Question

What is the concentration of [OH⁻] for a mixture that is 0.039 M in NaCH₃COO and 0.057 M in Ba(CH₃COO)2 (Ka(CH₃COOH) = 1.8 × 10⁻⁵)?

Answer 1

To determine the concentration of [OH-] for the given mixture, we can use the relationship [OH-] = Kw / [H3O+], where Kw is the ion product of water and [H3O+] is the concentration of the weak acid in the mixture. using the relationship [OH-] = Kw / [H3O+]. that [H3O+] is 0.057 M, we can solve for [OH-].

Step-by-step explanation:

The concentration of [OH-] can be determined by considering the reaction of the weak acid, CH3COOH, with water: CH3COOH + H2O → CH3COO- + H3O+ Since we know the concentration of CH3COO- for the mixture, we can calculate the concentration of [OH-] using the relationship [OH-] = Kw / [H3O+]. that [H3O+] is 0.057 M, we can solve for [OH-].

To determine the concentration of [OH-] for the given mixture, we can use the relationship [OH-] = Kw / [H3O+], where Kw is the ion product of water and [H3O+] is the concentration of the weak acid in the mixture. using the relationship [OH-] = Kw / [H3O+]. Given that [H3O+] is 0.057 M, we can solve for [OH-].