# Problem: Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air.  Assume the mole fraction of oxygen in air to be 0.21 and the Henryʹs law constant for oxygen in water at this temperature to be 1.3 × 10 -3 M/atm. A) 23.5 mg      B) 27.3 mg      C) 49.4 mg      D) 13.7 mg      E) 47.0 mg

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Calculate the mass of oxygen (in mg) dissolved in a 5.00 L bucket of water exposed to a pressure of 1.13 atm of air.  Assume the mole fraction of oxygen in air to be 0.21 and the Henryʹs law constant for oxygen in water at this temperature to be 1.3 × 10 -3 M/atm.

A) 23.5 mg      B) 27.3 mg      C) 49.4 mg      D) 13.7 mg      E) 47.0 mg

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the Henry's Law concept. You can view video lessons to learn Henry's Law. Or if you need more Henry's Law practice, you can also practice Henry's Law practice problems.

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Based on our data, we think this problem is relevant for Professor Kieber Emmons' class at UTAH.