Chapter 16, Problem 16.32QP

(a)

Interpretation Introduction

Interpretation: Which of the given statements are true regarding a 1.0-M solution of a strong acid $\text{HA}$ at ${25}^{\circ }\text{C}$ has to be explained

Concept Information:

Strong acids

In strong acids, the ionization of acid is complete. This implies that the concentration of the hydrogen ion or hydronium ion will be equal to the initial concentration of the acid at equilibrium.

For example:

Consider ionization of $\text{HCl}$ (a strong acid)

0.10-M $\text{HCl}$ solution contains 0.10 M hydronium ions ${\text{[H}}_{\text{3}}{\text{O}}^{\text{+}}\text{]}$  in it, because all the $\text{HCl}$ molecules ionizes.

At equilibrium (after the completion of ionization), the concentration of $\text{[HCl]}$  will be zero since no $\text{HCl}$ molecules remains after ionization.

The concentration after ionization will be as follows,

$\text{[HCl]}$= 0M

${\text{[H}}_{\text{3}}{\text{O}}^{\text{+}}\text{]}$ = 0.10 M

${\text{[Cl}}^{\text{-}}\text{]}$=0.1 M

At ${25}^{\circ }\text{C}$, the $\text{pH}$ of the solution will be,

$\begin{array}{l}\text{pH}=-\log (0.10)\\ =1.00\end{array}$

which is a  very small $\text{pH}$

Therefore, strong acids have low $\text{pH}$ value whereas weak acids have high $\text{pH}$ value

To Explain: Which of the given statements are true regarding a 1.0-M solution of a strong acid $\text{HA}$ at 25°C

The given statement ${\text{[A}}^{\text{-}}\text{]}\text{>}{\text{[H}}^{\text{+}}\text{]}$  is true or false

(b)

Interpretation Introduction

Interpretation: Which of the given statements are true regarding a 1.0-M solution of a strong acid $\text{HA}$ at ${25}^{\circ }\text{C}$ has to be explained

Concept Information:

Strong acids

In strong acids, the ionization of acid is complete. This implies that the concentration of the hydrogen ion or hydronium ion will be equal to the initial concentration of the acid at equilibrium.

For example:

Consider ionization of $\text{HCl}$ (a strong acid)

0.10-M $\text{HCl}$ solution contains 0.10 M hydronium ions ${\text{[H}}_{\text{3}}{\text{O}}^{\text{+}}\text{]}$  in it, because all the $\text{HCl}$ molecules ionizes.

At equilibrium (after the completion of ionization), the concentration of $\text{[HCl]}$  will be zero since no $\text{HCl}$ molecules remains after ionization.

The concentration after ionization will be as follows,

$\text{[HCl]}$= 0M

${\text{[H}}_{\text{3}}{\text{O}}^{\text{+}}\text{]}$ = 0.10 M

${\text{[Cl}}^{\text{-}}\text{]}$=0.1 M

At ${25}^{\circ }\text{C}$, the $\text{pH}$ of the solution will be,

$\begin{array}{l}\text{pH}=-\log (0.10)\\ =1.00\end{array}$

which is a  very small $\text{pH}$

Therefore, strong acids have low $\text{pH}$ value whereas weak acids have high $\text{pH}$ value

To Explain: Which of the given statements are true regarding a 1.0-M solution of a strong acid $\text{HA}$ at 25°C

The given statement $\text{pH}\text{=}\text{0}\text{.00}$ is true or false

(c)

Interpretation Introduction

Interpretation: Which of the given statements are true regarding a 1.0-M solution of a strong acid $\text{HA}$ at ${25}^{\circ }\text{C}$ has to be explained

Concept Information:

Strong acids

In strong acids, the ionization of acid is complete. This implies that the concentration of the hydrogen ion or hydronium ion will be equal to the initial concentration of the acid at equilibrium.

For example:

Consider ionization of $\text{HCl}$ (a strong acid)

0.10-M $\text{HCl}$ solution contains 0.10 M hydronium ions ${\text{[H}}_{\text{3}}{\text{O}}^{\text{+}}\text{]}$  in it, because all the $\text{HCl}$ molecules ionizes.

At equilibrium (after the completion of ionization), the concentration of $\text{[HCl]}$  will be zero since no $\text{HCl}$ molecules remains after ionization.

The concentration after ionization will be as follows,

$\text{[HCl]}$= 0M

${\text{[H}}_{\text{3}}{\text{O}}^{\text{+}}\text{]}$ = 0.10 M

${\text{[Cl}}^{\text{-}}\text{]}$=0.1 M

At ${25}^{\circ }\text{C}$, the $\text{pH}$ of the solution will be,

$\begin{array}{l}\text{pH}=-\log (0.10)\\ =1.00\end{array}$

which is a  very small $\text{pH}$

Therefore, strong acids have low $\text{pH}$ value whereas weak acids have high $\text{pH}$ value

To Explain: Which of the given statements are true regarding a 1.0-M solution of a strong acid $\text{HA}$ at 25°C

(d)

Interpretation Introduction

Interpretation: Which of the given statements are true regarding a 1.0-M solution of a strong acid $\text{HA}$ at ${25}^{\circ }\text{C}$ has to be explained

Concept Information:

Strong acids

In strong acids, the ionization of acid is complete. This implies that the concentration of the hydrogen ion or hydronium ion will be equal to the initial concentration of the acid at equilibrium.

For example:

Consider ionization of $\text{HCl}$ (a strong acid)

0.10-M $\text{HCl}$ solution contains 0.10 M hydronium ions ${\text{[H}}_{\text{3}}{\text{O}}^{\text{+}}\text{]}$  in it, because all the $\text{HCl}$ molecules ionizes.

At equilibrium (after the completion of ionization), the concentration of $\text{[HCl]}$  will be zero since no $\text{HCl}$ molecules remains after ionization.

The concentration after ionization will be as follows,

$\text{[HCl]}$= 0M

${\text{[H}}_{\text{3}}{\text{O}}^{\text{+}}\text{]}$ = 0.10 M

${\text{[Cl}}^{\text{-}}\text{]}$=0.1 M

At ${25}^{\circ }\text{C}$, the $\text{pH}$ of the solution will be,

$\begin{array}{l}\text{pH}=-\log (0.10)\\ =1.00\end{array}$

which is a  very small $\text{pH}$

Therefore, strong acids have low $\text{pH}$ value whereas weak acids have high $\text{pH}$ value

To Explain: Which of the given statements are true regarding a 1.0-M solution of a strong acid $\text{HA}$ at 25°C

The given statement $\text{[HA]}\text{=}\text{0}\text{.1}\text{M}$  is true or false