2006-12-14 03:41:38 · 4 answers · asked by bollywoodturtle 4 in Science & Mathematics ➔ Chemistry
I think the question is meant as one solution containing two species, not two separate solutions.
Use the Henderson-Hasselbach equation.
pH = pKa + log ([A-]/[HA]
The acid is acetic acid, and in your book, you should be given the pKa of acetic acid. If not, the general value is pKa = 4.75. [A-] is the concentration of the conjugate base, which is sodium acetate. [HA] is the concentration of the acid, which is acetic acid (obviously).
pH = 4.75 + log (0.3/.1) = 5.22
Lastly, always be sure to check your answer. pKa is the pH at which you have equal concentrations of acid and base. Since in your solution, your concentration of your base is higher than your acid, the pH should be higher as well, which as the number shows, it is.
2006-12-14 04:52:46 · answer #1 · answered by romanwahoo 2 · 0⤊ 0⤋
This is a buffer solution question.
You need to quote the Ka of the acid (it's 1.7 x 10-5).
Then [H+] = Ka x 0.1/0.3.
Then take the logarithm of [H+] to get the pH.
2006-12-14 04:41:46 · answer #2 · answered by Gervald F 7 · 0⤊ 0⤋
Taking the -log(KsubA) yields that answer. I wish i'd desire to tell you extra, yet i've got no longer taken any Chem in a mutually as. i will submit a extra suitable clarification later after looking into it.
2016-12-11 09:01:50 · answer #3 · answered by unck 4 · 0⤊ 0⤋
pH= -log(concentration)
pH(.1)=-log.1=1
pH(.3)= .52287453
2006-12-14 04:23:07 · answer #4 · answered by suraiya a 2 · 0⤊ 2⤋