Neutralization occurs at the stoichiometric point.
For this titration, the stoichiometric point is where the moles of
of the added titrant (HCl) is equal to the moles of
of the analyte (NaOH).
Basically, we want to get the amount of moles of HCl = the amount of moles of NaOH.
Just to see things out, our chemical equation is:
The net ionic equation for this is:
First, we find the moles of NaOH by diving its molarity
(M) by the volume
.110 M / .025 L = 0.00275 mol (Remember to convert mL to L)
Since we want to neutralize only half
of the hydroxide ions, we have to divide the moles by 2.
0.00275/2 = 0.001375 mol
Remember our moles of
must equal, so we can set our moles of HCl to 0.001375 mol NaOH, and solve for the unknown volume.
.150 M * V = 0.001375 mol (Molarity*Volume= moles)
Our answer will come out to be 0.009166 or
Hope this helps!