Write the expression of for the base dissociation constant for hydrazine, N2H4, a weak base. Hydrazine reacts with water to form the N2H5+ ion.
N2H4 + HOH ==>N2H5+ + OH^-
Kb = (N2H5^+)(OH^-)/(N2H4)
Kb=[OH^-]^2/[N2H4]
Ah, hydrazine, the chemist's favorite funny-named compound! Don't worry, I've got just the expression for you:
Kb = [N2H5+][OH-] / [N2H4]
Now, let's break it down a bit. The base dissociation constant, Kb, measures the extent to which a base dissociates in water. In this case, it's hydrazine, N2H4, reacting with water to form the N2H5+ ion.
The expression has a numerator and a denominator. The numerator is the concentration of the N2H5+ ion times the concentration of hydroxide ions, OH-. This represents the products of the reaction.
The denominator is the concentration of the hydrazine, N2H4, which represents the reactant.
So, when you divide the concentrations of the products by the concentration of the reactant, you get the base dissociation constant, Kb. It tells us how much of the hydrazine actually dissociates in water to form the N2H5+ ion. It's like a popularity contest for hydrazine.
Now, go out there and rock that base dissociation constant like a chemistry comedian!
To write the expression for the base dissociation constant for hydrazine, we need to consider the balanced chemical equation for the reaction of hydrazine with water:
N2H4 + H2O ⇌ N2H5+ + OH-
The dissociation constant for a weak base, K_b, is defined as the equilibrium constant for the reaction of the base with water.
The expression for K_b can be written as follows:
K_b = [N2H5+][OH-] / [N2H4]
In this expression, the square brackets [] represent the concentration of each species involved in the reaction. The terms [N2H5+], [OH-], and [N2H4] represent the concentrations of the N2H5+ ion, hydroxide ion (OH-), and hydrazine (N2H4), respectively.
By measuring the concentrations of these species at equilibrium, you can determine the value of the base dissociation constant, K_b, for hydrazine.