how does the value of $k_a$ and $k_b$ compare with the concentrations of hydronium ion and hydroxide…

how does the value of $k_a$ and $k_b$ compare with the concentrations of hydronium ion and hydroxide ion?\n$k_a\times k_b = h_3o^+oh^-$\n$k_a\times k_b>h_3o^+oh^-$\n$k_a\times k_b<h_3o^++oh^-$\n$k_a\times k_b=\frac{h_3o^+}{oh^-}$

how does the value of $k_a$ and $k_b$ compare with the concentrations of hydronium ion and hydroxide ion?\n$k_a\times k_b = h_3o^+oh^-$\n$k_a\times k_b>h_3o^+oh^-$\n$k_a\times k_b<h_3o^++oh^-$\n$k_a\times k_b=\frac{h_3o^+}{oh^-}$

Answer

Explanation:

Step1: Recall ion - product constant and acid - base dissociation constants

The ion - product constant of water $K_w=[H_3O^+][OH^-]$. Also, for a conjugate acid - base pair, $K_a\times K_b = K_w$.

Answer:

$K_a\times K_b=[H_3O^+][OH^-]$