Question: (A) Use data from Example 14-5 to determine the partial pressure of O 2 above an aqueous solution at 0 C known to contain 5.00
(A) Use data from Example 14-5 to determine the partial pressure of O2 above an aqueous solution at 0 °C known to contain 5.00 mg O2 per 100.0 mL of solution.
(B) A handbook lists the solubility of carbon monoxide in water at 0 °C and 1 atm pressure as 0.0354 mL CO per milliliter of H2O. What pressure of CO(g) must be maintained above the solution to obtain 0.0100 M CO?
Example 14-5
At 0 °C and an O2 pressure of 1.00 atm, the aqueous solubility of O2(g) is 48.9 mL O2 per liter. What is the molarity of O2 in a saturated water solution when the O2 is under its normal partial pressure in air, 0.2095 atm?
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A mol O2 mass O2 molar mass O2 where mol O2 is the moles of O2 mass O2 is the mass of O2 in mg molar mass O2 is the molar mass of O2 in gmol Plugging ... View full answer
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