an acid has an acid dissociation constant of 2.8×10⁻⁹. what is the base dissociation constant of its…

an acid has an acid dissociation constant of 2.8×10⁻⁹. what is the base dissociation constant of its conjugate base? use (k_ak_b = k_w).\no 2.8×10⁻²³\no 3.6×10⁻⁶\no 2.8×10⁵\no 3.6×10²²

an acid has an acid dissociation constant of 2.8×10⁻⁹. what is the base dissociation constant of its conjugate base? use (k_ak_b = k_w).\no 2.8×10⁻²³\no 3.6×10⁻⁶\no 2.8×10⁵\no 3.6×10²²

Answer

Explanation:

Step1: Recall the relationship formula

$K_aK_b = K_w$, where $K_w=1.0\times 10^{- 14}$ at $25^{\circ}C$ and $K_a = 2.8\times 10^{-9}$.

Step2: Solve for $K_b$

$K_b=\frac{K_w}{K_a}=\frac{1.0\times 10^{-14}}{2.8\times 10^{-9}}$.

Step3: Calculate the value of $K_b$

$K_b=\frac{1.0}{2.8}\times10^{-14 + 9}\approx0.36\times10^{-5}=3.6\times 10^{-6}$.

Answer:

$3.6\times 10^{-6}$