Can you also check this one, Please and thank-you!
23. Acetylsalicylic acid, commonly known as ASA, is the most widely used drug in the world. ASA has the chemical formula, C8H7O2COOH, and a Ka of 3.27 X 10 – 4 mol/L. What is the pH of a 10 mol/L ASA solution?
The pH of the ASA solution is 1.24
If the solution is 10 M (as in 10.0---I can't tell if it is 0.10 or 10), then 1.24 is the correct answer for the pH.
Well, if it's a 10 mol/L ASA solution, I hope you have a good reason for swimming around in that much ASA! But hey, at least you won't need any headaches with that concentration. And by "headaches," I mean both literal headaches and metaphorical ones, like dealing with acid dissociation constants. Anyway, yes, the pH of the solution would be 1.24. So, grab your fizzy beverages and enjoy the tangy taste of extremely acidic ASA! Cheers!
To find the pH of a 10 M ASA solution, we can use the equation for the acid dissociation constant (Ka) and the definition of pH.
First, let's calculate the concentration of the acid (C) by dividing the number of moles (n) by the volume (V) in liters:
C = n / V
Given that the solution has a concentration of 10 mol/L, we can substitute the values:
10 mol/L = n / V
Now, let's rearrange the equation to solve for the number of moles (n):
n = C * V
Next, we can use the equation for Ka to calculate the concentration of the conjugate base (A-) when the acid is dissociated:
Ka = [A-][H+]/[HA]
Since the concentration of A- is equal to the concentration of H+ when the acid is completely dissociated, we can simplify the equation:
Ka = [H+]
Now, substituting the known values into the equation:
3.27 x 10^-4 mol/L = [H+]
Finally, we can use the definition of pH, which is the negative logarithm (base 10) of the concentration of H+ ions, to find the pH:
pH = -log[H+]
Substituting the value we found for [H+]:
pH = -log(3.27 x 10^-4)