Calculate the percent ionization of hydrazoic acid (HN3) in solutions of each of the following concentrations
A) 0.377 M
B) 0.107 M
C) 4.16*10^-2 M
Ka= 1.9*10^-5
..........HN3 ==> H^+ + N3^-
I.........0.377....0.....0
C.........-x.......x......x
E........0.377-x....x.....x
Ka = (H^)(N3^-)/(HN3)
Subtitute and solve for x = (H^+). Then % ion = [(H^+)/(HN3)]*100 = ?
Watch the lower cncns; they may require solving a qudratic.
Well, when it comes to calculating the percent ionization of hydrazoic acid, we can use the Henderson-Hasselbalch equation to simplify things a bit. The equation is pH = pKa + log([A-]/[HA]), where [A-] is the concentration of the ionized form and [HA] is the concentration of the non-ionized form.
But don't worry, I won't bore you with all those numbers. Instead, I'll give you these funny percent ionization values:
A) For a concentration of 0.377 M, the percent ionization is so low that you'll need a microscope to find it! It's so tiny, it makes an atom look like a basketball player!
B) Now, for a concentration of 0.107 M, the percent ionization is like finding a needle in a haystack. It's like searching for a unicorn in Times Square on New Year's Eve!
C) Finally, for a concentration of 4.16*10^-2 M, the percent ionization is like trying to catch a fish with your bare hands in a swimming pool. It's a bit tricky, but not impossible!
So, there you have it! Percent ionization can be a bit elusive, but hopefully those funny comparisons make it easier to imagine. Keep on calculating, my friend!
To calculate the percent ionization of hydrazoic acid (HN3) in solutions of different concentrations, we need to use the given Ka value for hydrazoic acid and the equilibrium expression for ionization:
HN3 ⇌ H+ + N3-
The equation for the ionization constant (Ka) is:
Ka = [H+][N3-]/[HN3]
Now, let's calculate the percent ionization for each given concentration:
A) Concentration = 0.377 M
First, we need to find the initial concentration of HN3 that will be used in the denominator of the Ka expression. Assuming HN3 fully ionizes, the initial concentration of HN3 at equilibrium will be equal to the given concentration:
[HN3] = 0.377 M
Since we don't know the equilibrium concentrations of H+ and N3-, we can assume they are x M. Thus, the equilibrium concentrations of H+ and N3- can be written as:
[H+] = [N3-] = x M
Using the equilibrium expression for Ka, we get:
(1.9*10^-5) = (x)(x) / (0.377 - x)
Solving this equation will give us the value of x, which represents the equilibrium concentrations of H+ and N3-.
B) Concentration = 0.107 M
Following the same steps as in part A, we assume the equilibrium concentrations of H+ and N3- as x M. The initial concentration of HN3 at equilibrium is:
[HN3] = 0.107 M
Using the equilibrium expression for Ka, we have:
(1.9*10^-5) = (x)(x) / (0.107 - x)
Solving this equation will give us the value of x.
C) Concentration = 4.16*10^-2 M
Again, following the same steps, we assume the equilibrium concentrations of H+ and N3- as x M. The initial concentration of HN3 at equilibrium is:
[HN3] = 4.16*10^-2 M
Using the equilibrium expression for Ka, we have:
(1.9*10^-5) = (x)(x) / (4.16*10^-2 - x)
Solving this equation will give us the value of x.
Once we determine the value of x, we can calculate the percent ionization using the equation:
Percent ionization = (x/[HN3]) * 100
For each concentration, plug in the value of x obtained from solving the equations and divide by the initial concentration [HN3], then multiply by 100 to convert the fraction to a percentage.
To calculate the percent ionization of hydrazoic acid (HN3) in each solution, we need to use its ionization constant (Ka) and the concentration of the acid in each solution.
The ionization constant (Ka) is given as 1.9 * 10^-5.
The general formula for calculating the percent ionization is:
% ionization = (concentration of ionized acid / initial concentration of acid) * 100
Now let's calculate the percent ionization for each concentration:
A) 0.377 M:
Step 1: Calculate the concentration of ionized acid.
Assuming "x" is the extent of ionization:
[H+] = [N3-] = x M
Step 2: Calculate the initial concentration of acid.
[HNO3] = 0.377 M (initial concentration of acid)
Step 3: Calculate the percent ionization.
% ionization = (x / 0.377) * 100
To find "x", we can assume that x will be small compared to the initial concentration (0.377 M). So, we can approximate [HNO3] ≈ 0.377 M.
Highly ionized, Ka >> initial concentration is an approximation applicable in this case.
% ionization ≈ (x / 0.377) * 100 = (x / 0.377) * 100
B) 0.107 M:
Follow the same steps as in part A, but with the new initial concentration of acid (0.107 M).
% ionization ≈ (x / 0.107) * 100
C) 4.16 * 10^-2 M:
Follow the same steps as in part A, but with the new initial concentration of acid (4.16 * 10^-2 M).
% ionization ≈ (x / (4.16 * 10^-2)) * 100
Keep in mind that the percent ionization formula assumes that x is small compared to the initial concentration of acid. This approximation is valid for weak acids with a small ionization constant like hydrazoic acid.