Posted by Liz on Monday, April 23, 2012 at 10:53am.
I found that it came to 6.30 for the pH. So I first balanced the equation set up an "ICE" box and then solved for x using the Ka equation...Ka=([H+][A-])/([HA]), I neglected the +x and -X and plugged in to solve. Then I got the pH by doing the negative log of the x. Hope this helped :)
I agree with 6.30 but I used the Henderson-Hasselbalch equation. It's easier and you don't need an ICE chart.
Related Questions
chemistry - titration - Show that for the titration of a weak acid, HA, with ...
CHEMISTRY FOR DR. BOB or anyone else - A hypothetical weak acid HA, was combined...
Science - Determine the pH of a .10M solution of KA, the potassium salt of HA. ...
Chemistry - An unknown monoprotic weak acid, HA, has a molar mass of 65.0. A ...
Chemistry Very Urgent!! - A 0.035 M solution of a weak acid (HA) has a pH of 4....
chemistry - 1)A solution has a [OH-] of 5.2 x 10-4. What is the [H3O+] in the ...
chemistry - A buffer solution is composed of 0.370M HA, a weak monoproctic acid...
ap chem - A 9.00 M solution of a weak acid, HA, has a pH of 1.30 1.) calculate [...
chemistry - A. Strong Base 1.) What is the concentration of a solution of KOH ...
AP Chemistry - calculate the ph of a 0.10 M CoCl3 solution. The ka value for Co(...
For Further Reading
