USING ENGLISH TO REPORT

I.                   Title of Experiment
Acid Base Titration

II.                 Date And Time
Monday, April 17, 2017

III.              Research Purposes
1. Knowing the acid-base penetration by titration method
2. Determine the concentration of an acid or base solution by using acid titration
    Bases
3. Knowing the equivalence and end points of titration-base

IV.  Basic Theory

Titration is a method to determine the content of a substance by using another substance that has been determined by its concentration. Titration is usually distinguished by the type of reaction involved in the titration process, for example when it involves an acid-base reaction, it is referred to as acid-base titration, redox titration for titration involving oxidation-reduction reactions, a titration of complexometry for titration involving complex reaction formation and so forth. (Here only discussed about acid-base titration)

Substances to be determined are referred to as "titrant" and are usually placed in the Erlenmeyer, whereas the known substances are referred to as "titers" and are usually placed in a "burette". Both titer and titrant are usually solvents.

Titration Acid base principles

 Acid base titration involves both acid and base as titer or titrant. Acid base titration based on neutralizing reaction. The acid solution is determined by using an alkaline solution and vice versa.

Titrant is added titer bit by bit until it reaches the equivalent state (meaning the titrant stoichiometry and the right titer runs out). This is called the "equivalent point".

At this point of equivalence the titration process is stopped, then we record the volume of titer required to reach that state. By using titrant volume data, volume and concentration of titer we can calculate titrant level.

How to Know the Equivalent PointThere are two general ways to determine the equivalence point of acid-base titration.

1. Use pH meter to monitor pH change during titration, then plot between pH and titrant volume to obtain the titration curve. The midpoint of the titration curve is the "equivalent point".
2. Use acid-base indicator. The indicator is added to the titrant before the titration process is performed. This indicator will change color when the equivalent point occurs, at which point we stop the titration.

In general the second way is chosen due to the ease of observation, no additional tools required, and very practical. The indicator used in acid-base titration is an indicator whose color is affected by pH. The addition of the indicator is kept as little as possible and generally is two to three drops.

Indicator	Color Change		Solvent
	Acid	Bases
Thimol blue	Red	Yellow	Water
Yellow Methyl	Red	Yellow	Ethanol 90%
Orange Methyl	Red	Red-orange	Water
Red Methyl	Red	Yellow	Water
Bromtimol blue	Yellow	Blue	Water
Phenolphthalein	Not colored	Purple	Ethanol 70%
Thimolftalein	Not colored	Blue	Ethanol 90%

 
 

Acommonly used indicator of acid-base titration is the phenolphthalein indicator. The following table is a characteristic of the phenolphthalein indicator.

PH	< 0	0−8.2	8.2−12.0	>12.0
conditions	Very acidic	Acid or near Neutral	Bases	Very Bases
Color	Orange	Not colored	Purple Pink	Not colored
Picture

 

To obtain the accuracy of the titration result, the titration end point is chosen as close as possible to the equivalent point, this can be done by selecting the appropriate indicator and in accordance with the titration to be performed. The circumstance in which titration is stopped by seeing the indicator color change is referred to as the "end point of the titration".
Acid base titration is divided into 5 types:

1.

1.    Strong acids - Strong bases

2.    Strong acid - weak base

3.    Weak acid - Strong base

4.    Strong acids - Salt of weak acids

5.    Strong base - Salt of weak base

1.      Titration of Strong Acids - Strong Bases

Example:
- Strong acids: HCl
- Strong base: NaOH

Reaction Equation:
HCl + NaOH → NaCl + H2O
The ionic reaction:
H + + OH- → H2O
Strong Acid Base Acid Titration Curve

2.      Titration of Strong Acids - Weak Bases
Example:
- Strong acids: HCl
- Weak base: NH4OH
Reaction Equation:
HCl + NH4OH → NH4Cl + H2O
The ionic reaction:
H + + NH4OH → H2O + NH4 +
Strong Acid Titration Curve - Weak Base

3.      Weak Acid Titration - Strong Bases
Example:
- Weak acid: CH3COOH
- Strong base: NaOH
Reaction Equation:
CH3COOH + NaOH → NaCH3COO + H2O
The ionic reaction:
H + + OH- → H2O
Weak Acid Titration Curve - Strong Base

4.      Titration of Strong Acid - Salt of Weak Acid
Example:
- Strong acids: HCl
- Salt of weak acid: NH4BO2
Reaction Equation:
HCl + NH4BO2 → HBO2 + NH4Cl
The ionic reaction:
H + + BO2- → HBO2

