H2 Chemistry 10 - Chemistry of Aqueous Solutions: Solubility Product and Precipitation
What you will learn
- For this fixed-temperature exercise, use the given concentration-model value Ksp,c(BaSO4) = 1.1 x 10^-10 mol^2/dm^6. Neglect activity corrections and competing equilibria, and assume additive volumes when mixing 25.0 cm^3 of 0.010 mol/dm^3 BaCl2 with 25.0 cm^3 of 0.020 mol/dm^3 Na2SO4.
- Before precipitation, the initial concentrations after equal-volume mixing are halved: [Ba2+]0 = 0.0050 mol/dm^3 and [SO4 2-]0 = 0.010 mol/dm^3.
- The initial concentration product is Q0 =(0.0050)(0.010) = 5.0 x 10^-5 mol^2/dm^6, much greater than the supplied Ksp,c.
The displayed lesson text qualifies the supplied concentration model and distinguishes initial concentrations from equilibrium. The original audio and on-screen content are unchanged.
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