acid: HCI 0.10 M
Base:NaOH O.050 M
3 ml of HCI was used.
Calculate the volume of base required to reach the equivalence point of this titration.
Somewhere in the finding the solution, i have to use the fact that
Moles HCl = moles NaOH.
this is what i have so far:
Volume of base= [(Molarity of NaOH)( Volume of NaOH)]/Molarity of HCI
(0.050 M)( mL) = (0.10 M)(x mL)
when do i use Moles HCl = moles NaOH.
Your work is off.
MolesHCL=MolesNaOH
VolumeHCl(MolarityHCL)=Volumebase*MolarityBAse
Volumebase=VolumeHCl*MolarityHCl/MolarityNaOH
To determine the volume of base required to reach the equivalence point of this titration, you can use the fact that the moles of acid (HCl) will be equal to the moles of base (NaOH) at the equivalence point. Here's how you can incorporate this information into your calculation:
1. First, calculate the moles of HCl used:
Moles HCl = Molarity of HCl x Volume of HCl used
Moles HCl = 0.10 M x 0.003 L (converted 3 ml to liters)
Moles HCl = 0.0003 moles
2. Since Moles HCl = Moles NaOH at the equivalence point, you can now calculate the volume of NaOH needed:
Moles NaOH = Moles HCl
Molarity of NaOH x Volume of NaOH = 0.0003 moles
3. Rearrange the equation to solve for the volume of NaOH:
Volume of NaOH = 0.0003 moles / Molarity of NaOH
Volume of NaOH = 0.0003 moles / 0.050 M
Now, you have all the necessary information to calculate the volume of NaOH required to reach the equivalence point.