calculate the morality of THE H2SO4 solution for each of the three runs. do the three values agree closely together with each other.
Part A. Titration 1
volume of unknown acid =20ml
initial buret reading of NaOH =0.5 ml
final buret reading of NaOH=10.0ml
See your post above.
To calculate the molarity of the H2SO4 solution for each of the three runs, you need to know the balanced chemical equation for the reaction between the unknown acid (H2SO4) and NaOH.
Let's assume the balanced equation is as follows:
H2SO4 + 2NaOH -> Na2SO4 + 2H2O
In order to determine the molarity of H2SO4, you need to know the volume of NaOH used in the reaction and the molarity of NaOH solution.
From the given information:
Volume of unknown acid (H2SO4) = 20 ml
Initial buret reading of NaOH = 0.5 ml
Final buret reading of NaOH = 10.0 ml
To calculate the volume of NaOH used, you need to find the difference between the final and initial buret readings:
Volume of NaOH used = Final reading - Initial reading
Volume of NaOH used = 10.0 ml - 0.5 ml
Volume of NaOH used = 9.5 ml
Now, you need to determine the molarity of NaOH used. To do this, you need to know the concentration (molarity) of the NaOH solution you used in the titration.
Once you have the volume of NaOH used and its molarity, you can use the balanced chemical equation to determine the moles of H2SO4 present in the reaction. Since the balanced equation shows a 1:1 stoichiometric ratio between H2SO4 and NaOH, the moles of NaOH used will be equal to the moles of H2SO4 present in the solution.
Finally, to calculate the molarity of the H2SO4 solution, divide the moles of H2SO4 by the volume of H2SO4 solution used in the titration (20 ml).
Repeat this process for all three runs and compare the calculated molarity values. If the three values agree closely with each other, it indicates good precision in the experimental results.