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 ?
pH (Type an integer or a decimal.)
© What is the pH of a solution for which is 0.001 ?
pH (Type an integer or a decimal.)
(d) What happens to pH as the hydrogen ion concentration decreases?
pH decreases
pH increases

Ask by Dawson Chambers. 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 ?
pH (Type an integer or a decimal.)
© What is the pH of a solution for which is 0.001 ?
pH (Type an integer or a decimal.)
(d) What happens to pH as the hydrogen ion concentration decreases?
pH decreases
pH increases

Ask by Dawson Chambers. in the United States

Mar 26,2025

UpStudy AI · Accepted Answer

Let's solve each part step by step using the formula $$ \mathrm{pH} = -\log_{10}\left[\mathrm{H}^{+}\right] $$.

### Part (a)
For $$ \left[\mathrm{H}^{+}\right] = 0.1 $$:
$$
\mathrm{pH} = -\log_{10}(0.1)
$$

### Part (b)
For $$ \left[\mathrm{H}^{+}\right] = 0.01 $$:
$$
\mathrm{pH} = -\log_{10}(0.01)
$$

### Part (c)
For $$ \left[\mathrm{H}^{+}\right] = 0.001 $$:
$$
\mathrm{pH} = -\log_{10}(0.001)
$$

### Part (d)
As the hydrogen ion concentration decreases, the pH increases. This is because pH is inversely related to the concentration of hydrogen ions.

Now, let's calculate the pH values for parts (a), (b), and (c).
Calculate the value by following steps:
- step0: Calculate:
  $$-\log_{10}{\left(0.001\right)}$$
- step1: Calculate:
  $$-\left(-3\right)$$
- step2: Remove the parentheses:
  $$3$$
Calculate or simplify the expression $$ -\log_{10}(0.1) $$.
Calculate the value by following steps:
- step0: Calculate:
  $$-\log_{10}{\left(0.1\right)}$$
- step1: Calculate:
  $$-\left(-1\right)$$
- step2: Remove the parentheses:
  $$1$$
Calculate or simplify the expression $$ -\log_{10}(0.01) $$.
Calculate the value by following steps:
- step0: Calculate:
  $$-\log_{10}{\left(0.01\right)}$$
- step1: Calculate:
  $$-\left(-2\right)$$
- step2: Remove the parentheses:
  $$2$$
Here are the results for each part:

### Part (a)
For $$ \left[\mathrm{H}^{+}\right] = 0.1 $$:
$$
\mathrm{pH} = 1
$$

### Part (b)
For $$ \left[\mathrm{H}^{+}\right] = 0.01 $$:
$$
\mathrm{pH} = 2
$$

### Part (c)
For $$ \left[\mathrm{H}^{+}\right] = 0.001 $$:
$$
\mathrm{pH} = 3
$$

### Part (d)
As the hydrogen ion concentration decreases, the pH **increases**.

So, the answers are:
- (a) pH = 1
- (b) pH = 2
- (c) pH = 3
- (d) pH increases
- (a) pH = 1 - (b) pH = 2 - (c) pH = 3 - (d) pH increases

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