Monday
March 30, 2015

Homework Help: Chemistry

Posted by Saira on Wednesday, July 15, 2009 at 12:40am.

A 0.040M solution of a monoprotic acid is 14% ionized. Calculate the Ka for the weak acid.

----------------
so:
HX <---> H+ + X-

Ka= [H+][X-]/ [HX]

Since its a monoprotic acis i know the concentration of H and X will be equal

And the HX will be 86% (100%-14%)

BUt i m not sure how to solve for it

Answer this Question

First Name:
School Subject:
Answer:

Related Questions

chemistry - A. Strong Base 1.) What is the concentration of a solution of KOH ...
chemistry - Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. ...
chemistry - Weak Acid 1.) The pH of a 0.060M weak monoprotic acid HA is 3.44. ...
Chemistry 104 - A 0.30M solution of a weak monoprotic acid is 0.41% ionized. ...
Chemistry - A 0.490 M solution of an unknown monoprotic weak acid, HA, is 2.80% ...
AP CHEMISTRY - Determine the volume of 0.125 M NaOH required to titrate to the ...
chemistry - In a 1.070 M aqueous solution of a monoprotic acid, 4.81% of the ...
chemistry - A 0.010 M solution of a weak monoprotic acid has a pH of 3.70. What ...
Chemistry - In a 1.760 M aqueous solution of a monoprotic acid, 3.21% of the ...
chemistry - enzoic acid is a weak monoprotic acid with Ka = 6.510-5 M. NaOH(s) ...

Members