Chapter 16 Lecture 1

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

This preview shows pages 1–5. Sign up to view the full content.

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

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
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
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.

This preview has intentionally blurred sections. Sign up to view the full version.

View Full Document
This is the end of the preview. Sign up to access the rest of the document.

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?...
View Full Document

{[ snackBarMessage ]}

### Page1 / 5

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

This preview shows document pages 1 - 5. Sign up to view the full document.

View Full Document
Ask a homework question - tutors are online