Preparation and Standardization of a Sodium Hydroxide Solution Essay Sample

August 6, 2017 History

Objective/Purpose: The aim of this experiment will be the standardisation of Na hydrated oxide utilizing K H phthalate by the titration method. Introduction:
The concentration of solutions can be reported in footings of molar concentration and normalcy. Molarity is equal to: HCL. HBR. H2SO4. HNO3
M = mol Solute ( mol ) ( Monoprotic ) ( Diprotic )

V ( L ) g solutions ( L )

M = __N___ for Monoprotic acids molar concentration = normalcy molar mass V

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One molar solution can be prepared by fade outing the mass of 1 mole of the peculiar substance in adequate H2O to do a 1L solution.

HCL + NaOH ? H2O + NaCl

H2SO4 + NaOH ? H2O + Na2SO4

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

To execute an acid-base neutralisation utilizing the titration technique to find the concentration ( normalcy ) of the NaOH prepared in portion A.

C8H5O4K + NaOH? H2O + KC8H4O4Na


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

*Phenolphthalein- colorless in acid and pink in base. The terminal point of the titration is the first lasting colour alteration.

-Sodium hydrated oxide. Phenolphthalein solution. KHP. Pipette. 10 milliliter graduated cylinder. big beaker. medium beaker. 25mL volumetric flask. Distilled H2O. stopper. 10mL burette. pealing base. clinch. analytical balance graduated table. 25mL Erlenmeyer flask. weighing paper. Method:

A pipette was used to put 10 beads of 6N NaOH solution into a 25mL volumetric flask. The NaOH was so diluted by adding C dioxide-free distilled H2O to the 25mL grade. A 10mL burette was so put clamped onto a ring base in perpendicular place. The burette was so rinsed with 1mL part of the NaOH solution that was prepared in measure one. The burette was so filled with a pipette to the nothing grade with NaOH.

0. 3000 to 0. 4000 gm of K H phthalate ( KHP ) was used as a beginning for the experiment. A piece of weighing paper was so weighed on the analytical balance graduated table. 0. 0700 to 0. 0800g of KHP was placed onto the paper and was so weighed once more. The KHP crystals were so transferred to 3. 25mL Erlenmeyer flask’s. 10mL of C dioxide-free distilled H2O was added to each flask and was swirled gently to fade out all the KHP crystals. 2-3 beads of phenolphthalein were added to all 3 flasks.

The initial volume of the burette was taken down before get downing the experiment. The KHP acerb solution was so titrated utilizing the NaOH solution prepared in measure one bead by bead. The titration stopped when the solution turned for good pink. The concluding volume was so recorded for test one. This process was so repeated two more times for the remainder of the tests. With the information obtained. the normalcy of the NaOH solution was so calculated.

Consequences: See affiliated informations sheet

After carry oning the experiment we were able to execute an acid-base neutralisation utilizing the titration technique to find the concentration ( normalcy ) of the NaOH prepared in portion A. After ciphering the normalcy we noticed that values of the 3 tests was a spot greater than 10 % . Some mistakes that we may take into history are user mistake. Possibly when adding the NaOH solution to the acid. we may hold added excessively much beads and therefore got a darker pink colour. Another mistake that we may hold encountered is non halting the dropper up to the semilunar cartilage. These are some mistakes that may hold altered our consequences.


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