Multiple choice

At ${20}^{o}C$ and $1.00atm$ partial pressure of hydrogen, $10mL$ of hydrogen, measured at STP, dissolves in $1L$ of water. If water at ${20}^{o}C$ is exposed to a gaseous mixture having a total pressure of $1400$ Torr (excluding the vapour pressure of water) and containing $68.5$% ${H}{2}$ by volume, find the volume of ${H}{2}$, measured at STP, which will dissolve in $1L$ of water.

  1. $18mL$
  2. $12mL$
  3. $23mL$
  4. $121mL$
Reveal answer Fill a bubble to check yourself
B Correct answer
Explanation

Henry's Law: Solubility is proportional to partial pressure. Initial: 10 mL/L at 1 atm. New partial pressure of H2 = (68.5/100) * (1400/760) atm = 0.685 * 1.842 = 1.26 atm. New solubility = 10 * 1.26 = 12.6 mL/L. 12 mL is the closest option.

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