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Dil. HCL

This document provides a comprehensive guide for determining the strength of dilute hydrochloric acid (HCl) using a standard 0.1N sodium hydroxide (NaOH) solution through titration. It outlines the aim, theory, apparatus, procedure, calculations, and precautions necessary for accurate results. Key steps include standardizing NaOH, performing titrations with HCl, and calculating the normality of HCl based on the volume of NaOH used.

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70 views1 page

Dil. HCL

This document provides a comprehensive guide for determining the strength of dilute hydrochloric acid (HCl) using a standard 0.1N sodium hydroxide (NaOH) solution through titration. It outlines the aim, theory, apparatus, procedure, calculations, and precautions necessary for accurate results. Key steps include standardizing NaOH, performing titrations with HCl, and calculating the normality of HCl based on the volume of NaOH used.

Uploaded by

Kb
Copyright
© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
Available Formats
Download as PDF, TXT or read online on Scribd
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Here's a comprehensive guide on the determination of the strength of dilute hydrochloric acid

(HCl) using standard 0.1N NaOH solution:


Aim:
To determine the strength (normality) of dilute HCl using standard 0.1N NaOH solution through
titration.
Theory:
● Normality (N): Number of gram equivalents of a solute present in one liter of solution.
● Equivalent weight: Molecular weight of a substance divided by its valency.
● HCl is a monoprotic acid: It releases one H+ ion per molecule.
Apparatus and Reagents:
● Burette (50 mL)
● Pipette (25 mL)
● Conical flask (250 mL)
● Burette stand and clamp
● Dilute HCl
● Standard 0.1N NaOH solution
● Phenolphthalein indicator
Procedure:
1. Titration:
○ Standardization of NaOH: If the exact normality of the NaOH solution is uncertain,
standardize it using a primary standard like oxalic acid or potassium hydrogen
phthalate.
○ Titration of HCl:
■ Pipette out 25 mL of dilute HCl into a conical flask.
■ Add 2-3 drops of phenolphthalein indicator.
■ Fill the burette with standard 0.1N NaOH solution.
■ Titrate the HCl solution with NaOH until a faint pink color persists for 30
seconds.
■ Record the initial and final burette readings.
■ Repeat the titration two more times to obtain consistent results.
Calculations:
● Calculate the average volume of NaOH used in the three titrations.
● Use the following formula to calculate the normality of HCl:
Normality of HCl = (Normality of NaOH × Volume of NaOH used) /
Volume of HCl taken

Precautions:
● Always add acid to water, not water to acid, to avoid splashing and heat generation.
● Wear gloves and eye protection when handling acids.
● Work in a well-ventilated area.
Additional Considerations:
● The dilution factor should be chosen such that the titration volume is within the accurate
range of the burette.
● The endpoint detection should be sharp and clear.
● The burette and pipette should be rinsed with the respective solutions before use.
● The conical flask should be rinsed with distilled water before each titration.
By following these steps and precautions, you can accurately determine the strength of dilute
HCl using standard 0.1N NaOH.

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