This is my question:
AspirinTM (acetylsalicylic acid) is a monoprotic acid with molar mass of 180g/mol. An aqueous solution containing 3.3 g/L has a pH of 2.62. What percentage of acetylsalicylic acid molecules ionizes
in the solution?
first, the H+ in solution.
pH=-log[H]
2.62=-logH
H=antilog-2.62= 0.00239883292
Now the H in the aspirin: molesH=3.3/180= you do it.
Now divide the H in solution by the H in the aspirin, and forpercent, multiply by 100
To determine the percentage of acetylsalicylic acid molecules that ionize in the solution, you need to calculate the concentration of the acid in its ionized form.
Let's start by finding the concentration of acetylsalicylic acid in the solution. The molar mass of acetylsalicylic acid is given as 180 g/mol, and the solution has a concentration of 3.3 g/L. We can use these values to find the molarity (M) of the solution:
Molarity (M) = Mass of solute (g) / Volume of solution (L)
Plugging in the values, we have:
M = 3.3 g/L / 180 g/mol
Next, to determine the concentration of ionized form of acetylsalicylic acid (let's call it [A-]), we need the concentration of hydrogen ions ([H+]) in the solution. The pH value of 2.62 gives us this information.
pH = -log[H+]
So, we can rearrange this equation to find [H+]:
[H+] = 10^(-pH)
Plugging in the value, we have:
[H+] = 10^(-2.62)
Now, we assume that each molecule of acetylsalicylic acid that ionizes will contribute one H+ ion. Therefore, the concentration of ionized form [A-] is equal to the concentration of hydrogen ions [H+].
Now, let's calculate the concentration of ionized form [A-] in Molarity (M) using the concentration of hydrogen ions [H+].
[A-] = [H+] = 10^(-2.62)
Finally, to find the percentage of acetylsalicylic acid molecules that ionize, we need to compare the concentration of [A-] with the initial concentration of acetylsalicylic acid. We can use the following equation:
Percentage Ionization = ([A-] / Initial concentration of acetylsalicylic acid) x 100
Substitute the values to calculate the percentage of ionization.
To determine the percentage of acetylsalicylic acid molecules that ionizes in the solution, you can use the pH of the solution. The pH can be related to the concentration of H+ ions in the solution using the equation:
pH = -log[H+]
First, let's calculate the concentration of H+ ions in the solution using the pH given.
pH = 2.62
[H+] = 10^(-pH)
[H+] = 10^(-2.62)
[H+] = 1.47 x 10^(-3) M
Since acetylsalicylic acid is a monoprotic acid, it will dissociate in water as follows:
Acetylsalicylic acid (HA) ⇄ H+ + A-
The percentage ionization can be calculated using the formula:
% Ionization = (concentration of H+ ions) / (initial concentration of acid) x 100
The concentration of H+ ions is 1.47 x 10^(-3) M.
To find the initial concentration of acetylsalicylic acid, we need to convert the given concentration from g/L to mol/L.
Molar mass of acetylsalicylic acid = 180 g/mol
Concentration of acetylsalicylic acid = 3.3 g/L
Concentration of acetylsalicylic acid = (3.3 g/L) / (180 g/mol)
Concentration of acetylsalicylic acid = 0.0183 mol/L
Now, we can calculate the percentage ionization.
% Ionization = (1.47 x 10^(-3) M) / (0.0183 mol/L) x 100
% Ionization ≈ 8.03%
Therefore, approximately 8.03% of the acetylsalicylic acid molecules ionize in the solution.