Subjects
| Sections | |||
|---|---|---|---|
| Solutions, Molarity and Intermolecular Forces | 7 mins | 0 completed | Learn |
| Henry's Law | 20 mins | 0 completed | Learn Summary |
| Calculate Molarity | 27 mins | 0 completed | Learn Summary |
| Mass Percent | 10 mins | 0 completed | Learn |
| Molality | 15 mins | 0 completed | Learn |
| Mole Fraction | 14 mins | 0 completed | Learn |
| The Colligative Properties | 45 mins | 0 completed | Learn |
| Additional Practice |
|---|
| Making Solutions |
| Freezing Point Depression |
| Colloid |
| Additional Guides |
|---|
| ppm |
| The Freezing Point Depression |
| Boiling Point Elevation |
Calculate the pressure of O2 necessary to generate an aqueous solution that is 6.0 x 10‐2 M in O 2 at 25° C. The Henry’s law constant for O 2 in water at 25°C is 1.3 x 10 ‐3 mole/L•atm
A) 7.8 x 10‐5 atm
B) 2.1 x 10‐2 atm
C) 46 atm
D) 1.28 x 104 atm
E) none of these
We’re being asked to determine the partial pressure of O2 at 25 ˚C to produce a solution of 6.0 × 10–2 M. Recall that the solubility of a gas is given by Henry’s law:
where Sgas = solubility of the gas (in mol/L or M), kH = Henry’s law constant for the gas, Pgas = partial pressure of the gas.
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