Question

Calculate the degree of hydrolysis ammonium acetate. Given Kₐ = 1.75 × 10⁻⁵ ; Kᵦ = 1.80 × 10⁻⁵.

A. 2.3 × 10⁻⁶
B. 5.63 × 10⁻³
C. 8.4 × 10⁻²
D. 9.8 × 10⁻¹

Answer 1

The degree of hydrolysis of ammonium acetate is calculated using the equilibrium constants for acetic acid and ammonia, resulting in a very small hydrolysis value due to the weak acid-base combination.

Step-by-step explanation:

To calculate the degree of hydrolysis of ammonium acetate, we can use the concept of acid-base equilibria. Ammonium acetate is a salt of a weak acid (acetic acid) and a weak base (ammonia). In water, it can hydrolyze to form acetic acid and ammonia. The equilibrium constants (Ka for the acid and Kb for the base) are essential to determining the degree of hydrolysis.

To find the degree of hydrolysis (h), we use the formula:

h = √(Ka * Kb / Kw)

where Kw is the ionic product of water, which is 1.0 x 10-14 at 25°C. Plugging in the given values:

h = √((1.75 x 10-5) * (1.80 x 10-5) / (1.0 x 10-14))

h ≈ √(3.15 x 10-9)

h ≈ 1.77 x 10-5

Given the typical approximation that h << 1 for weak acid-base combinations, the degree of hydrolysis is often very small, as it is in this case.