Preparation and Standardization of a Sodium Hydroxide Solution

Topics: Sodium hydroxide, Acid, Titration Pages: 3 (574 words) Published: April 11, 2014
Title: Preparation and Standardization of a Sodium Hydroxide Solution

Objective/Purpose: The objective of this experiment will be the standardization of sodium hydroxide using potassium hydrogen phthalate by the titration method. Introduction:
The concentration of solutions can be reported in terms of molarity and normality. Molarity is equal to: HCL, HBR, H2SO4, HNO3
M = mol Solute (mol) (Monoprotic) (Diprotic)
V(L)g solutions (L)

M = __N___ for Monoprotic acids molarity = normality molar mass

One molar solution can be prepared by dissolving the mass of 1 mole of the particular substance in enough water to make a 1L solution.

HCL + NaOH  H2O + NaCl

H2SO4 + NaOH  H2O + Na2SO4

N = __EW__
L EW= molar mass L = number of titratable protons

To perform an acid-base neutralization using the titration technique to determine the concentration (normality) of the NaOH prepared in part A.

C8H5O4K + NaOH H2O + KC8H4O4Na


*Acid base indicator- substances that have different colors in acidic and basic environments

*Phenolphthalein- colorless in acid and pink in base. The end point of the titration is the first permanent color change.

-Sodium hydroxide, Phenolphthalein solution, KHP, Pipette, 10 ml graduated cylinder, large beaker, medium beaker, 25mL volumetric flask, Distilled water, stopper, 10mL burette, ring stand, clamp, analytical balance scale, 25mL Erlenmeyer flask, weighing paper. Method:

A pipette was used to place 10 drops of 6N NaOH solution into a 25mL volumetric flask. The NaOH was then diluted by adding carbon dioxide-free distilled water to the 25mL mark. A 10mL burette was then put clamped onto a ring stand in vertical position. The burette was then rinsed with 1mL portion of the NaOH solution that was prepared in step one. The burette was then filled with a pipette to the zero...
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