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12 Cards in this Set
- Front
- Back
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Where is solubility used?
Hint: Three basic techniques |
Crystallization, extraction and chromatography
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How can solubility behavior be described?
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Soluble, insoluble, g/L, mg/mL
Miscible (two liquids completely soluble in the other) Immiscible (do not mix and form two layers) |
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Like dissolves like
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Polar dissolves polar (dipole-dipole interaction)
Ion dissolves ion (ion-ion, ion-dipole) Nonpolar dissolves nonpolar (london/dispersion forces) |
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Stronger the intermolecular forces
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The higher melting/boiling points
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Greater the surface area (less branch),
The heavier, |
Greater the boiling point
Hexane > Pentane |
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Order them from weakest to strongest force
H-bond (NH or OH), ion-ioin, London/dispersion, ion-dipole, dipole-dipole |
London/dispersion, dipole-dipole, H-bond, ion-dipole, ion-ion
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Would benzoic acid dissolve in water? NaOH?
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No in water, although benzoic acid has a polar hydroxyl group, majority of the compound is nonpolar (aromatic ring = very nonpolar)
Yes in NaOH, due to acid - base interaction |
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Would methanol dissolve in polar compounds? nonpolar compounds?
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Yes in polar compounds due to OH, hydroxyl group.
Sometimes yes in nonpolar compounds because methanol also has a nonpolar CH3 part. |
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Benzoic acid soluble in water? in NaOH? in HCl?
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Not soluble in water because it has a very nonpolar phenol group (HOWEVER it becomes water soluble after addition of OH-)
Yes, soluble in NaOH No, not soluble in HCl |
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Ethyl-4-aminobenzoate soluble in water? in NaOH? in HCl?
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Not soluble in water because it has a very nonpolar phenol group (HOWEVER it becomes water soluble after addition of H+)
No, not soluble in NaOH Yes, soluble in HCl |
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