# You have a vinegar solution you believe to be 0.83 M. You are going to titrate 20.0mL of it with a NaOH solution that you know to be 0.519 M. At what volume of added NaOH solution would you expect to see the end point?

May 8, 2017

You should expect to see the endpoint at 32 mL of added $\text{NaOH}$.

#### Explanation:

Let's write the formula for acetic acid as $\text{HA}$.

Then the equation for the reaction is

$\text{HA + NaOH" → "NaA" + "H"_2"O}$.

1. Calculate the moles of $\text{HA}$

$\text{Moles of HA" = 0.0200 color(red)(cancel(color(black)("L HA"))) ×( "0.83 mol HA")/(1 color(red)(cancel(color(black)("L HA")))) = "0.0166 mol HA}$

2. Calculate the moles of $\text{NaOH}$

$\text{Moles of NaOH" = 0.0166 color(red)(cancel(color(black)("mol HA"))) × ("1 mol NaOH")/(1 color(red)(cancel(color(black)("mol HA")))) = "0.0166 mol NaOH}$

3. Calculate the volume of the $\text{NaOH}$

$\text{Volume of NaOH" = 0.0166 color(red)(cancel(color(black)("mol NaOH"))) × ("1 L NaOH")/(0.519 color(red)(cancel(color(black)("mol NaOH")))) = "0.032 L" = "32 mL}$