5.      Titration of Strong Bases - Salt of Weak Bases
Example:
- Strong base: NaOH
- Salt of weak base: CH3COONH4
Reaction Equation:
NaOH + CH3COONH4 → CH3COONa + NH4OH
The ionic reaction:
OH- + NH4- → NH4OH

 

General Titration Formulas

At the point equivalent point, the mol-equivalent acid will be equal to the base mol-equivalent, so we can write as follows:

Mol-equivalent acid = mol-equivalent base

The mol-equivalent is obtained from the multiplication of Normality with volume then the above formula can we write as:

NxV acid = NxV base

Normality is obtained from the multiplication of molarity (M) with the amount of H + ions on the acid or the amount of OH ions in the base, so the above formula becomes:

NxMxV acid = nxVxM bases
information :
N = Normality
V = Volume
M = Molarity
N = number of H + ions (on acid) or OH - (on base)

IV.    Tools And Materials
Tool:
• Measuring cup
• Erlenmeyer pumpkin
• Beaker
• Buret
• Stative and clamps
• Funnel
• Drop pipette
• Cleaning brush

INGREDIENTS:
• 0.1 M HCl solution
• 0.1 M CH3COOH solution
• NaOH solution
• PP solution

V.      WAYS OF WORKING:

1.      Prepare a stative burette and clamps

2.      Filling the burette with NaOH solution right up to the zero line with the help of the funnel

3.     Insert 15 ml of 0.1 M HCl into the erlenmeyer flask, then add 3 drops of PP indicator to the  solution

4.    Lay the erlenmeyer flask just below the burette, then open the burette faucet slowly so that NaOH can drip into the solution.

5.    During addition of NaOH, wiggle the erlenmeyer flask so that the NaOH can be well blended and until the earliest color changes occur.

6.      Observe the color changes that occur in HCl solution.

7.      Recording the amount of NaOH used is the difference between the final volume and the initial volume of NaOH.

8.      Determining the concentration of NaOH used with the formula V1.M1 = V2.M2

9.     Perform 1-7 activities once again and calculate the average amount of NaOH used to know the equivalent point

10.  Repeat activities 1-9 for 0.1 M CH3COOH solution

VI.    Discussion

A. Table Of Observation Results

No	Solution	Trial to-	Volume of NaOH Used (mL)		Color of solution
1	HCl + PP + NaOH	1	28 drops = 1,4 ml		Purple to pink-pink an
2	HCl + PP + NaOH	2	33 drops = 1,65 ml		Young purple
3	HCl + PP + NaOH	3	20 drops = 1 ml		Old purple
4	HCl + PP + NaOH	4	28 drops = 1,4 ml		Young purple
5	HCl + PP + NaOH	5	34 drops = 1,7 ml		Pink
6	HCl + PP + NaOH	6	33 drops = 1,65 ml		Pink
7	HCl + PP + NaOH	7	67 drops =  3,35 ml		Purple Pink
8	HCl + PP + NaOH	8	27 drops = 1,35 ml		Purple Pink

 

No	Solution	Trial to-	Volume of NaOH Used (mL)	Color of solution
1	CH3COOH + PP + NaOH	1	58 drops = 2,9 ml	Pink
2	CH3COOH + PP + NaOH	2	59 drops = 2,95 ml	Pink
3	CH3COOH + PP + NaOH	3	49 drops = 2,45 ml	Young purple
4	CH3COOH + PP + NaOH	4	52 drops = 2,6 ml	Pink
5	CH3COOH + PP + NaOH	5	41 drops = 2,05 ml	Pink purple
6	CH3COOH + PP + NaOH	6	55 drops = 2,75 ml	Pink purple
7	CH3COOH + PP + NaOH	7	34 drops = 1,7 ml	Pink purple
8	CH3COOH + PP + NaOH	8	33 drops = 1,65 ml	Pink purple

VI.    Discussion

       Titration is an analytical way of measuring the amount of solution needed to react constantly with a substance present with another solution. In this experiment we determined the molarity of NaOH by using a titration process between 15 ml 0.1 M HCl solution with NaOH solution. 15 ml of HCl solution was put into Erlenmeyer flask and then added 3 drops of PP indicator, then dropped with NaOH solution already provided in buret dropwise until equivalent or finished reacting. Similarly, titration between CH3COOH solution of 15 ml 0.1 M with NaOH solution. 15 ml of CH3COOH solution was put into Erlenmeyer flask and then added 3 drops of PP indicator, then dropped with NaOH solution which had been provided in buret dropwise until equivalent or finished reacting.

