Asked by anonymous
Known:
Cyanaocetic acid
Ka=3.55*10^-3
ionization equation: HC3H2NO2<==> H^+ + C3H2NO2^-
Unknown: pH of 0.4M of Cyanaocetic acid
How can I find out the pH of 0.4M of Cyanaocetic acid ? Is there another way solving for it other than using ICE chart? Please help me out.I really need this. Thanks in advance.
Cyanaocetic acid
Ka=3.55*10^-3
ionization equation: HC3H2NO2<==> H^+ + C3H2NO2^-
Unknown: pH of 0.4M of Cyanaocetic acid
How can I find out the pH of 0.4M of Cyanaocetic acid ? Is there another way solving for it other than using ICE chart? Please help me out.I really need this. Thanks in advance.
Answers
Answered by
GK
Let [H+] = x
Ka = [H^+][C3H2NO2^-] / [HC3H2NO2]
3.55x10^-3 = x^2 / (0.4-x)
•For an exact solution, you must convert the previous equation to a quadratic trinomial equal to 0, the solve.
•For an approximate solution, you assume that
(0.4-x)=0.4, when x is much smaller than 0.4.
Using the approximate method, 3.55x10^-3 = x^2 / 0.4.
x = [H+] = sqrt[(0.4)(3.55x10^-3)] = 0.0377 M
pH = 1.4
For a more precise answer, solve for x:
x^2 / (0.4-x) = 3.55x10^-3
Ka = [H^+][C3H2NO2^-] / [HC3H2NO2]
3.55x10^-3 = x^2 / (0.4-x)
•For an exact solution, you must convert the previous equation to a quadratic trinomial equal to 0, the solve.
•For an approximate solution, you assume that
(0.4-x)=0.4, when x is much smaller than 0.4.
Using the approximate method, 3.55x10^-3 = x^2 / 0.4.
x = [H+] = sqrt[(0.4)(3.55x10^-3)] = 0.0377 M
pH = 1.4
For a more precise answer, solve for x:
x^2 / (0.4-x) = 3.55x10^-3
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.