<p>Chem Worksheet: Ionic Reactions and Ksp. Block: ____ Name: ______</p><p>Solubility Rules. + - - - 1. All salts containing ions of Group IA, NH4 , NO3 , C2H3O2 (acetate ion), or CIO3 ARE SOLUBLE. - - - + + 2+ 2+ 2. Salts of Cl , Br , or I ARE SOLUBLE, EXCEPT with Ag , Cu , Hg2 , or Pb . 2- 2+ 2+ 2+ 2+ 2+ 3. Salts of SO4 ARE SOLUBLE, EXCEPT with Pb , Ca , Sr , Ba , or Ra . 4. Salts of OH- and S2- ARE NOT SOLUBLE, EXCEPT for Rule 1, or Ca2+, Sr2+, Ba2+ or Ra2+. 2- 2- 3- 2- 2- -2 5. Salts of O , CO3 , PO4 , SO3 , CrO4 , and SiO4 ARE, NOT SOLUBLE,, EXCEPT for Rule I.</p><p>1. Based upon the above rules, predict whether each of the compounds listed will be Soluble or Insoluble. a. K2CO3 ____ b. CaSO4 ______c. AgNO3 ______d. MnPO4 _____ e. PbI2 ______f. (NH4)2SO3 _____ g. Ca(OH)2 _____ h. Pb(C2H3O2)2 _____ i. AgI _____ j. Na2SiO4 _____ k. FeSO4 _____ m. WC14 _____</p><p>2. When the following ionic substances dissolve (however little) in water, into what ions will they dissociate? a. NH4Cl →______b. K2CrO4 →______c. Fe(OH)2 →______d. Co(C2H302)2 →______e. SnSO4 →______f. CaCl2 →______g. KSCN →______h. NaOH →______</p><p>3. For each of the following double replacement reactions occurring in water solution, write 3 balanced equations: one in “molecular” form , one in ionic form and one in net (ionic equation) form (leaving out spectator ions). Remember that in ionic forms insoluble materials (precipitates) must be written in molecular form. For example: Molecular: 1 NaCl (aq)+ 1 AgNO3 (aq) = 1 NaNO3 (aq) + 1 AgCl(s) (See solubility rules for why AgCl is (s)) + - + - + - Ionic: 1 Na (aq) + 1 Cl (aq) + 1 Ag (aq) + 1 N03 (aq) = 1 AgCl (s) + 1 Na (aq) + 1N03 (aq) + - Net Ionic: 1 Ag (aq) + 1 Cl (aq) = 1 AgCl (s) a. KI + Pb(Cl03)2 →</p><p> b. CaCl2 + (NH4)3PO4 →</p><p> c. Fe2(SO4 )3 + Ba(OH)2 → </p><p>+ - -16 4. For the reaction AgI(s) = Ag (aq) + I (aq) , the equilibrium constant (the solubility product), Ksp, has the value 1.5 x l0 . (a) Write the mass action expression for this reaction. (b) Calculate the concentration of Ag+ and I- ions in a saturated solution of AgI. (c) What is the solubility of AgI? --- how many moles of AgI can dissolve in a liter of solution?</p><p>-3 +2 - 5. The solubility of PbI2 is 1.5 x 10 moles per liter of solution. In a saturated solution of PbI2, calculate [Pb ] and [I ], and Ksp.</p>