The pH of a 1.2 M solution of hypobromous acid (HBrO) is measured to be 4.28. Calculate the acid dissociation constant K, of hypobromous acid. Be sure your answer has the correct number of significant digits.
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![**Educational Content: Calculating the Acid Dissociation Constant**
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**Problem Statement:**
The pH of a \(1.2 \, \text{M}\) solution of hypobromous acid (\(\text{HBrO}\)) is measured to be 4.28. Calculate the acid dissociation constant \(K_a\) of hypobromous acid. Be sure your answer has the correct number of significant digits.
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**Visual Components:**
1. **Equation Field:**
- Placeholder for \(K_a =\) with an empty box where the calculated value of the acid dissociation constant should be entered.
2. **Input Options:**
- A small box labeled \( \times 10 \) to input the power of ten.
- Buttons for confirming (\(\checkmark\)), resetting (\(\hookleftarrow\)), and seeking help (\(?\)).
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**Instructions:**
To solve this problem, you need to:
1. **Understand pH and \(K_a\):**
- Use the formula to convert pH to \([H^+]\):
\[
[H^+] = 10^{-\text{pH}}
\]
- Establish the relationship between \(K_a\) and the concentrations of the products and reactants.
2. **Perform the Calculation:**
- Given pH, calculate \([H^+]\).
- Use an ICE table to determine the concentrations at equilibrium.
- Solve for \(K_a\) using the equilibrium concentrations.
3. **Significant Figures:**
- Ensure the final answer reflects the correct number of significant figures based on the given data.
This information will guide you through understanding and calculating the acid dissociation constant for hypobromous acid with precision and accuracy.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa21199a8-7a5a-4751-9685-1126762a8cde%2Fd3a52004-2f45-4ec1-806d-d96344edb963%2F090hmtp_processed.png&w=3840&q=75)
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