the following data were collected when titrating 25.00 mL samples of HCL with 0.511 M NaOH:
initial burette reading (mL): trial 1=1.06 trial2=0.04 trial3=1.03
final burette reading (mL): trial1= 27.60 trial2=26.21 trial3=27.22
MolarityAcid*.025=.511M*volumebase
averaging the volume of base:
27.60-1.06=26.54
26.21-.04=26.17
27.22-1.03=26.18
Now I am wondering what your question is.
using this data what is the [HCL]?
To determine the volume of NaOH needed to neutralize the HCl, you need to calculate the difference between the initial and final burette readings. Subtract the initial burette reading from the final burette reading for each trial to get the volume of NaOH used.
For example, for trial 1:
Volume of NaOH used = Final burette reading - Initial burette reading
Volume of NaOH used = 27.60 mL - 1.06 mL
Volume of NaOH used = 26.54 mL
For trial 2:
Volume of NaOH used = Final burette reading - Initial burette reading
Volume of NaOH used = 26.21 mL - 0.04 mL
Volume of NaOH used = 26.17 mL
For trial 3:
Volume of NaOH used = Final burette reading - Initial burette reading
Volume of NaOH used = 27.22 mL - 1.03 mL
Volume of NaOH used = 26.19 mL
Now you have the volumes of NaOH used for each trial.