Work Sheet 8+ CH302 Spring 2008 1. A solution is made with NaI and NaCl such that it is 0.01 M in both I- and Cl-. To 1 L of this solution 0.01 moles Cu(NO3) are added (you can ignore any volume change). The NaI, NaCl, and Cu(NO3) are completely soluble (as is NaNO3 but you already knew that). The KSP for CuI is 1.3 x 10-12 and for CuCl is 1.0 x10-6. After the solution has reached equilibrium what are the concentrations of the following? [Cu+] [I-] [Cl-] Are there any solid precipitates? If so how many grams of each. 2. The Ksp of PbCl2 is 1.7 x 10-5. How many grams of PbCl2 will dissolve in 100 mL of a 0.1 M NaCl solution? 3. Will CaF2 be more soluble in acid or base? 4. Consider the following reactions AgCN(s) --- Ag+(aq) + CN-(aq) Ksp = 1.2 x 10-16 AgCl(s) - Ag+(aq) + Cl-(aq) Ksp = 1.8 x 10-10 HCN (aq) --- H+(aq) + CN-(aq) You a saturated solution of AgCN, what will the effect of each of the following (nothing, more AgCN dissolves, some AgCN precipates) A. Adding NaCl B. Adding HCl C. Adding HNO3 D. Adding KCN E. Adding KNO35. A blast from the past ! AgBr(s) " Ag+(aq) + Br#(aq)Ag+(aq) + 2S2O32#(aq) " Ag(S2O3)23#(aq)S2O32#(aq) + H3O+(aq) " HS2O3#(aq) + H2O(l) What is the effect of each of these on the solubility of AgBr(s) 1. Adding the soluble salt Kbr 2. Adding the soluble salt Na2S2O3 3. Adding HCl 4. Adding solid
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