Be sure to answer all parts. Calculate the K, of a weak acid if a 0.057 M solution of the acid has a pH of 3.47 at 25°C. x 10 K¸ = (Enter your answer in scientific notation.)
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### Acid Dissociation Constant Calculation
**Be sure to answer all parts.**
Calculate the \( K_a \) of a weak acid if a \( 0.057 M \) solution of the acid has a pH of 3.47 at 25°C.
\[ K_a = [\ \ \_ \ \ \ ] \times 10^{[\ \ \_ \ \ \ ]} \]
*(Enter your answer in scientific notation.)*
**Instructions:**
- Use the given concentration and pH values to determine the \( K_a \) of the weak acid.
- Apply the principles of equilibrium and acid dissociation constants.
- Express your final answer in scientific notation.
**Note:**
- \( K_a \) represents the acid dissociation constant, a quantitative measure of the strength of an acid in solution.
- Use the formula relating pH and hydrogen ion concentration: \( \text{pH} = -\log[H^+] \).
- For a weak acid, \( HA \leftrightarrow H^+ + A^- \), where \( K_a = \frac{[H^+][A^-]}{[HA]} \).
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