An acid (HA) dissociates as follows: HA → H* + A minus Arrow should be interpreted as an equilibrium arrow. The pH of the 0.10 M solution of HA is 4.02. What is [H*]? Express your answer as a decimal, not an exponent. Please include a proper (abbreviated) unit.
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![### Acid Dissociation and pH Calculation
**An acid (HA) dissociates as follows:**
\[ \text{HA} \rightleftharpoons \text{H}^+ + \text{A}^- \]
(Note: The arrow indicates equilibrium)
**Given Data:**
- The pH of the 0.10 M solution of HA is 4.02.
**Problem:**
**What is the concentration of hydrogen ions \([\text{H}^+]\)?**
**Instructions:**
- Express your answer as a decimal, not an exponent.
- Please include a proper (abbreviated) unit.
**Solution:**
The concentration of hydrogen ions, \([\text{H}^+]\), can be calculated using the pH value. The relationship between pH and \([\text{H}^+]\) is given by the formula:
\[ \text{pH} = -\log[\text{H}^+] \]
Rearranging the formula to solve for \([\text{H}^+]\):
\[ [\text{H}^+] = 10^{-\text{pH}} \]
Using the provided pH value:
\[ [\text{H}^+] = 10^{-4.02} \]
Calculating the value:
\[ [\text{H}^+] = 0.000095 \, \text{M} \]
So, the hydrogen ion concentration is:
\[ [\text{H}^+] = 0.000095 \, \text{M} \]
Or, as a decimal:
\[ [\text{H}^+] = 9.5 \times 10^{-5} \, \text{M} \]
**Note:** Ensure to double-check the calculations with proper significant figures based on context and instructional requirements.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8c8d8a42-8de4-4466-9c46-ae253053e314%2Fc8c1af5e-112a-48d1-8334-5b6ab94fe01d%2Fhsidi1m.png&w=3840&q=75)
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