October 10, 2015

Homework Help: Chemistry

Posted by Cassie on Saturday, April 9, 2011 at 2:54pm.

The pH of a weak monoprotic acid, HA, is 4.55. It took 39.22 ml of 0.2334 M NaOH to titrate 25.00 ml of the acid.

a. Write an equation for the above reaction.

b. Calculate the molarity of the weak acid

c. Write the equilibrium equation. Construct a table showing initial concentration, change in concentration and the equilibrium concentration. Calculate the ionization constant Ka, for the above acid

d. 23.55 ml of the NaOH were added to partially neutralize a new 25.00 ml sample of the acid. The pH of the mixture was measured as 5.33. Calculate Ka for the acid, HA, using the partial neautralization method

Answer this Question

First Name:
School Subject:

Related Questions

More Related Questions