General Chemistry (Alexandra Gomez) :: Intro/Background - Digication

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General Chemistry (Alexandra Gomez)

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DRAFT: This module has unpublished changes.
DRAFT: This module has unpublished changes.

Lab 6a: Standardizing a Solution of Sodium Hydroxide

  • Intro/Background
  • Methods/Equipment
    • Materials
    • Methods/Procedure
  • Data Analysis
    • Primary Data
      • Graphs
    • Sample Calculations
  • Conclusions
    • Source of Error
    • No Copyright Infringement Intended
DRAFT: This module has unpublished changes.

Purpose:  To accurately determine the molarity of a sodium hydroxide (NaOH)  solution via titration, which is to standardize the diluted sodium hydroxide solution.  This standardizing technique is an essential lab skill to attain.

 

Important Notes:

Sodium Hydroxide (NaOH) is the base being titrated, while potassium hydrogen phthalate (KHC8H4O4, but will later be referred to as KHP) is the acidic titrant.

 

Equally important information is the following background knowledge:

 

The dissociation process of KHC8H4O4 is:

KHC8H4O4 + H2O -> K+ + C8H4O4- + H3O+

 

NaOH also dissociates in aqueous solutions

NaOH -> Na+ + OH-

(1 mol of NaOH yields 1 mole of OH- ions respectively.)

 

In the acid-base reaction to be examined, the OH- ions react with the H30 ions from the KHP solution:

OH- + H3O -> 2 H2O

 

 

 

We can only obtain the measurement for the volume at which the titrant was  NEUTRAL by irrovacably acidifying it. It is the equivalence point we seek, which is to be measured using the pH sensor and data collection system, NOT with indicators- so as to avoid subjectivity.  The maximum of the derivative for each individual trial's slope reads the equivalence point.

The equivalence point derives from neutralization.

DRAFT: This module has unpublished changes. Show Comments (0) and Tags In order to comment on this portfolio you must be logged in to the school or organization it is associated with. If you have a Digication account, you may log in below: username: password:

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