the acetate ion is the conjugate base of the weak acid acetic acid. the value of ( k_{b} ) for ( mathrm{ch}_{3} mathrm{coo}^{-} ) is ( 5.56 imes 10^{-10} ). write the equation for the reaction that goes with this equilibrium constant. it is not necessary to include states such as (aq) or (l)

Question

the acetate ion is the conjugate base of the weak acid acetic acid. the value of ( k_{b} ) for ( mathrm{ch}_{3} mathrm{coo}^{-} ) is ( 5.56 	imes 10^{-10} ). write the equation for the reaction that goes with this equilibrium constant. it is not necessary to include states such as (aq) or (l)

Accepted Answer

# Explanation:
## Step1: Recall the definition of $K_b$
$K_b$ is the base - dissociation constant. For a base $B$, the general reaction is $B + H_2O
ightleftharpoons BH^+ + OH^-$.
## Step2: Apply the definition to acetate ion ($CH_3COO^-$)
When acetate ion ($CH_3COO^-$) acts as a base, it accepts a proton ($H^+$) from water. The reaction is $CH_3COO^-+H_2O
ightleftharpoons CH_3COOH + OH^-$

# Answer:
$CH_3COO^-+H_2O
ightleftharpoons CH_3COOH + OH^-$

Sovi.AI - AI Math Tutor

QUESTION IMAGE

Question

Explanation:

Step1: Recall the definition of \(K_b\)

Step2: Apply the definition to acetate ion (\(CH_3COO^-\))

Answer: