1 TOP: 3.6 Precipitation Reactions 14. ANS: C PTS: 1 TOP: 3.6 Precipitation Reactions 15. ANS: B PTS: 1 TOP: 3.7 Acids and Bases 16. ANS: C PTS: 1 TOP: 3.7 Acids and Bases 17. ANS: B PTS: 1 TOP: 3.7 Acids and Bases 18. ANS: D PTS: 1 TOP: 3.7 Acids and Bases 19. ANS: B PTS: 1 TOP: 4.5 Measuring Concentrations of Compounds in Solution 20. ANS: E PTS: 1 TOP: 4.5 Measuring Concentrations of Compounds in Solution 21. ANS: D PTS: 1 TOP: 4.5 Measuring Concentrations of Compounds in Solution 22. ANS: A PTS: 1 TOP: 4.7 Stoichiometry of Reactions in Aqueous Solution 23. ANS: C PTS: 1 TOP: 4.7 Stoichiometry of Reactions in Aqueous Solution