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Bilal & Mohanad

The document outlines a chemistry lab experiment focused on acid-base titrations, specifically the preparation and standardization of 0.1N HCl and NaOH solutions. It includes detailed procedures for diluting concentrated HCl and standardizing both HCl and NaOH using Na2CO3 as a primary standard. The document also discusses the calculations involved in determining the normality of the solutions used in the experiment.

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Othman Laith
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29 views6 pages

Bilal & Mohanad

The document outlines a chemistry lab experiment focused on acid-base titrations, specifically the preparation and standardization of 0.1N HCl and NaOH solutions. It includes detailed procedures for diluting concentrated HCl and standardizing both HCl and NaOH using Na2CO3 as a primary standard. The document also discusses the calculations involved in determining the normality of the solutions used in the experiment.

Uploaded by

Othman Laith
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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Al-Hadbaa University

Ministry of Higher
College-Nineveh
Education and
Department of Medical
Scientific Research-
laboratories techniques
IRAQ
2020 - 2021
STAGE ONE

Chemistry

Supervised: Dr. Reem Abed Al-


Luhaiby

By Students:
1. Bilal Ayad Abdulilah (G: D)
2. Mohanad Abd Al-muniem Fathi (G: F)

Chemistry 1
Acid-Base Titrations

Preparation and Standardization of


an acid and a base
:A) Preparation of 0.1N HCl from concentrated HCl

d=1.18 ,Eq.wt=36.5 ,%=37% Therefore: N of


concentrated HCl = 12

Chemistry 2
To calculate the volume of concentrated HCl that
:can be taken to prepare 250 ml of 0.1 N HCl
N1 V1 of conc. HCl = N2 V2 of diluted HCl N1
V1=0.1×250 → V1=2.08ml
Should be taken from concentrated HCl and should
be diluted with distilled water in 250 ml volumetric
. lask to obtain 0.1 N HCl
B) Standardization of prepared of 0.1 N HCl
:solution
1) Fill the burette with the prepared HCl solution
2) Transfer 10 ml of exactly 0.1N Na2CO3 (primary
standard) into conical lask by using a bulb pipette.
(0.1 N Na2CO3 solution is prepared by weighing
exactly 5.3 g of Na2CO3 and diluted to 1000 ml
.with distilled water in a volumetric lask)
3) Add 2 drops of methyl orange as an indicator
.Yellow color is obtained
4) Titrate with HCl solution drop by drop from the
burette into the conical lask until a faint orange
.color is obtained
5) The exact normality of HCl can be calculated
.from the following equation

Chemistry 3
f
f
f
f
Na2CO3 + 2HCl → 2NaCl + H2O + CO2 N1 V1
ofNa2CO3 ≡ N2 V2 ofHCl
C) Determination of the Normality of 0.1 N NaOH
:solution
:I.Preparation of a ≈ 0.1 N NaOH
Weigh 4 g of NaOH dissolve and dilute to one liter
.with distilled water
:II.Standardization of ≈ 0.1 N NaOH
1) Transfer 10 ml of standard HCl solution to a.
..conical lask
2)Add 1-2 drops of phenolphthalein (Ph.Ph.) as an
indicator.
3) Fill the burette with the prepared NaOH solution.
Add NaOH drop by drop into the conical lask.4
until the color of the solution is faint pink
The exact normality of NaOH is obtaind from:.
HCl+NaOH →NaCl+H2O
N1 V1 ofNaOH ≡ N2 V2 ofHCl

Chemistry 4
f
f
Discussion:

A bottle of concentrated HCl has the


following information on its label:
M.wt = 36.5 , d = 1.18 and 40% HCl (w/
w).

The normality of this solution is:

Chemistry 5
N of current concentrated HCL = 12.9 N

If we want to prepare 500 mL of 0.1 N from this


concentrated HCL we have to do that
= −→ . × = . ×

V1= 3.87 mL of this concentrated HCL we have


to add to 500 ml of D.W to prepare 0.1 N HCL.

* Normality(N): It is de ined as the number of


equivalents of a solute present in on liter of
solution.
*Titrations : the process of gradually adding a
standard solution from a burette to the material
whose concentration is to be found to complete
the reaction and reach the end point.

Chemistry 6
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