NaOH rough draft.docx - Richard Romero Standardization of NaOH Draf Abstract The purpose of this experiment is to standardize a solution of NaOH by

NaOH rough draft.docx - Richard Romero Standardization of...

This preview shows page 1 - 3 out of 6 pages.

Richard Romero October 01, 2019 Standardization of NaOH Draf Abstract The purpose of this experiment is to standardize a solution of NaOH by accurately and precisely determining the concentration used in a titration with Potassium Acid Phthalate. Some techniques include using titrations as well as phenolphthalein as our indicator to tell us when to stop titrating the solution as it is standardized. Overall, found that the concentration that was standardized from a sample of NaOH and KHP was relatively close in concentrations of all 4 successful titrations with the RSD of 2.7 %, aiming for less than 3% which is how precise the concentration was. The average found was 0.1155 M with a percent error of 2.1%. Introduction The purpose of this experiment is to standardize a solution of NaOH by accurately and precisely recording the concentration used in a titration. The reaction studied was Potassium Acid Phthalate (KHP) and NaOH to make H 2 O and NaOH, as shown in equation (1) below. KHP was used as the acid to standardize the solution. KHC 8 H 4 O 4 (aq) + NaOH (aq) NaKC 8 H 4 O 4 (aq) + H 2 O (l) Using KHP was a good choice because when measuring out the solid it is easier to get a better measurement with a solid than a liquid. Also, KHP has a 1:1 mole ratio with NaOH as shown in equation (1). With a mole ratio of 1:1, it is easier to convert from one chemical substance to another. When distinguishing between which indictor to use, it is important to show a clear distinction of when the solution is standardizing. Phenolphthalein will change to pink at a pH of 8, to make a titration you need an indicator to help tell you when the solution
Image of page 1

Subscribe to view the full document.

concentration is met. After recording three good trials of the titration, the amount of KHP (g) and the volume of NaOH titrated into KHP (mL), along with the final concentration of that trial will be used to calculate the NaOH concentration using equation (2) below After the solution is
Image of page 2
Image of page 3
  • Fall '18

What students are saying

  • Left Quote Icon

    As a current student on this bumpy collegiate pathway, I stumbled upon Course Hero, where I can find study resources for nearly all my courses, get online help from tutors 24/7, and even share my old projects, papers, and lecture notes with other students.

    Student Picture

    Kiran Temple University Fox School of Business ‘17, Course Hero Intern

  • Left Quote Icon

    I cannot even describe how much Course Hero helped me this summer. It’s truly become something I can always rely on and help me. In the end, I was not only able to survive summer classes, but I was able to thrive thanks to Course Hero.

    Student Picture

    Dana University of Pennsylvania ‘17, Course Hero Intern

  • Left Quote Icon

    The ability to access any university’s resources through Course Hero proved invaluable in my case. I was behind on Tulane coursework and actually used UCLA’s materials to help me move forward and get everything together on time.

    Student Picture

    Jill Tulane University ‘16, Course Hero Intern

Ask Expert Tutors You can ask 0 bonus questions You can ask 0 questions (0 expire soon) You can ask 0 questions (will expire )
Answers in as fast as 15 minutes