Chapter 13, Problem 46E

(a)

Interpretation Introduction

Interpretation: The $\left[{\text{H}}^{+}\right]$ of each of the given solutions is to be calculated. The solutions are to be identified as neutral, acidic or basic.

Concept introduction: A neutral species has a $\text{pH}$ value equal to $7$, that is the $\left[{\text{OH}}^{-}\right]$ is equal to the $\left[{\text{H}}^{+}\right]$. An acidic species has a $\text{pH}$ value less than $7$, that is the $\left[{\text{OH}}^{-}\right]$ is less than the $\left[{\text{H}}^{+}\right]$. A basic species has a $\text{pH}$ value greater than $7$, that is the $\left[{\text{H}}^{+}\right]$ is less than the $\left[{\text{OH}}^{-}\right]$.

The equilibrium constant for water is denoted by $K_{\text{w}}$ and is expressed as,

$K_{\text{w}}=\left[{\text{H}}^{+}\right]\left[{\text{OH}}^{-}\right]$

At $\text{25}\text{°C}$, $\left[{\text{H}}^{+}\right]\left[{\text{OH}}^{-}\right]=1\times {10}^{-14}$

(b)

Interpretation Introduction

Interpretation: The $\left[{\text{H}}^{+}\right]$ of each of the given solutions is to be calculated. The solutions are to be identified as neutral, acidic or basic.

Concept introduction: A neutral species has a $\text{pH}$ value equal to $7$, that is the $\left[{\text{OH}}^{-}\right]$ is equal to the $\left[{\text{H}}^{+}\right]$. An acidic species has a $\text{pH}$ value less than $7$, that is the $\left[{\text{OH}}^{-}\right]$ is less than the $\left[{\text{H}}^{+}\right]$. A basic species has a $\text{pH}$ value greater than $7$, that is the $\left[{\text{H}}^{+}\right]$ is less than the $\left[{\text{OH}}^{-}\right]$.

The equilibrium constant for water is denoted by $K_{\text{w}}$ and is expressed as,

$K_{\text{w}}=\left[{\text{H}}^{+}\right]\left[{\text{OH}}^{-}\right]$

At $\text{25}\text{°C}$, $\left[{\text{H}}^{+}\right]\left[{\text{OH}}^{-}\right]=1\times {10}^{-14}$

(c)

Interpretation Introduction

Interpretation: The $\left[{\text{H}}^{+}\right]$ of each of the given solutions is to be calculated. The solutions are to be identified as neutral, acidic or basic.

Concept introduction: A neutral species has a $\text{pH}$ value equal to $7$, that is the $\left[{\text{OH}}^{-}\right]$ is equal to the $\left[{\text{H}}^{+}\right]$. An acidic species has a $\text{pH}$ value less than $7$, that is the $\left[{\text{OH}}^{-}\right]$ is less than the $\left[{\text{H}}^{+}\right]$. A basic species has a $\text{pH}$ value greater than $7$, that is the $\left[{\text{H}}^{+}\right]$ is less than the $\left[{\text{OH}}^{-}\right]$.

The equilibrium constant for water is denoted by $K_{\text{w}}$ and is expressed as,

$K_{\text{w}}=\left[{\text{H}}^{+}\right]\left[{\text{OH}}^{-}\right]$

At $\text{25}\text{°C}$, $\left[{\text{H}}^{+}\right]\left[{\text{OH}}^{-}\right]=1\times {10}^{-14}$

(d)

Interpretation Introduction

Interpretation: The $\left[{\text{H}}^{+}\right]$ of each of the given solutions is to be calculated. The solutions are to be identified as neutral, acidic or basic.

Concept introduction: A neutral species has a $\text{pH}$ value equal to $7$, that is the $\left[{\text{OH}}^{-}\right]$ is equal to the $\left[{\text{H}}^{+}\right]$. An acidic species has a $\text{pH}$ value less than $7$, that is the $\left[{\text{OH}}^{-}\right]$ is less than the $\left[{\text{H}}^{+}\right]$. A basic species has a $\text{pH}$ value greater than $7$, that is the $\left[{\text{H}}^{+}\right]$ is less than the $\left[{\text{OH}}^{-}\right]$.

The equilibrium constant for water is denoted by $K_{\text{w}}$ and is expressed as,

$K_{\text{w}}=\left[{\text{H}}^{+}\right]\left[{\text{OH}}^{-}\right]$

At $\text{25}\text{°C}$, $\left[{\text{H}}^{+}\right]\left[{\text{OH}}^{-}\right]=1\times {10}^{-14}$