29.4mL of an #CH_3COOH# solution were titrated with 18.5mL of a 0.175M #LiOH# solution to reach the equivalence point What is the molarity of the #CH_3COOH# solution?

1 Answer
Jul 4, 2016

Answer:

#sf(0.11color(white)(x)"mol/l")#

Explanation:

Start with the equation:

#sf(CH_3COOH_((aq))+LiOH_((aq))rarrCH_3COO^(-)Li_((aq))^(+)+H_2O_((l))#

Concentration = amount of solute / volume of solution

#sf(c=n/v)#

#:.##sf(n=cxxv)#

#:.##sf(nLiOH=0.175xx18.5/1000=0.003238)#

Where #sf(n)# refers to the number of moles.

From the 1:1 molar ratio as shown by the equation, we can say that the number of moles of ethanoic acid must be the same.

#:.##sf([CH_3COOH_((aq))]=n/v=0.003238/(29.4/1000)=0.11color(white)(x)"mol/l")#

Note that I have converted #sf(ml)# to #sf(litre)# by dividing by 1000.