Question

a 10.0 ml sample of 0.75 m c3h6o3 (lactic acid) is titrated with 0.25 m koh. what is the ratio of conjugate base to weak acid, at the point where 15.0 ml of koh has been added during the titration? ka for c3h6o3 is 1.4 x 10-4.

Answer 1

The ratio of conjugate base to weak acid in the solution is 1:1.

Step-by-step explanation:

To determine the ratio of conjugate base to weak acid in the solution, we need to consider the stoichiometry of the reaction between lactic acid (Hox-) and KOH. The balanced equation for the reaction is:

Hox- + OH- → ox²- + H2O

From the stoichiometry of the reaction, we can see that for every 1 mol of lactic acid (Hox-) that reacts, 1 mol of conjugated base (ox²-) is formed. Therefore, the ratio of conjugate base to weak acid is 1:1.