Calculate the pH of a solution that is prepared by dissolving 0.174 mol of m-chlorobenzoic acid (C6H4CICOOH, K, 1.00x104) and 0.430 mol of hydrocyanic acid (HCN, K, 6.17x10-10) in water and diluting to 2.40 L. Also, calculate the equilibrium concentrations of CeHaCICOOH, C6H4CICOO, HCN, and CN". Do not make an approximation unless the initial acid concentration is greater than 1000 x Ka. (Hint: The pH will be determined by the stronger acid of this pair.) pH = [C6H4CICOOH) = [CH₂CICOO"]= [HCN] = [CN"]= M M M M
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![**Problem Statement: Acid-Base Equilibrium and pH Calculation**
Calculate the pH of a solution prepared by dissolving 0.174 mol of *m*-chlorobenzoic acid (C₆H₄ClCOOH, Kₐ = 1.00×10⁻⁴) and 0.430 mol of hydrocyanic acid (HCN, Kₐ = 6.17×10⁻¹⁰) in water and diluting to 2.40 L. Also, calculate the equilibrium concentrations of C₆H₄ClCOOH, C₆H₄ClCOO⁻, HCN, and CN⁻. Do not make an approximation unless the initial acid concentration is greater than 1000 × Kₐ. (Hint: The pH will be determined by the stronger acid of this pair.)
**Calculations Required:**
- **pH**: [ ]
- **Equilibrium Concentrations**:
- [C₆H₄ClCOOH] = [ ] M
- [C₆H₄ClCOO⁻] = [ ] M
- [HCN] = [ ] M
- [CN⁻] = [ ] M](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0e109430-7b34-4d38-8cab-38f4ccc5aed5%2F08c7985f-a4f3-40f3-b947-df014bfe4e47%2F4xzji8_processed.jpeg&w=3840&q=75)
Given:
Moles of C6H4ClCOOH = 0.174 mol
Ka of C6H4ClCOOH = 1.00×10-4
Moles of HCN = 0.430 mol
Ka of HCN = 6.17 × 10-10
Volume = 3.00 L
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