Questions1. Write a balanced chemical equation for the reaction of KHP and NaOH. Use the molecularformulas and include states of matter.2. If the balance were not tared prior to weighing out the KHP how would you expect this to affectthe molarity of NaOH calculated? What type of error is this?3. Following a standardization reaction, the concentration of an aqueous solution of NaOH isdetermined to be 0.4510 M.a. What is the mass of NaOH in 50.0 mL of this solution? Show your work.b. What mass of KHP would be needed to completely react with 50.0 mL of this NaOHsolution? Show your work. Name:Date:Experiment # 11: Acid-Base Titration: Standardization of NaOHData and resultsData table *Remember to include unitsTrial 1Trial 2Trial 3Trial 4Mass of KHC8H4O4 (KHP)Initial buret reading (NaOH)Final buret reading (NaOH)Volume of NaOH usedResults tableTrial 1Trial 2Trial 3Trial 4Moles of KHPMoles of NaOHVolume of NaOH (L)Molarity of NaOHAverage molarity of NaOHSample calculation:In the space below show complete calculations for moles of KHP and molarity of NaOH using data fromTRIAL 2 only. Include formulas and units.

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1. Write a balanced chemical equation for the reaction of KHP and NaOH. Use the molecular formulas and include states of matter.

Chemical Principles in the Laboratory

11th Edition

ISBN:9781305264434

Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi

Chapter24: The Standardization Of A Basic Solution And The Determination Of The Molar Mass Of An Acid

Section: Chapter Questions

Problem 2ASA: In an acid-base titration, 21.16 mL of an NaOH solution are needed to neutralize 20.04 mL of a...

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