REPORT of chemistry statement
Titration of NaOH 0,1 M and CH3COOH
COMPILED BY:
AHMAD MUHAEMIN
XI SCIENCE 1
01
SMA Negeri 2 kota Cirebon
Jalan Dr. Cipto Mangunkusumo No.1 Cirebon Telepon (0231) 203301 Fax. (0231)
239814
Chemistry Report
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A. Purpose
Determine the concentration of CH3COOH
B. Basic Theory
1) Understanding
1. Arrhenius Theory
Svante Arrenhius (1857-1927)
Arrenhius proposed in his doctoral thesis (1883) that ionic compounds dissociate and
can become free ions acting as separate entities in solution. Faraday had assumed ions
were produced only during electrolysis and required an electric current. Due to his
revolutionary theory, Arrenhius received low rating for his dissertation (he was awarded
Nobel Prize in 1903 for this work).
ACID: Substance that produces H+1 in water.
BASE: Substance that produces OH-1 in water.
HCl(aq)
H+1 + Cl-1
produces H+1 in water
+1
-1
NH3(aq)
NH4 + OH produces OH-1 in water
Although NH3 does not contain OH-1, hydroxide ions form when added to water.
Arrhenius acid and base neutralize each other to produce salt and water:
HCl(aq) + NaOH(aq)
NaCl(aq) + H20(l)
+1
-1
H (aq) + OH (aq)
H20(l)
Arrenhius theory most limited of the three theories since it requires reactions be aqueous
and applies only to substances producing H3O+1 or OH-1.
2. Bronsted/Lowry Theory
Johannes Bronsted (1879-1947)
Thomas Lowry (1874-1936)
In 1923, Bronsted (Danish) and Lowry (English) published independent papers on the same
subject. Unlike the Arrenhius theory, their approach was not limited to aqueous solutions
but for all proton (H+) containing systems.
ACID: Substance that can donate proton (H+1).
BASE: Substance that can accept proton (must contain lone pair of electrons).
Acids may be cations, neutral molecules, or anions, while bases may be anions or
neutral molecules. Just as a reduction must always accompany an oxidation, a proton donor
(acid) must accompany a proton acceptor (base). Once an acid transfers its proton it
becomes the conjugate base (CB) and once a base accepts the proton it becomes the
conjugate acid (CA). Since protons are always transferred in the Arrenhius concept, all
Arrhenius acid/base reactions are also Bronsted-Lowry acid/base reactions.
But if water is not involved (HCl & NH3), the reaction can be explained by Bronsted/Lowry
concept and not Arrenhius. (Some remarks on the concept of acids and bases by Bronsted).
HCl + NH3
NH4+1 + Cl-1
acid base
CA
CB
Bronsted/Lowry expands Arrenhius to include any proton transfer (water not requirement).
3. Lewis Theory
Gilbert Lewis (1875-1946)
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Just as the Arrenhius theory did not support observations of acid-base behavior in
nonaqueous systems, the Bronsted-Lowry model excluded nonprotonated systems. Lewis
suggested his theory in a 1923 book "Thermodynamics and the Free Energy of Chemical
Substances" and fully developed the theory in 1938.
ACID: Substance that can accept a pair of electrons from another atom to form a new bond.
BASE: Substance that can donate a pair of electrons to another atom to form a new bond.
The product of Lewis acid-base reaction referred to as adduct. The proton itself can act as
Lewis acid. Lewis expands acid/base reactions to include many substances without H in
formula.
F3B + :NH3
F3B:NH3
Explained by Lewis but not Arrenhius or BL
acid base
adduct
All Bronsted/Lowry acid/base reactions are also Lewis acid/base reactions.
