Ask a New Question

Question

A 0.039 M solution of a weak acid (HA) has a pH of 4.28. What is the Ka of the acid?
9 years ago

Answers

DrBob222
pH = -log (H^+)
(H^+) = ?. I estimate 5E-5 but you need a better answer than that.

...........HA ==> H^+ + A^-
I........0.039....0......0
C.........-x......x......x
E......0.039-x....x......x

The pH tells you the value of x; i.e., approx 5E-5 so you can evaluate x and 0.039-x.
Plug those values into the Ka expression and evaluate Ka.
9 years ago

Related Questions

When a 0.1M solution of weak acid HA was titrated with a 0.1M NaOH. The pH measured when Vol<sub>bas... When a 0.1M solution of weak acid HA was titrated with a 0.1M NaOH. The pH measured when Volbase=1/2... A 0.010 M solution of a weak monoprotic acid is 3.0% dissociated. What is the equilibrium constant,... A 0.010 M solution of a weak monoprotic acid has a pH of 3.70. What is the acid-ionization constant,... A 0.10 M solution of a weak monoprotic acid has a hydronium-ion concentration of 5.0 ยด 10-4 M. What... A 0.39 M solution of a weak acid is 3.0% dissociated. Calculate Ka. A 0.035 M solution of a weak base has a pH of 10.88. What is the Kb for the acid? Where Di I even... In a .25 M solution, a weak acid is 3.0% dissociated. A. calculate the pH of the solution B. cal... A 0.60 M solution of a weak acid, HA, has a pH of 3.72. What is the percentage ionization of the aci...
Ask a New Question
Archives Contact Us Privacy Policy Terms of Use