Chapter 13, Problem 13.161P

(a)

Interpretation Introduction

Interpretation:

The $k_{\text{H}}$ in $\text{mol/L}\cdot \text{atm}$ is to be calculated.

Concept introduction:

Henry’s law gives the quantitative relationship between the pressure of the gas and its solubility. It states that the amount of gas dissolved in a liquid is proportional to the partial pressure of the gas. Higher the partial pressure of the gas, more will be its solubility and vice-versa.

The formula to calculate the solubility of gases according to Henry’s law is as follows:

  $S_{\text{gas}}=k_{\text{H}}\times P_{\text{gas}}$        (1)

Here,

$S_{\text{gas}}$ is the solubility of the gas.

$k_{\text{H}}$ is Henry’s constant.

$P_{\text{gas}}$ is the partial pressure of the gas.

The formula to calculate the density of the substance is as follows:

  $\text{Density of substance}\left(\rho \right)=\frac{\text{Mass of substance}\left(M\right)}{\text{Volume of substance}\left(V\right)}$        (2)

(b)

Interpretation Introduction

Interpretation:

The solubility of ${\text{O}}_2$ in water at $25°\text{C}$ is to be calculated in $\text{ppm}$.

Concept introduction:

Henry’s law gives the quantitative relationship between the pressure of the gas and its solubility. It states that the amount of gas dissolved in a liquid is proportional to the partial pressure of the gas. Higher the partial pressure of the gas, more will be its solubility and vice-versa.

The formula to calculate the solubility of gases according to Henry’s law is as follows:

  $S_{\text{gas}}=k_{\text{H}}\times P_{\text{gas}}$        (1)

Here,

$S_{\text{gas}}$ is the solubility of the gas.

$k_{\text{H}}$ is Henry’s constant.

$P_{\text{gas}}$ is the partial pressure of the gas.

The $\text{ppm}$ or parts per million is a concentration term that is defined as the mass of any substance divided by the mass of the solution, multiplied by ${10}^6$.

The formula to calculate the concentration of an ion in $\text{ppm}$ is as follows:

  $\text{ppm}=\left(\frac{\text{mass}\text{of solute}}{\text{mass}\text{of}\text{solution}}\right){10}^6$        (8)

(c)

Interpretation Introduction

Interpretation:

The decreasing order of $k_{\text{H}}$ for ${\text{O}}_2$ in water, ethanol, ${\text{C}}_6{\text{F}}_{14}$ and ${\text{C}}_6{\text{H}}_{14}$ is to be determined. Also, its explanation is to be given.

Concept introduction:

Henry’s law gives the quantitative relationship between the pressure of the gas and its solubility. It states that the amount of gas dissolved in a liquid is proportional to the partial pressure of the gas. Higher the partial pressure of the gas, more will be its solubility and vice-versa.

The formula to calculate the solubility of gases according to Henry’s law is as follows:

  $S_{\text{gas}}=k_{\text{H}}\times P_{\text{gas}}$        (1)

Here,

$S_{\text{gas}}$ is the solubility of the gas.

$k_{\text{H}}$ is Henry’s constant.

$P_{\text{gas}}$ is the partial pressure of the gas.