Question

At 25 °C and 765 Torr, carbon dioxide has a solubility of 0.0342 M in water. What is its solubility at 25 °C and 1730 Torr?

Answer 1

Answer is: solubility of a carbon dioxide is 0,077 M.
The solubility of a carbon dioxide is directly proportional to the pressure:
p₁ = 765 torr.
p₂ = 1730 torr.
solubility₁ = 0,0342 M.
solubility₂ = ?
p₁/p₂ = solubility₁/solubility₂.
solubility₂ = p₂ · solubility₁ ÷ p₁.
solubility₂ = 1730 torr · 0,0342 M ÷ 765 torr.
solubility₂ = 0,077 M.

Answer 2

The solubility of carbon dioxide at 1730 Torr is 0.07734 M

According to Henry's Law, it posits that the solubility of a gas in a solvent varies directly proportional to the gas pressure at solution equilibrium provided the temperature remains constant:

i.e.

Concentration (C) ∝ P (pressure)

$\mathbf{\dfrac{C}{P}= k(constant)}$

From the given information:

C₁ = 0.0342M

P₁ = 765 Torr

C₂ = ???

P₂ = 1730 Torr

∴

We can say that:

$\mathbf{\dfrac{C_1}{P_1}= \dfrac{C_2}{P_2}}$

$\mathbf{ C_2 = \dfrac{C_1 \times P_2}{P_1}}$

$\mathbf{ C_2 = \dfrac{0.0342 \ M \times 1730 \ torr}{765 \ torr}}$

$\mathbf{ C_2 = 0.07734 \ M}$

Therefore, we can con conclude that the solubility of carbon dioxide at 1730 Torr is 0.07734 M

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