Multiple Choice
Determine the Henry's law constant for ammonia in water at 25°C if an ammonia pressure of 0.022 atm produces a solution with a concentration of 1.3 M.
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14. Solutions
Henry's Law Calculations
Multiple Choice
What is the millimolar solubility of oxygen gas, O2, in water at 16 °C, if the pressure of oxygen is 1.00 atm? Express the millimolar concentration numerically to two significant figures.
A
0.43 mM
B
0.65 mM
C
0.10 mM
D
0.21 mM
Verified step by step guidance1
Identify that the problem involves calculating the solubility of a gas in a liquid, which can be determined using Henry's Law.
Recall Henry's Law, which states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas above the liquid. The formula is: , where is the concentration of the gas, is Henry's Law constant, and is the partial pressure of the gas.
Determine the value of Henry's Law constant, , for oxygen in water at 16 °C. This value is typically found in tables or literature and is necessary for the calculation.
Substitute the given pressure of oxygen, 1.00 atm, and the Henry's Law constant into the formula to calculate the concentration of oxygen in molarity (M).
Convert the molarity to millimolarity (mM) by multiplying the result by 1000, as 1 M = 1000 mM. This will give you the millimolar solubility of oxygen in water at the specified conditions.
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