Experiment 12 Neutralization Titration-Standardization of a Sodium Hydroxide Solution IV*. *DATA: *Trial I*: Tri*a*l II: Initial buret reading Final buret reading Volume of NaOH Moles of KHP Molarity of NaOH Trial III: V.CALCULATIONS: Write the balanced molecular equation for the reaction occurring. Calculate the moles of KHP used. Moles of base present in volume of NaOH used. Molarity of your base solution for each of the three titration. Average the values of the molarity of the base. VII. SUMMARY AND RESULTS: Conclusion: Give the values of the molarity of your NaOH solution along with the average value. Report these values in tabular form. Give any problems you encountered during the standardization of your base solution. Error: In your discussion paragraph, give and explain two possible errors, other than calculation errors, that could occur in this experiment. How could these errors be minimized? Discuss problem that you encountered, irregularities in your results, and how you handled them. If you were to do this lab again or were to advise another chemistry 3 student regarding this experiment, what useful information would you relate? Include a traditional assessment of the strengths and weaknesses of this experiment, demonstrating your knowledge of what was done. VIII. POSTAL LABORATORY ASSIGNMENT: A student weighed out 1.250g KHP. How many moles was that? A titration 16.86ml of 0.1672 M NaOH. How many moles of NaOH were in this volume? A student weighed a sample of KHP and found it weighed 1.126g titration of this KHP required 20.19ml of base (NaOH). Calculate the molarity of the base. Forgetful Freddy weighed his KHP sample, but forgot to bring his lab notebook along, so he recorded his weighed on paper towel. During his...