ws7302 - CN(aq K sp = 1.2 x 10-16 AgCl(s-Æ Ag(aq Cl(aq K...

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Work Sheet 7 —More Solubility Equilibria 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(NO 3 ) are added (you can ignore any volume change). The NaI, NaCl, and Cu(NO 3 ) are completely soluble (as is NaNO 3 but you already knew that). The K SP 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 K sp of PbCl 2 is 1.7 x 10 -5 . How many grams of PbCl 2 will dissolve in 100 mL of a 0.1 M NaCl solution? 3. Will CaF 2 be more soluble in acid or base? 4. Consider the following reactions AgCN(s) --- Æ Ag + (aq) +
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Unformatted text preview: CN-(aq) K sp = 1.2 x 10-16 AgCl(s) -Æ Ag + (aq) + Cl-(aq) K sp = 1.8 x 10-10 HCN (aq) ---Æ 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 HNO 3 D. Adding KCN E. Adding KNO 3 5. A blast from the past AgBr ( s ) ⇔ Ag + ( aq ) + Br − ( aq ) Ag + ( aq ) + 2 S 2 O 3 2 − ( aq ) ⇔ Ag ( S 2 O 3 ) 2 3 − ( aq ) S 2 O 3 2 − ( aq ) + H 3 O + ( aq ) ⇔ HS 2 O 3 − ( aq ) + H 2 O ( 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 Na 2 S 2 O 3 3. Adding HCl 4. Adding solid AgBr...
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This note was uploaded on 10/07/2011 for the course CHEMISTRY 51635 taught by Professor Laude during the Spring '10 term at University of Texas.

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ws7302 - CN(aq K sp = 1.2 x 10-16 AgCl(s-Æ Ag(aq Cl(aq K...

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