EXP-NO-( )
Date:……..
Acid - base Titration
Theory:-The concentration of acidic solution may be found by titration with a known
concentration of base solution. The end-point is found by using phenolphthalein as
the acid-base indicator.
-At the endpoint the indicator changes color from pink to colorless.
Equation:HCl + NaOH
NaCl + H2O
Apparatus:25 ml burette
250 ml beakers (2)
250 ml conical flask
Balance wash bottle
Funnel
Pipette
Procedure:- To find the end-point accurately:
- Rinse the burette, pipette and conical flask respectively with distilled water.
- Rinse the burette with sodium hydroxide solution(0.5 M), and rinse the pipette
with hydrochloric solution. Using the pipette, transfer 5.00 cm3 of the unknown
hydrochloride solution into the clean conical flask. Add 3 drops of phenolphthalein
indicator.
- Fill the burette to the 0 cm3 mark with sodium hydroxide solution.
- titrate hydrochloric acid in conical flask against sodium hydroxide in burette.
- Carry out one rough and two accurate titrations.
- Calculate the concentration of the hydrochloric.
Results:Initial volume(ml)
Final volume(ml)
Volume used(ml)
Average
volume=…………………………………………………………………
Calculation:𝑴×𝑽
𝑴×𝑽
𝒏
𝒏
(
)𝒂𝒄𝒊𝒅 = (
𝑴𝒂𝒄𝒊𝒅 ×𝟓𝒎𝒍
𝟏
=
)𝒃𝒂𝒔𝒆
𝟎.𝟓 𝑴 × 𝑽𝒃𝒂𝒔𝒆
𝟏
……………………………………………………………………………
……………………………………………………………………………
…………………………………………………………………………….
…………………………………………………………………………….
Conclusion:We found concentration of hydrochloric acid is ………………………………….
EXP- NO ( )
Date:……...
Density
Theory:-The density of a substance is defined as the mass per unit volume. Mass is usually
measured in g and volume in mL or cm3.
-Density does vary with the temperature of the substance, so it is usually expressed
at 20°C, which is considered to be room temperature.
Equation:Density =
𝑴𝒂𝒔𝒔
𝑽𝒐𝒍𝒖𝒎𝒆
g\cm3
Apparatus:Balance
Beaker (50 and 25 ml)
Pipette 10 ml
Chemicals:Cyclohexane
Procedure:- Weight a clean and dry 25 ml beaker.
- Using 10 ml pipette, pipette exactly 10 ml of the unknown liquid in beaker.
- Weight the beaker and record your result
- Calculation the density.
Results:Volume \ ml
Mass \ g
Calculating:Density =
𝑴𝒂𝒔𝒔
𝒗𝒐𝒍𝒖𝒎𝒆
……………………………………………………………………………
……………………………………………………………………………
…………………………………………………………………………….
Conclusion:Density of cyclohexane was found is …………………………………….
EXP –NO- ( )
Date:……….
Preparation of Aspirin
Theory:- Aspirin is the common name for the compound acetylsalicylic acid, widely used
as a fever reducer and as a pain killer.
- To prepare aspirin, salicylic acid is reacted with an excess of acetic anhydride.
A small amount of a strong acid is used as a catalyst which speeds up the reaction.
In this experiment, phosphoric acid will be used as the catalyst.
-The aspirin product is not very soluble in water so the aspirin product will
precipitate when water is added.
Equation:-
Apparatus:-125 ml conical flask
-10 ml graduated cylinder
-Filter paper
-Beakers
-Funnel
-Balance
Chemicals:-Acetic anhydride
-Salicylic acid
-concentrated sulfuric acid
- -ice
- distilled water
Procedure:-Weight about 3g of salicylic in a 125ml conical flask .
-Add 6ml of acetic anhydride.
-Add five drops of concentrated sulfuric acid.
-Please the flask in beaker of water warmed to 80° to 90°C and heat for 20 mint.
- remove the flask from the hot water and allow it to cool at room temperature.
-Add 40 ml of distilled water to the mixture in the flask.
- cool the mixture in an ice bath to complete the crystallization.
- filter and wash the crystal with a little ice-cold water.
- after aspirin has dried . obtain and record mass.
-calculate the theoretical and percent yield of aspirin ,based on the mass of
salicylic acid used and the mass of product.
Result:Mass of Aspirin = ……………………..g
Calculation:Yield % =
𝒂𝒄𝒕𝒖𝒂𝒍 𝒚𝒊𝒆𝒍𝒅
𝒕𝒉𝒆𝒐𝒓𝒆𝒕𝒊𝒄𝒂𝒍 𝒚𝒊𝒆𝒍𝒅
%
……………………………………………………………………………………….
………………………………………………………………………………………
………………………………………………………………………………………
………………………………………………………………………………………
………………………………………………………………………………………
Calculation:The percentage of Aspirin was found =……………………………………..
Date …………
EXP-NO-( )
Heat of neutralization
Theory:
Difination:
Large concentrations of hydrogen ion and hydroxide ion cannot coexist in
solution, because the neutralization reaction
In this experiment, an aqueous hydrochloric acid solution will be added to an
aqueous sodium hydroxide solution. The neutralization reaction will occur
until either H+ or OH- is entirely consumed. The reactant which is consumed
first is called the limiting reactant.
Equation:
NaOH + HCl  NaCl + H2O
H+ (aq) + OH- (aq) → H2O (l)
Apparatus:- Beakers
- Thermometer
Chemicals:
- Sodium hydroxide (0.1M)
- Hydrochloric acid (0.1M)
Procedure:- Weight clean and dry beakers (m1)
- But in beakers 25ml of hydrochloric acid (0.5M). measured temperature(T1)

Add 25ml of (0.1M) aqueous HCl to 25ml of (0.1M) aqueous NaOH
and weight the beaker (m2).

Measured the temperature of the system before and after the
neutralization reaction occurs (T2).

Calculate the change in temperature for the system(∆T).

Use the temperature change and heat capacities for the calorimeter
and aqueous solution to calculate the heat of neutralization.

Divide the heat of neutralization by the moles of the limiting reactant
to determine heat of neutralization.
Result:m1
m2
T1
T2
Calculation:H  m1 x 1 x (T2  T1 )  m 2 x  2 x (T2  T1 )
qneut
ΔHneut =
n
n=
𝑀×𝑉
1000
(M = 0.1M ,
V = 25ml)
∆H = Heat of neutralization
m1 = mass of calorimeter
m2 = mass of solution ( mass of acid + mass of base)
m2 = v2
p1 = 0.836 J/g. °c
p2 = 4.182 J/g. °c
n = No of mole of water
……………………………………………………………………………
……………………………………………………………………………
……………………………………………………………………………
……………………………………………………………………………
……………………………………………………………………………
……………………………………………………………………………
……………………………………………………………………………
……………………………………………………………………………
……………………………………………………………………………
……………………………………………………………………………
Conclusion:Heat of neutralization for one mol was found equal …………………………..