The pH of a 1.3M solution of boric acid (H₂BO3) is measured to be 4.56. Calculate the acid dissociation constant K of boric acid. Round your answer to 2 significant digits. K = 0 X 3
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![**Title: Calculating the Acid Dissociation Constant of Boric Acid**
**Text:**
The pH of a 1.3 M solution of boric acid (H₃BO₃) is measured to be 4.56.
Calculate the acid dissociation constant \(K_a\) of boric acid. Round your answer to two significant digits.
**Response Fields:**
- \(K_a =\) [Input box for user to enter the \(K_a\) value]
**Exponential Notation:**
- An additional input box provided for exponential notation, with placeholders for base and exponent, indicating \( \times 10^{[exponent]}\).
**Interactive Options:**
- **Explanation** Button: Provides more information or guidance on how to perform the calculation.
- **Check** Button: Allows the user to submit their answer and verify its correctness.
**Note on Calculation:**
To find \(K_a\), you'd typically use the formula involving the concentration of hydrogen ions derived from the pH measurement and the initial concentration of the acid.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fcef3f1b2-56cd-4f45-949e-fc7a38ef994c%2F51198372-8f2d-44b3-bc4c-deb8edc826ca%2F729qo8_processed.jpeg&w=3840&q=75)
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