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?

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Answer 1 · 2016-07-04T22:10:54

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

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.

29.4mL of an CH_3COOHCH_3COOH solution were titrated with 18.5mL of a 0.175M LiOHLiOH solution to reach the equivalence point What is the molarity of the CH_3COOHCH_3COOH solution?