Posted by **khin** on Thursday, May 13, 2010 at 6:13am.

Chloroacetic acid has a relatively large equilibrium constant, so at low acid concentrations it is necessary to use the quadratic equation in order to calculate the concentrations of the aqueous species. Ka for ClCH2COOH is 1.4 ยด 10-3. For the problems that follow, consider one liter of a solution that originally had 0.0200 mol of chloroacetic acid.

What is the equilibrium concentration of [ClCH2COOH]?

a. 0.010

b. 0.012

c. 0.015

d. 0.017

## Answer This Question

## Related Questions

- Hayden - Chloroacetic acid has a relatively large equilibrium constant, so at ...
- Chemistry - A .1M solution of chloroacetic acid is 11% ionized. Using this ...
- Chem - What is the equilibrium concentration of chloroacetic acid in a solution ...
- chm - The equilibrium constant for the equation 2 H2(g) + CO(g) CH3OH(g) Is 19 ...
- chemistry - A diprotic acid solution H2A has a molarity of .95 M. the ...
- chemistry - Use the systematic treatment of equilibrium to determine the pH and ...
- Chemistry - Consider the equilibrium 2NOCl (g) <---> 2NO (g) + Cl2 (g). In...
- chemistry - the acid dissociation constant of dichloroethanoic acid is 0.033 . ...
- chemistry 2 - Calculate the relative concentrations of o-ethylbenzoic acid (pKa ...
- Chemistry - Okay so my lecturer has this in our slides and there are no notes ...

More Related Questions