Monday
April 21, 2014

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-Dr Bob help!! - 0.100 M solution of a weak acid, HX, is known to be ...
chemisty - 0.100 M solution of a weak acid, HX, is known to be 15% ionized. The ...
PHYSICAL CHEMISTRY - A.CALCULATE THE CRYOSCOPIC CONSTANT OF H2O. USE IT TO ...
AP Chemistry - A 0.00100 M solution of a weak acid HX is 6% ionized. Calculate ...
chemistry - A. Strong Base 1.) What is the concentration of a solution of KOH ...
Chemistry - A student titrates 0.100M KOH into 50.00 ml of weak acid HX. The pH ...
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 20.1 mL sample of a weak monoprotic acid, HX, requires 50.0 mL of ...

Search
Members