Calculate the solubility (in m units) of ammonia gas in water at 298 k and a partial pressure of 2.50 bar. the henry's law constant for ammonia gas at 298 k is 58.0 m/atm and 1 bar=0.9869 atm.

Henry's Law (formulated in 1803 by William Henry) states that aa constant temperature, the amount of gas dissolved in a liquid is directly proportional to the partial pressure exerted by that gas on the liquid.

Mathematically it can be formulated as

C = H⨯P

being:

C: the molar concentration of dissolved gas A,

P: the partial pressure of it

H: Henry's constant

Substituting:

C = P * H

C = (2.50 * 0.9869) * 58.0

C = 143.1

Answer:

the solubility (in m units) is

C = 143.1