       The equivalent point can be known with the help of PP solution, the color range is not colored to purple, ie if colorless means acidic and if purple is a base. If the solution is equivalent then, the solution will experience the earliest discoloration, and the color is very young and bright when that titration is stopped. When the solution shows the earliest discoloration is the so-called end point of the titration.

Experiment 1 uses HCl

Titration strong acid + strong base

In our titration experiments on 15 ml of HCl solution titrated with NaOH yielded the following reaction equations;

HCl + NaOH à NaCl + H2O

Titration 1

In the first experiment, the first step was HCl 15 ml 0.1 M inserted into Erlenmeyer glass, then added 3 drops of penoftaline. 50 ml NaOH is fed into the burette, then let drip dropwise until the indicator changes color or the end point of the titration is reached, and the titration volume is 1.4 ml and the color is purple pink

1.4 M = 1.5

Titration 2

HCl 15 ml 0.1 M was inserted into Erlenmeyer glass, then added 3 drops of penoftaline. 50 ml of NaOH is fed into the burette, then let drip dropwise until the indicator changes color or the end point of the titration is reached, and the titration is obtained at 1.65 ml and the color is purple.
15.0.1 = 1.65 M2
1.5 = 1.65 M2

Titration 3

HCl 15 ml 0.1 M was inserted into Erlenmeyer glass, then added 3 drops of penoftaline. 50 ml NaOH is fed into the burette, then let drip dropwise until the indicator changes color or the end point of titration is reached, and the titration volume is 1 ml and the color is purple.

15.0,1 = 1 M2
1.5 = 1 M2

Titration 4

HCl 15 ml 0.1 M was inserted into Erlenmeyer glass, then added 3 drops of penoftaline. 50 ml NaOH is fed into the burette, then let drip dropwise until the indicator changes color or the end point of the titration is reached, and the titration volume is 1.4 ml and the color is purple pink.

15.0.1 = 1.4 M2
1.5 = 1.4 M2

Titration 5

HCl 15 ml 0.1 M was inserted into Erlenmeyer glass, then added 3 drops of penoftaline. 50 ml NaOH is fed into the burette, then let drip dropwise until the indicator changes color or the end point of the titration is reached, and the titration volume is obtained at 1.7 ml and the color is pink / pink.

15.0.1 = 1.7 M2
1.5 = 1.7 M2

Titration 6

HCl 15 ml 0.1 M was inserted into Erlenmeyer glass, then added 3 drops of penoftaline. 50 ml NaOH is fed into the burette, then let drip dropwise until the indicator changes color or the end point of the titration is reached, and the titration volume is found at 1.65 ml and the color is pink / pink.

15.0.1 = 1.65 M2
1.5 = 1.65 M2

Titration 7

HCl 15 ml 0.1 M was inserted into Erlenmeyer glass, then added 3 drops of penoftaline. 50 ml of NaOH is fed into the burette, then let drip dropwise until the indicator changes color or the

end point of the titration is reached, and the titration volume is 3.35 ml and the color is purple pink.

15.0.1 = 3.35 M2
1.5 = 3.35 M2

Titration 8

HCl 15 ml 0.1 M was inserted into Erlenmeyer glass, then added 3 drops of penoftaline. 50 ml NaOH is fed into the burette, then let drip dropwise until the indicator changes color or the end point of the titration is reached, and the titration volume is obtained at 1.35 ml and the color is purple pink.

15.0.1 = 1.35 M2
1.5 = 1.35 M2

The molarity of NaOH is:

So the molarity of NaOH is 0.99

Experiment 2 uses CH3COOH

Titration of weak acid + strong base

In our titration experiments on 15 ml of CH3COOH solution titrated with NaOH yielded the following reaction equations;

CH3COOH + NaOH     NaCH3COO + H2O

Titration   1

CH3COOH 15 ml 0.1 M was put into Erlenmeyer glass, then added 3 drops of penoftaline. 50 ml NaOH is fed into the burette, then let drip dropwise until the indicator changes color or the end point of the titration is reached, and the titration volume is 2.9 ml and the color is pink.

2.9 M = 1.5

Titration 2

CH3COOH 15 ml 0.1 M was put into Erlenmeyer glass, then added 3 drops of penoftaline. 50 ml NaOH is fed into the burette, then let drip dropwise until the indicator changes color or the end point of the titration is reached, and the titration volume is 2.95 ml and the color is pink.

