Calculate the [H+] in a solution that is 0.16 M in NaF and 0.25 M in HF. HF + H₂O = F¯ + H3O+ K₂ for HF = 7.2 x 10-4 [H+] = [?] x 10¹ M Coefficient (green) Exponent (yellow) Enter
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![**Calculate the [H+] in a solution that is 0.16 M in NaF and 0.25 M in HF**
**Chemical Equation:**
\[ \text{HF} + \text{H}_2\text{O} \rightleftharpoons \text{F}^- + \text{H}_3\text{O}^+ \]
**Given Data:**
\[ K_a \text{ for HF} = 7.2 \times 10^{-4} \]
**Expression to Calculate [H+]:**
\[ \left[\text{H}^+\right] = \boxed{\text{Coefficient}} \times 10^{\boxed{\text{Exponent}}} \text{ M} \]
**Input Fields:**
- Coefficient (in green box)
- Exponent (in yellow box)
**Submit Button:**
- "Enter"
This webpage prompts users to calculate the hydrogen ion concentration \([H^+]\) in a buffer solution containing NaF and HF. The provided chemical equilibrium for the dissociation of HF in water, along with the \( K_a \) value for HF, indicates that users need to apply the Henderson-Hasselbalch equation or an equivalent method to determine [H+].
**Instructions:**
1. Use the given data to perform the necessary calculations.
2. Fill in the coefficient (green box) and the exponent (yellow box) in the equation \([H^+] = \text{Coefficient} \times 10^{\text{Exponent}}\) M.
3. Click "Enter" to submit your solution.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6e6a7604-eb1c-41a1-a623-753603ba28f3%2F698b6c15-590f-4883-aed9-ee775df05b1e%2F3sno9v6_processed.jpeg&w=3840&q=75)
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