That’s some example of acid base
HI + H2O
H3O+1 + I-1 Explained by all 3 theories
HI + NH3
NH4+1 + I-1 Explained by BL & Lewis
I2 + NH3
NH3I+1 + I-1 Explained by Lewis
I2 + Cl
ICl + I
Cannot be explained by any of the theories
X:-1 + Y+1
Y:X
Explained by Lewis but not Arrenhius or BL
H2 + Cl2
2HCl
Cannot be explained by any of the theories
2) Acid-Base Character
For a molecule with a H-X bond to be an acid, the hydrogen must have a positive
oxidation number so it can ionize to form a positive +1 ion. For instance, in sodium hydride
(NaH) the hydrogen has a -1 charge so it is not an acid but it is actually a base. Molecules
like CH4 with nonpolar bonds also cannot be acids because the H does not ionize. Molecules
with strong bonds (large electronegativity differences), are less likely to be strong acids
because they do not ionize very well. For a molecule with an X-O-H bond (also called an
oxoacid) to be an acid, the hydrogen must again ionize to form H+. To be a base, the O-H
must break off to form the hydroxide ion (OH-). Both of these happen when dealing with
oxoacids.
Strong Acids: These acids completely ionize in solution so they are always represented in
chemical equations in their ionized form. There are only seven (7) strong acids:
HCl, HBr, HI, H2SO4, HNO3, HClO3, HClO4
To calculate a pH value, it is easiest to follow the standard "Start, Change, Equilibrium"
process.
Weak Acids: These are the most common type of acids. They follow the equation:
HA(aq)
H+(aq) + A-(aq)
The equilibrium constant for the dissociation of an acid is known as Ka. The larger the value
of Ka, the stronger the acid.
[H+][A-]
Ka =
[HA]
Strong Bases: Like strong acids, these bases completely ionize in solution and are always
represented in their ionized form in chemical equations. There are only eight (8) strong
bases:
LiOH, NaOH, KOH, RbOH, CsOH, Ca(OH)2, Sr(OH)2, Ba(OH)2
Weak Bases: These follow the equation:
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Weak Base + H2O
conjugate acid + OHexample: NH3 + H2O
NH4+ + OHKb is the base-dissociation constant:
[conjugate acid][OH-]
Kb =
[weak base][H2O]
[NH4+][OH-]
example: Kb =
[NH3[H2O]
Ka x Kb = Kw = 1.00x10-14
To calculate the pH of a weak base, we must follow a very similar "Start, Change,
Equilibrium" process as we did with the weak acid, however we must add a few steps.
3) pH
What is of interest in this reading, however, is the acid-base nature of a substance like
water. Water actually behaves both like an acid and a base. The acidity or basicity of a
substance is defined most typically by the pH value, defined as below:
pH = -log[H+]
Solutions with a pH of seven (7) are said to be neutral, while those with pH values
below seven (7) are defined as acidic and those above pH of seven (7) as being basic.
pOH gives us another way to measure the acidity of a solution. It is just the opposite of pH.
A high pOH means the solution is acidic while a low pOH means the solution is basic.
pOH = -log[OH-]
pH + pOH = 14.00 at 25°C
4) Molarity concentrate
In chemistry, the molar concentration, ci is defined as the amount of a constituent ni
divided by the volume of the mixture V :
It is also called molarity, amount-of-substance concentration, amount concentration,
substance concentration, or simply concentration. The volume V in the definition ci =
ni / V refers to the volume of the solution, not the volume of the solvent. One litre of
a solution usually contains either slightly more or slightly less than 1 litre of solvent
because the process of dissolution causes volume of liquid to increase or decrease.
Units
The SI unit is mol/m3. However, more commonly the unit mol/L is used. A solution of
concentration 1 mol/L is also denoted as "1 molar" (1 M).
1 mol/L = 1 mol/dm3 = 1 mol dm−3 = 1 M = 1000 mol/m3.
