Chapter 16 Lecture 1

Chapter 16 Lecture 1 - but the fluoride is more soluble...

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Chapter 16 Lecture 1 The old definition of solubility If and only if you have a saturated solution: CaSO 4 (s) Ca 2+ + SO 4 - Ksp = [Ca 2+ ][SO 4 - ] Solubility Product Constant - Ksp Size of Ksp matters s - Molar solubility – moles of solid that dissolve per liter s ≠ Ksp Ksp can be used to find s
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Find solubility of SrSO 4 in water SrSO 4 (s) Sr 2+ + SO 4 2 - Let s = the moles of strontium sulfate that dissolve SrSO 4 (s) Sr 2+ SO 4 2 - I C E Ksp = [Sr 2+ ][SO 4 2 - ] = 3.2 X 10 - 7 Find the solubility of SrF 2 in water Ksp for strontium fluoride is 2.5 X 10 - 9
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Compare the solubilities: SrF 2 , Ksp = 2.5 X 10 - 9 , s = 8.5 X 10 - 4 SrSO 4 , Ksp = 3.2 X 10 - 7 , s = 5.6 X 10 - 4 Note: Ksp for the fluoride is 1/100 that of the sulfate.
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Unformatted text preview: but the fluoride is more soluble than the sulfate Comparing Ksp can not be used to compare solubilities. The common ion effect: Two sources of the same ion. Determine the solubility of Li 3 PO 4 in water. Ksp = 3.2 X 10-9 What is the concentration of each ion in solution? Li 3 PO 4 3Li + + PO 4 3-What happens if you add Na 3 PO 4 ? Discover the solubility of lithium phosphate in 1.0M sodium phosphate. To 1.0 g of LiCl is added to 125 mL of a saturated of lithium phosphate. What is the concentration of each ion in solution?...
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Chapter 16 Lecture 1 - but the fluoride is more soluble...

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