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Conc. H2so4

This guide outlines the procedure for determining the strength of concentrated H2SO4 using standard 0.1N NaOH through titration. It includes details on the necessary apparatus, preparation of dilute H2SO4, titration steps, calculations for normality, and important safety precautions. Key considerations for accurate results are also highlighted, such as proper dilution and endpoint detection.

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136 views2 pages

Conc. H2so4

This guide outlines the procedure for determining the strength of concentrated H2SO4 using standard 0.1N NaOH through titration. It includes details on the necessary apparatus, preparation of dilute H2SO4, titration steps, calculations for normality, and important safety precautions. Key considerations for accurate results are also highlighted, such as proper dilution and endpoint detection.

Uploaded by

Kb
Copyright
© © All Rights Reserved
We take content rights seriously. If you suspect this is your content, claim it here.
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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 concentrated H2SO4

using standard 0.1N NaOH, incorporating the best aspects of previous responses and
addressing potential issues:
Aim:
To determine the strength (normality) of concentrated H2SO4 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.
● H2SO4 is a diprotic acid: It releases two H+ ions per molecule.
Apparatus and Reagents:
● Burette (50 mL)
● Pipette (25 mL)
● Conical flask (250 mL)
● Burette stand and clamp
● Concentrated H2SO4
● Standard 0.1N NaOH solution
● Phenolphthalein indicator
Procedure:
1. Preparation of dilute H2SO4:
○ Dilute 10 mL of concentrated H2SO4 to 1000 mL in a volumetric flask using distilled
water. This dilution significantly reduces the concentration for safer handling and
accurate titration.
2. 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 H2SO4:
■ Pipette out 25 mL of dilute H2SO4 into a conical flask.
■ Add 2-3 drops of phenolphthalein indicator.
■ Fill the burette with standard 0.1N NaOH solution.
■ Titrate the H2SO4 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 H2SO4:
Normality of H2SO4 = (Normality of NaOH × Volume of NaOH used) /
Volume of H2SO4 taken

● Convert the normality of the dilute H2SO4 to the concentration of the original
concentrated H2SO4 using the dilution factor.
Precautions:
● Always add acid to water, not water to acid, to avoid splashing and heat generation.
● Wear gloves and eye protection when handling concentrated H2SO4.
● 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
concentrated H2SO4 using standard 0.1N NaOH.

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