Calulate the degree of ionization for NH3(aq) in 1.0 M solution, Kb = 3.236E-4. I've seen degree ionization for acids and not bases. Do I need to find the Ka [H+] value of the base to determine the degree of ionization?
No, it's the same concept as %ionization for acids. Set up an ICE chart for NH3
..........NH3 + H2O ==> NH4^+ + OH^-
initial...1.0M..........0........0
change.....-x............x........x
equil.....1-x............x........x
Then calculate OH^- and
% ionization = (OH^-)/(1.0)*100 = ?
The degree of ionization is the fraction (the decimal) instead of percent.
calculate the degree of ionization of a 0.05F solution of lactic acid.
if a monoprotic acid,HX, is 3.8% percent ionized in a 0.2F solution,calculate its ionization constant.What is the percentage ionizationof this acid in a 0.01F solution?
To calculate the degree of ionization for NH3 (ammonia) in a 1.0 M solution, we can use the value of Kb (base ionization constant), which is given as 3.236E-4.
Firstly, let's define the equation for the ionization of NH3:
NH3 + H2O ⇌ NH4+ + OH-
Here, NH3 acts as the base, accepting a proton (H+) from water, which forms the ammonium ion (NH4+) and hydroxide ion (OH-).
The degree of ionization (α) for a weak base like NH3 represents the extent to which it undergoes ionization in solution. In this case, α represents the fraction of NH3 molecules which ionize. We can express it as follows:
α = [NH4+] / [NH3]
Since NH3 is a weak base and doesn't ionize completely, we can assume that the initial concentration of NH3 is equal to the concentration of un-ionized NH3 at equilibrium:
[NH3]eq = [NH3]initial = 1.0 M
Now, we need to determine the concentration of NH4+ at equilibrium. Since the solution initially contains only NH3, the concentration of NH4+ at equilibrium is equal to the concentration of NH3 that has ionized:
[NH4+]eq = [NH3]initial - [NH3]eq
To find the concentration of NH3 at equilibrium ([NH3]eq), we need to find out how much of it has ionized using the Kb value.
Kb = [NH4+][OH-] / [NH3]
Since the concentration of OH- is dependent on the degree of ionization (α), we can substitute [OH-] with Kb * α:
Kb = [NH4+][Kb * α] / [NH3]
Simplifying gives us:
α = Kb * [NH3] / [NH4+]
Now we can plug in the given values:
Kb = 3.236E-4
[NH3] = 1.0 M
To solve for [NH4+], we need to convert α to a decimal value, so α = degree of ionization / 100.
Now we can calculate the degree of ionization:
α = Kb * [NH3] / [NH4+]
α = 3.236E-4 * 1.0 M / [NH4+]
Solving for α:
α = 3.236E-4 M / [NH4+]
Since we don't know the concentration of NH4+ at this point, we cannot directly determine the degree of ionization and thus cannot calculate the value. To determine [NH4+], we need more information, such as the initial concentration of NH3.
Therefore, we need additional information or data to calculate the degree of ionization for NH3 in a 1.0 M solution.