An SI prefix is often used to denote concentrations. Commonly used units are listed in the
table hereafter:
Name Abbreviation
Concentration
Concentration (SI unit)
−3
3
millimolar
mM
10 mol/dm
100 mol/m3
micromolar
μM
10−6 mol/dm3
10−3 mol/m3
nanomolar
nM
10−9 mol/dm3
10−6 mol/m3
picomolar
pM
10−12 mol/dm3
10−9 mol/m3
femtomolar
fM
10−15 mol/dm3
10−12 mol/m3
attomolar
aM
10−18 mol/dm3
10−15 mol/m3
zeptomolar
zM
10−21 mol/dm3
10−18 mol/m3
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yoctomolar
yM
10−24 mol/dm3
(1 molecule per 1.6 L)
10−21 mol/m3
5) Ekuivalen
The equivalent (symbol: eq or Eq), sometimes termed the molar equivalent, is a unit of
amount of substance used in chemistry and the biological sciences.
The equivalent is formally defined as the amount of a substance which will either:
 react with or supply one mole of hydrogen ions (H+) in an acid–base reaction; or
 react with or supply one mole of electrons in a redox reaction.[1][2]
The mass of one equivalent of a substance is called its equivalent weight.
A historical definition, used especially for the chemical elements, describes an equivalent as
the amount of a substance that will react with one gram of hydrogen, or with eight grams of
oxygen, or with 35.5 grams (1.25 oz) of chlorine, or displaces any of the three.[3]
In practice, the amount of a substance in equivalents often has a very small magnitude,
so it is frequently described in terms of milliequivalents (mEq or meq), the prefix milli
denoting that the measure is divided by 1000. Very often, the measure is used in terms of
milliequivalents of solute per litre of solvent (or milliNormal, where mEq/L = mN). This is
especially common for measurement of compounds in biological fluids; for instance, the
healthy level of potassium in the blood of a human is defined between 3.5 and 5.0 mEq/L.
6) Indicator pp
Fenolftalin or pp is another indicator of the titration is often used, and
phenolphthalein is a weak acid to another.
In this case, a weak acid is colorless and its ion is bright pink. The addition of
hydrogen ions shifts the equilibrium position to the left, and turn the indicator
colorless. The addition of hydroxide ion removes hydrogen ions from the equilibrium
that leads to the right to replace him - turns the indicator pink.
Half the rate occurs at pH 9.3. Because mixing pink and colorless produces a pale
pink color, it is difficult to detect with accuracy!
7) Titrations
Titrations are not all that hard to understand. In fact, the word "titration" comes from
the Greek titros which means "to figure out the molarity of an acid or base solution" and the
Latin ations which means "by neutralizing it with a solution whose concentration you
already know". Those ancient people really had a way with words.
Here's the idea. Let's say that you had really bad eyes and wanted to see how many
toothpicks you had in a pile. In fact, your eyes are so bad that you can't even see the
toothpicks to pick them up, much less count them accurately. This poses a problem.
Your friend has an idea. You've got a bunch of little sandwiches lying around the
house from the dinner party your parents hosted last night. If your friend sticks one
toothpick into each sandwich, you could figure out how many toothpicks you had because
all you'd need to do is count the number of sandwiches. You wouldn't be measuring the
number of toothpicks directly by counting them, you'd be measuring them secondhand by
how they interacted with something else.
That's what a titration is. Let's say you have an acidic solution and wanted to figure
out the molarity. Well, you can't do that directly, because you can't count acid
molecules. They're too small. You can, however, make a basic solution with a
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concentration that you already know. If you keep adding base to the acid, eventually all of
the acid molecules will be neutralized and the solution will turn from an acid to a base. If
you know how many base molecules you added to the solution before the solution gets
neutralized (and you will, because you'll add the solution drop-by-drop), you can figure out
how much acid was in the solution in the first place.
Of course, this leads to an interesting problem: How can you tell when the solution
gets neutralized? The answer: Indicators! Indicators are chemical compounds that turn
different colors when they're in solutions with different pH's. The indicators you'd most
likely work with turn color when the solution becomes neutralized. Litmus, for example, is
red in acid solutions and blue in basic solutions. Phenolphthalein (pronounced fee-no-thayleen) is clear in acid solutions and pink in basic solutions.