15.0.1 = 2.95 M2
1.5 = 2.95 M2

Titration 3

CH3COOH 15 ml 0.1 M was put into Erlenmeyer glass, then added 3 drops of penoftaline. 50 ml NaOH is fed into the burette, then let drip dropwise until the indicator changes color or the end point of the titration is reached, and the titration volume is 2.45 ml and the color is purple.

15.0.1 = 2.45 M2
1.5 = 2.45 M2

Titration 4

CH3COOH 15 ml 0.1 M was put into Erlenmeyer glass, then added 3 drops of penoftaline. 50 ml of NaOH is fed into the burette, then let drip dropwise until the indicator changes color or the end point of the titration is reached, and the titration is 2.6 ml and the color is pink.

15.0.1 = 2.6 M2
1.5 = 2.6 M2

Titration 5

CH3COOH 15 ml 0.1 M was put into Erlenmeyer glass, then added 3 drops of penoftaline. 50 ml of NaOH is fed into the burette, then let drip dropwise until the indicator changes color or the end point of the titration is reached, and the titration volume is 2.05 ml and the color is purple pink.

15.0.1 = 2.05 M2
1.5 = 2.05 M 2

Titration 6

CH3COOH 15 ml 0.1 M was put into Erlenmeyer glass, then added 3 drops of penoftaline. 50 ml of NaOH is fed into the burette, then let drip dropwise until the indicator changes color or the end point of the titration is reached, and the titration volume is 2.75 ml and the color is purple pink.

15.0.1 = 2.75 M2
1.5 = 2.75 M2

Titration 7

CH3COOH 15 ml 0.1 M was put into Erlenmeyer glass, then added 3 drops of penoftaline. 50 ml of NaOH is fed into the burette, then let drip dropwise until the indicator changes color or the end point of the titration is reached, and the titration volume is obtained at 1.7 ml and the color is purple pink.

15.0.1 = 1.7M2
1.5 = 1.7 M2

Titration 8

CH3COOH 15 ml 0.1 M was put into Erlenmeyer glass, then added 3 drops of penoftaline. 50 ml NaOH is fed into the burette, then let drip dropwise until the indicator changes color or the end point of the titration is reached, and the titration volume is obtained at 1.65 ml and the color is purple pink.

15.0.1 = 1.65 M2
1.5 = 1.65 M2
The molarity of NaOH is:
So the molarity of NaOH is 0.662 M

In this experiment we performed titration eight times each, a strong acid titration with a strong base eight times and a weak acid titration with a strong base of guard eight times. In the eight experiments on the titration of HCl with NaOH there are some that fail where the color change is too old as well as in the titration of CH3COOH with NaOH. However, there are also some who succeed.

This failure is due to several factors:

1.    Less careful eye when paying attention to the color changes that occur, which may be the initial color changes have occurred but because it is not paid attention carefully so that the penetration is continued and the resulting color is too concentrated and conspicuous

2.    Less careful when carrying out the titration proces

3.    Less precisely the preparation of 0.1 M HCl and CH3COOH in the weighing process.

4.    Less precise in the calculation of droplets of NaOH solution that allows excessive penetrations so that the resulting color more concentrated

5.     At the time of almost reaching the equivalent point of buret faucet flow

 

VI.   Conclusion

1.    The equivalent point is the point where the acid concentration is equal to the base concentration (depleted reacting) or the point at which the amount of base added is equal to the amount of neutralized acid accompanied by the indicator color change.

2.    The end point of the titration is the state where the titration is stopped by looking at the indicator color change

3.    The PP indicator needs to be added to the solution because it knows the color change that occurs at the equivalence point

4.    The reaction equations for each experiment:

A. Strong acid + strong base

HCl + NaOH     NaCl + H2O

B. Weak acid + strong base

CH3COOH + NaOH      NaCH3COO + H2O M

VII.Bibliography

Www.isolabgmbh.com/product.asp%3...rup%3D19
Www.indigo.com/glass/gphglass/buret.html
Www.daym.gov.tr/index2.php%3Fad%...kat%3D57www.analisateknisia.blogspot.com/20 11 ... ive.html www.oldprint.blogspot.com/20 11/12 / pe. ..int.html

Www.try4know.co.cc/20 11 / 12/gelas...mia.html

Www.an89.wordpress.com/20 11 /03/2...am-basa/

Http://kimia.upi.edu/utama/bahanajar/kuliah_web/20011/SRIYANI(050679)/latihan.html
Http://kimia.upi.edu/utama/bahanajar/kuliah_web/2011/Sri%20Ratisah%20054828/materi.HTMhttp://akhitochan.wordpress.com/201 1/02/13 / titration-acid-base /

VIII.       Attachment