Test: Solubility (NCERT) - NEET MCQ

At dynamic equilibrium, number of solute particles going into the solution will be equal to solute particles separating out. Hence, the concentration of solute in the solution remains constant.

The solubility of gas in a liquid increases with increase in pressure and is directly proportional to the pressure of the gas.

Henry's law states that the solubility of a gas in a liquid is directly proportional to the partial pressure of the gas present above the surface of the liquid or solution.
p = K_HX

p = K_Hx. Higher the value of K_H at a given pressure, lower is the solubility of the gas in the liquid.

Higher the value of K_H, lower is the solubility of gas in the liquid.

No. of moles of H₂S = 0.195
No. of moles of H₂O = 1000/18 = 55.55mol
Mole fraction of H₂S =
Pressure at STP = 0.987 bar
According to Henry’s law, p = K_H^x
or K_H = pH₂S/xH₂S = 0.98/70.0035
= 282 bar

According to Henry's law, p = K_Hx
x = p/K_H
= 1.78 x 10^-3

p = K_H × x

Mole fraction = Moles of gas/Total moles
Moles of H₂O = 1000/18 = 55.55 (∵ 1L = 1000 g)
Mole fraction = (55.55 >>> x)

According to Henry’s law, s = K_H × p, where s is concentration of O₂ dissolved.
s = 1.4 × 10⁻³ × 0.5 = 0.7 × 10⁻³mol/L
s = n/V or n = 0.7×10⁻³ × 0.1 = 0.7 × 10⁻⁴mol
n = w/M or w = n × M
= 0.7 × 10⁻⁴ × 32 = 22.4 × 10⁻⁴g or 2.24mg

At high altitudes the partial pressure of oxygen is less than that at the ground level. This leads to low concentrations of oxygen in the blood and tissues of people living at high altitudes or climbers.