University:
Williams College
Course:
CHEM 201 | Organic Chemistry: Introductory Level
Academic year:

2024
Views:

97

Pages:

2
Author:

esplondafni9

3. Acrylic acid (HC₃H₃O₂): Kₐ = [H₃O⁺][C₃H₃O₂⁻] / [HC₃H₃O₂] = 5.8x10⁻⁵ [H₃O⁺] = 2.4x10⁻³ pH = -log[H₃O⁺] = 2.63 4. Percent ionization: % ionization = [H₃O⁺]/[HA] x 100% = 2.4% 5. Boric acid (H₃BO₃): Kₐ = [H₃O⁺][H₂BO₃⁻] / [H₃BO₃] = 5.9x10⁻¹⁰ [H₃O⁺] = 3.8x10⁻⁶ pH = -log[H₃O⁺] = 5.42 6. Salt solutions: Fe(NO₃)₃: Fe(OH)₃ + HNO₃ (acidic) Na₂CO₃: NaOH + H₂CO₃ (basic) CaCN₂: Ca(OH)₂ + HCN (basic) 5. Draw a pH titration curve that represents the titration of NH₃ by the addition of HCl from a buret below. 6. Indicate the equivalence point on the curve. 7. Is the solution acidic, basic, or neutral? Explain. WB + SA = acidic The cation of the salt is the conjugate of the weak base which hydrolyzes to produce an acidic solution.