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AAMC 8 PS #46 / Solubility Question

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letaps

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Hey,

I had a question about Ksp and solubilities. The lower the Ksp, the less soluble the compound is, and thus there will be less anions/cations in the solutions. Conversely, the higher the Ksp, the more soluble the compound is and thus there will be more cations/anions. Does that sound right?

Using the below question as an example, is this the correct reasoning: The one with the lowest Ksp, which is BaSO4, will be the least soluble. Therefore, a BaSO4 solution will be primarily BaSO4 (instead of Ba2+ ions and SO42- ions). The one withe highest Ksp, which is BaF2, will be the most soluble and therefore a BaF2 solution will be primarily Ba2+ and F- ions. Does that sound correct?


Ba2+(aq) is an ion that is very toxic to mammals when taken internally. Which of the following compounds, mixed in water, would be the safest if accidentally swallowed?

A) BaSO4, Ksp = 1.1 ´ 10–10
The lower the value of Ksp is, the lower the concentrations of the cation and anion in an aqueous solution and the lower the solubility of the compound in water. If mixed with water and accidentally swallowed, the Ba salt with the lowest value of Ksp would be the safest. Thus, A is the best answer.


B) BaCO3, Ksp = 8.1 ´ 10–9
C) BaSO3, Ksp = 8.0 ´ 10–7
D) BaF2, Ksp = 1.7 ´ 10–6
 

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