Chapter MPS, Problem 8.4MPS

a.

To determine

To find the concentration of the hydrogen ion

Answer to Problem 8.4MPS

  $-1995.26$

Explanation of Solution

Given:

The equation which determines the pH is as follows.

  $pH=-{\log }_{10}[H^{+}]$ .

Calculation:

The pH of an aqueous solution is $3.30$ .

The concentration of the hydrogen ion is calculated below.

  $\begin{array}{l}pH=-{\log }_{10}[H^{+}]\\ 3.30=-{\log }_{10}[H^{+}]\\ {10}^{3.30}=-[H^{+}]\\ [H^{+}]=-1995.26\end{array}$

Therefore, the concentration of the hydrogen ion is $-1995.26$ .

b.

To determine

To find the concentration of the hydrogen ion.

Answer to Problem 8.4MPS

  $-1.66\times {10}^{13}$

Explanation of Solution

Given:

The equation which determines the pH is as follows.

  $pH=-{\log }_{10}[H^{+}]$ .

Calculation:

The pH of an aqueous solution is $13.22$ .

The concentration of the hydrogen ion is calculated below.

  $\begin{array}{l}pH=-{\log }_{10}[H^{+}]\\ 13.22=-{\log }_{10}[H^{+}]\\ {10}^{13.22}=-[H^{+}]\\ [H^{+}]=-1.66\times {10}^{13}\end{array}$

Therefore, the concentration of the hydrogen ion is $-1.66\times {10}^{13}$ .

c.

To determine

To find the concentration of the hydrogen ion

Answer to Problem 8.4MPS

  $-{10}^7$

Explanation of Solution

Given:

The equation which determines the pH is as follows.

  $pH=-{\log }_{10}[H^{+}]$ .

Calculation:

The pH of an aqueous solution is $7$ .

The concentration of the hydrogen ion is calculated below.

  $\begin{array}{l}pH=-{\log }_{10}[H^{+}]\\ 7=-{\log }_{10}[H^{+}]\\ {10}^7=-[H^{+}]\\ [H^{+}]=-{10}^7\end{array}$

Therefore, the concentration of the hydrogen ion is $-{10}^7$ .

d.

To determine

To find the concentration of the hydrogen ion

Answer to Problem 8.4MPS

  $-3981$

Explanation of Solution

Given:

The equation which determines the pH is as follows.

  $pH=-{\log }_{10}[H^{+}]$ .

Calculation:

The pH of an aqueous solution is $3.6$ .

The concentration of the hydrogen ion is calculated below.

  $\begin{array}{l}pH=-{\log }_{10}[H^{+}]\\ 3.6=-{\log }_{10}[H^{+}]\\ {10}^{3.6}=-[H^{+}]\\ [H^{+}]=-3981\end{array}$

Therefore, the concentration of the hydrogen ion is $-3981$ .

e.

To determine

To find the pH level.

Answer to Problem 8.4MPS

  $2.568$

Explanation of Solution

Given:

The equation which determines the pH is as follows.

  $pH=-{\log }_{10}[H^{+}]$ .

Calculation:

The concentration of the hydrogen ion is $2.7\times {10}^3$ .

The concentration of the hydrogen ion is calculated below.

  $\begin{array}{l}pH=-{\log }_{10}[H^{+}]\\ pH=-{\log }_{10}[2.7\times {10}^3{}^{+}]\\ pH=-[-2.568]\\ pH=2.568\end{array}$

Therefore, the pH level is $2.568$ .

f.

To determine

To find the concentration of the hydrogen ion.

Answer to Problem 8.4MPS

  $-3.3\times {10}^6$

Explanation of Solution

Given:

The equation which determines the pH is as follows.

  $pH=-{\log }_{10}[H^{+}]$ .

Calculation:

The pH of an aqueous solution is $6.52$ .

The concentration of the hydrogen ion is calculated below.

  $\begin{array}{l}pH=-{\log }_{10}[H^{+}]\\ 6.52=-{\log }_{10}[H^{+}]\\ {10}^{6.52}=-[H^{+}]\\ [H^{+}]=-3.3\times {10}^6\end{array}$

Therefore, the concentration of the hydrogen ion is $-3.3\times {10}^6$ .