Homework Help

A 15.00 mL sample of NaOH was titrated to the stoichiometric point with 17.40 mL of...

user profile pic

spock3 | Student, Undergraduate | Honors

Posted April 23, 2013 at 12:51 PM via web

dislike 1 like

A 15.00 mL sample of NaOH was titrated to the stoichiometric point with 17.40 mL of 0.2340 M HCl. What is the molar concentration of the NaOH solution?

Tagged with chemistry, science

1 Answer | Add Yours

user profile pic

jerichorayel | College Teacher | (Level 1) Senior Educator

Posted April 23, 2013 at 3:17 PM (Answer #1)

dislike 1 like

First, we need to write the chemical equation for this reaction:

`NaOH + HCl -> NaCl + H_2O`

Looking at the balanced chemical equation we can see that there is 1:1 ration between the two reactants. Therefore:

`Mol es HCl = Mol es NaOH`

To determine the molar concentration of the NaOH solution, first we need to get the moles of HCl.

`Mol es HCl = (17.40)/(1000) L * 0.2340 M = 0.0040716 mol es HCl`

Since we know that moles of HCl are equal to the moles of NaOH, therefore:

moles HCl = moles NaOH = 0.0040716

 

`Molarity of NaOH = (mol es NaOH)/(volume of solution (L))`

`Molarity of NaOH = (0.0040716)/(0.015)`

Molarity of NaOH = 0.2714 M

Sources:

Join to answer this question

Join a community of thousands of dedicated teachers and students.

Join eNotes