JEE Main Chemistry question
What is the pH of a 1 M CH₃COONa solution? Ka of acetic acid=1.8×10⁻⁵, Kw=10⁻¹⁴ mol²litre⁻²:
Answer: (D)
Solution
Kb=Kw/Ka=5.56×10⁻¹⁰; [OH⁻]=√(Kb×1)=2.36×10⁻⁵; pOH=4.63; pH=9.4.
What is the pH of a 1 M CH₃COONa solution? Ka of acetic acid=1.8×10⁻⁵, Kw=10⁻¹⁴ mol²litre⁻²:
Kb=Kw/Ka=5.56×10⁻¹⁰; [OH⁻]=√(Kb×1)=2.36×10⁻⁵; pOH=4.63; pH=9.4.