Type 7 Predicting Solubility ksp3 note3 (1)

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Nov 24, 2024

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Predicting Solubility (pg. 487) Sect.7.6 - use a Qsp value which is compared to known Ksp values!!! 1) Use given information to create a balanced equation (double displacement equation) 2) Show the precipitate equilibrium equation (dissociation equation!!) 3) Find the molar [ions] for new solution 4) Solve for Qsp - based on the [ions] Ksp value represent saturation-maxiumum ions in solution before precipitate if Qsp > Ksp (look in table or given); Qsp=Ksp ; Qsp<Ksp --therefore precipitate forms saturated; unsaturated-no precipitate Qsp No I.C.E table required ex. 100mL of a 0.100M CaCl2 is mixed with 100.0mL of 0.0400M Na2 SO4. Will a (4 marks precipitate form.(4 marks) To solve- 2 chemical equations required 1) Double displacement to identify precipitation 2) Precipitate equation that creates Ksp -> What creates the equilibrium?! Determine the [each ion] that creates precipitate then Qsp compared to Ksp!! ( Ans: Qsp> Ksp, therefore precipitate (Qsp= 0.00100 )) Qsp vs Ksp
Ex.2 55.0mL, 1.6x10 -4 M Pb(NO 3 ) 2 (aq) reacted with 456.0mL of 2.3x10-4M NaCl. Determine if a precipitate forms. 1) Write chemical equations + look up Ksp in table(pg.802) ( ANS Qsp= 7.24x10 -13 < Ksp-- no precipitate ) HW Pg. 489#5; pg. 493#10
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