Question

The solubility of $N_2\left(g\right)$ in water exposed to the atmosphere, when its partial pressure is $593$ mm Hg is $5.3\times {10}^{-4}M$. Its solubility at $760$ and at the same temperature is:

• A. $4.1\times {10}^{-4}M$
• B. $6.8\times {10}^{-4}M$
• C. $1500M$
• D. $2400M$
  

Answer 1

The correct option is B $6.8\times {10}^{-4}M$

Solution:- $6.8\times {10}^{-4}M$

According to Henry's law-

$P=K_H\times C$

Here,

$P=$ Partial pressure of gas over solution

$C=$ concentration of the solute in the solution

$K_H=$ Henry's constant

For same gases-

$P\propto C$

Given that:-

$P_1=593\text{mm of Hg}$

$P_2=760\text{mm of Hg}$

$C_1=5.3\times {10}^{-4}M$

$C_2=?$

$\therefore \frac{P_1}{P_2}=\frac{c_1}{C_2}$

$\Rightarrow \frac{593}{760}=\frac{5.3\times {10}^{-4}}{C_2}$

$\Rightarrow C_2=\frac{5.3\times {10}^{-4}\times 760}{593}$

$\Rightarrow C_2=6.8\times {10}^{-4}M$