OK. Now that you have the basic idea behind titrations and know what indicators
are, let's figure out how to solve some problems.
The basic equation you need is this:
M 1V 1 = M 2V 2
 M1 stands for the molarity of the acid
 V1 stands for the volume of the acid you use
 M2 stands for the molarity of the base
 V2 stands for the volume of the base you use
 In an acid-base titration, the base will react with the weak acid and form a solution
that contains the weak acid and its conjugate base until the acid is completely gone.
To solve these types of problems, we will use the Ka value of the weak acid and the
molarities in a similar way as we have before. Before demonstrating this way, let us
first examine a short cut, called the Henderson-Hasselbalch Equation. This can only
be used when you have some acid and some conjugate base in your solution. If you
only have acid, then you must do a pure Ka problem and if you only have base (like
when the titration is complete) then you must do a Kb problem.
[base]
pH = pKa + log
[acid]
 Where:
pH is the log of the molar concentration of the hydrogen
pKa is the equilibrium dissociation constant for an acid
[base] is the molar concentration of a basic solution
[acid] is the molar concentration of an acidic solution
Acidimetry and alkalimetri the two different groups of neutralization titration. Acidimetry
and alkalimetry often called the acidimetry titration and alkalimetry titration.
 Acidimetry Titration
Is the titration of an alkaline solution (free base, and a solution of hydrolyzed salt derifed
from weak acids) with a standard solution of acid.
 Alkalimetry Titration
Is the titration of the acidic solution (free acid, and a solution of hydrolyzed salt derived
from weak base) with a standard alkaline solution.
C. equipment and materials
1) Equipments
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1.
2.
3.
4.
5.
6.
7.
Erlenmeyer
Burette
Spatula
pipette mumps 10 ml
flask 250 ml
measuring cup
neraca
2) Materials
1. CH3COOH 10 ml (concentrated)
2. NaOH 1 gram
3. Water
4. Tissue
5. Indikator
6. Pp
D. work steps
1. prepare all equipment and materials
2. for solution NaOH 0,1 M 250 ml
3. dilute CH3COOH (concentrated) as much as 10 times
4. input 10 ml CH3COOH (not concentrated) into erlenmeyer
5. Input NaOH into biuret (25 ml)
6. pp indicator drops into CH3COOH (not contrated)
7. Titration CH3COOH until become tobe pinki permanent
8. Write the final volume when equilibrium
E. Observations
CH3COOH
NaOH
10 ml
45 ml
10 ml
43 ml
10 ml
40 ml
F. Data processing

Need NaOH:
0.1 =
𝑔𝑟 1000
40 250
Gr = 1g

Determining the concentration of CH3COOH (by neutralization formula)
Vacid × Nacid = Vbases × Nbases
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10 × (acid valense × Macid) = 40 × (bases valense × Mbases)
10 × (1 × Macid) = 40 × (1 × 0,1)
Macid = 0,4 M


Determining the concentration of CH3COOH before diluented
V1 . M1 =
V2 . M2
10. M1
=
100 . 0,4
M1
=
4
Determining the percentation of CH3COOH
M=
4=
ρ × % × 10
Mr
1,05 ×10 ×%
60
60 ×4
% = 1,05 ×10
= 22,85 %
G. Conclusion
From the data above , the concentration of acetate acid CH3COOH that we
titrated is 22,85 % or 4 M .
H. Bibliography
Utami, Budi dkk. 2010. Kimia Untuk SMA/MA Kelas XI Program Ilmu Alam.
Jakarta : Pusat Perbukuan Depdiknas
Justiana, Sandri and Muchtaridi. 2009. Chemistry for senior high school. Jakarta :
Yudhistira
www.wikipedia.com
www.chem-is-try.org
www.google.com
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