1- school district67 okanagan skaha（1 -学校district67 okanagan skaha）.doc

Chapter 3 - Solubility Practice Test #1 ? 6. The equation that represents the equilibrium in a saturated solution of Fe2(SO4)3 is A. Fe2(SO4)3(s) ? 3Fe2+(aq) + 2SO43-(aq) B. Fe2(SO4)3(s) ? 2Fe2+(aq) + 3SO43-(aq) C. Fe2(SO4)3(s) ? 3Fe3+(aq) + 2SO42-(aq) D. Fe2(SO4)3(s) ? 2Fe3+(aq) + 3SO42-(aq) ? 7. When equal volumes of 0.20 M K2CrO4 and 0.20 M AgNO3 are mixed, a red precipitate is formed. The net ionic equation for this reaction is ? A. K+(aq) + NO3-(aq) → KNO3(s) B. 2Ag+(aq) + CrO42-(aq) → Ag2CrO4(s) C. K2CrO4(aq) + 2AgNO3(aq) → Ag2CrO4(s) + 2KNO3(aq) D. 2Ag+(aq) + CrO4-(aq) + 2K+(aq) + 2NO3-(aq) → Ag2CrO4(s) + 2KNO3(s) ? 8. Which of the following compounds could be used to prepare a 0.20 M solution of hydroxide ion? ? A. KOH B. Fe(OH)3 C. Mg(OH)2 D. Zn(OH)2 ? 9. When 250 mL of 0.36 M Sr(OH)2 are added to 750 mL of water, the resulting ion concentrations are ? A. [Sr2+] = 0.12 M and [OH-] = 0.12 M B. [Sr2+] = 0.12 M and [OH-] = 0.24 M C. [Sr2+] = 0.090 M and [OH-] = 0.090 M D. [Sr2+] = 0.090 M and [OH-] = 0.180 M ? 10. When equal volumes of 2.0 M Pb(NO3)2 and 2.0 M KCl are mixed, A. a precipitate forms because the trial ion product Ksp B. a precipitate forms because the trial ion product Ksp C. a precipitate does not form because the trial ion product Ksp D. a precipitate does not form because the trial ion product Ksp ? 11. Consider the following equilibrium: AgCl(s) ? Ag+(aq) + Cl-(aq) When Br-(aq) is added to a saturated solution of AgCl, A. more AgCl dissolves and its solubility product increases. B. more AgCl precipitates and its solubility product decreases. C. more AgCl dissolves and its solubility product remains constant. D. more AgCl precipitates and its solubility product remains constant. 12. The molar solubility of iron II sulphide is A. 3.6 x 10-37 M B. 3.0 x 10-19 M C. 6.0 x 10-19 M D. 7.7 x 10-10 M ? 13. A solution containing an unknown cation