The pH of a chemical solution is given by the formula , where is the concentration of
hydrogen ions in moles per liter. Values of pH range from 0 (acidic) to 14 (alkaline). Answer parts (a) through (f).
(a) What is the pH of a solution for which is 0.1 ?
(Type an integer or a decimal.)
(b) What is the pH of a solution for which is 0.01 ?
(Type an integer or a decimal.)
© What is the pH of a solution for which is 0.001 ?
(Type an integer or a decimal.)
(d) What happens to pH as the hydrogen ion concentration decreases?
pH decreases
(e) Determine the hydrogen ion concentration of a solution with
[ (Round to six decimal places as needed.)

Ask by Hampton Parry. in the United States

Mar 26,2025

Question

The pH of a chemical solution is given by the formula , where is the concentration of
hydrogen ions in moles per liter. Values of pH range from 0 (acidic) to 14 (alkaline). Answer parts (a) through (f).
(a) What is the pH of a solution for which is 0.1 ?
(Type an integer or a decimal.)
(b) What is the pH of a solution for which is 0.01 ?
(Type an integer or a decimal.)
© What is the pH of a solution for which is 0.001 ?
(Type an integer or a decimal.)
(d) What happens to pH as the hydrogen ion concentration decreases?
pH decreases
(e) Determine the hydrogen ion concentration of a solution with
[ (Round to six decimal places as needed.)

Ask by Hampton Parry. in the United States

Mar 26,2025

UpStudy AI · Accepted Answer

**(a)**  
We have  
$$
\mathrm{pH} = -\log_{10}(0.1)
$$  
Since $$ 10^{-1} = 0.1 $$, it follows that  
$$
\mathrm{pH} = 1.
$$

**(b)**  
We have  
$$
\mathrm{pH} = -\log_{10}(0.01)
$$  
Since $$ 10^{-2} = 0.01 $$, it follows that  
$$
\mathrm{pH} = 2.
$$

**(c)**  
We have  
$$
\mathrm{pH} = -\log_{10}(0.001)
$$  
Since $$ 10^{-3} = 0.001 $$, it follows that  
$$
\mathrm{pH} = 3.
$$

**(d)**  
The formula  
$$
\mathrm{pH} = -\log_{10} \left[\mathrm{H}^{+}\right]
$$  
shows that as the hydrogen ion concentration $$\left[\mathrm{H}^{+}\right]$$ decreases, the value of $$-\log_{10} \left[\mathrm{H}^{+}\right]$$ increases. Thus, the pH increases.

**(e)**  
We are given that  
$$
\mathrm{pH} = 3.5.
$$  
Using the formula, we write  
$$
3.5 = -\log_{10}\left[\mathrm{H}^{+}\right].
$$  
Rearrange to obtain  
$$
\log_{10}\left[\mathrm{H}^{+}\right] = -3.5.
$$  
Exponentiating both sides with base 10 gives  
$$
\left[\mathrm{H}^{+}\right] = 10^{-3.5}.
$$  
Calculating $$10^{-3.5}$$:  
$$
10^{-3.5} = 10^{-3} \times 10^{-0.5} = 0.001 \times 0.31622777 \approx 0.00031623.
$$  
Rounded to six decimal places,  
$$
\left[\mathrm{H}^{+}\right] \approx 0.000316\,\text{M}.
$$
**(a)** $$ \mathrm{pH} = 1 $$ **(b)** $$ \mathrm{pH} = 2 $$ **(c)** $$ \mathrm{pH} = 3 $$ **(d)** As hydrogen ion concentration decreases, pH increases. **(e)** $$ \left[\mathrm{H}^{+}\right] \approx 0.000316\,\text{M} $$

Upstudy AI Solution

Answer

Solution

Extra Insights

Related Questions

Latest Chemistry Questions