00 l of 0100 m cacl2 will a precipitate form the ions

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Unformatted text preview: ill form If If 2.00 mL of 0.200 M NaOH are added to 1.00 L of 0.100 M CaCl2, will a precipitate form? The ions present in solution: Na+, OH-, Ca2+, Cl-. Only possible precipitate is Ca(OH)2 Ca(OH) Is Q > Ksp for Ca(OH)2? [Ca2+] [OH − ]i = (0.002 L × 0.200 M ) /1L = 4.0 × 10 −4 M i = 0.100 M Q = [Ca 2 + ]i [OH − ]i = 0.10 × (4.0 × 10 −4 ) 2 = 1.6 × 10 −8 K sp = [Ca 2 + ]e [OH − ]e = 8.0 × 10 −6 Q < Ksp No precipitate will form Solubility Solubility and Common Ion Effect Will CaCO3 precipitate when 2.00 mL of 1.0×10-3 M CaCl2 is added to 50.0 mL of 0.020 M Na2CO3? Explain. CaCO 3 (s) 2Ca 2+ (aq) + CO 3 (aq) K sp = 4.5 × 10 −9 Q = [ Ca ][CO ] 2+ 23 [Ca 2+ ] = 1.0 × 10 −3 M × (2 mL 52 mL ) = 3.8 × 10 −5 M 2 [CO 3 - ] = 0.020 M × (50 mL 52 mL ) = 1.9 × 10 −2 M 2Q = [Ca 2+ ][CO 3 ] = 3.8 × 10 −5 × 1.9 × 10 −2 = 7.2 × 10 −7 Q = 7.2 × 10 −7 > 4.5 × 10 −9 YES! It will precipitate! What concentration of Ag+ is required to precipitate ONLY AgBr in a solution that contains both Br- and Cl- at a concentration of 0.02 M? AgBr (s) [Ag+] Ag+ (aq) + Br- (aq) Ksp = 7.7 x 10-13 Ksp = [Ag+][Br-] Ksp 7.7 x 10-13 = = = 3.9 x 10-11 M [Br-] 0.020 AgCl (s) -10 Ag+ (aq) + Cl- (aq) Ksp = 1.6 x 10 Ksp = [Ag+][Cl-] [Ag+] Ksp 1.6 x 10-10 = = 8.0 x 10-9 M -] = [Cl 0.020 3.9 × 10-11 M < [Ag+] < 8.0 × 10-9 M Factors That Affect Solubility (1) (1) Common...
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This document was uploaded on 02/26/2014.

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