USING ENGLISH TO REPORT

Report 
pH OF ACIDS BASES AND SALT

CHAPTER I

PRELIMINARY

1.1  Background

In everyday life we ​​have encountered many acids, bases and salts, such as, Sodium Chloride, Sodium Bikarnonate, Acetic Acid, Citric Acid, Sodium Hydroxide, and many more acids, bases and salts that we can find in everyday life . It is therefore imperative that we perform this practice

Acids, bases and salts are the most important chemical groups in everyday life, the solutions are differentiated into three groups: acidic, alkaline and neutral. According to the theory of Arrhenius, a substance in water produces H⁺ ions called acid, while a substance in ionized water produces OH^- ions is a base

Acids and bases can be identified using indicator substances, ie substances that give different colors in acidic environments and alkaline environments (substances whose color may change when interacting or reacting with acidic compounds or basic compounds)

1.2  Experiment Objectives

The purpose of this practice is  :

1.    Determine the pH of the solution with the pH of the universal indicator

2.    Calculate the concentration of the solution with a certain pH value

CHAPTER II

LITERATURE REVIEW

Acids and bases were defined by chemists centuries ago in the properties of their aqueous solutions. In this sense a substance whose acid-based water solution redacts the blue lacmus reacts with the active metal to form hydrogen and neutralize the base. Following a similar pattern a base is defined as a substance whose aqueous solution is bitter and feels slippery in skin (Achmad 1996).

An indicator is a reference agent that distinguishes a solution, an acid or base, or neutral attaches some of the indicators and their changes to a particular pH route, the usefulness of this indicator is to know how much pH is a solution. Besides, it is also used to know the end point of concentration in some organic compounds and inorganic compounds. The acidity or basicity of a substance depends on the presence or absence of H (for acid) and OH (for alkaline) ions in the substance and the degree of ionization of the substance (Pudjaatmaka 1980).

Acid in general is a chemical compound which, when dissolved in water, will produce a solution with a pH less than 7. In the modern definition, acid is a substance that can give protons (H⁺ ions) to other substances (called bases) Free electrons of a base. An acid reacts with a base in the neutralizing reaction to form a salt. Examples of acids are acetic acid (found in vinegar) and sulfuric acid (used in batteries or car batteries). Acids generally taste sour, but highly concentrated acidic liquids can damage the skin and be careful eyes, if splashed acid concentrated can result in blindness. If you get concentrated acid should be washed with running water until completely clean (Syafnil: 2015)

The acid-base indicator is a halochromic compound added in small amounts to the sample, generally a solution which will give the color according to the pH conditions of the solution. At a temperature of 25 ° Celsius, the pH value for the neutral solution is 7.0. Below that value the solution is said to be acid, and above that value the solution is said to be a base. Most organic compounds produced by living things easily release protons (are Lewis Acids), commonly Carboxylic Acids and Amines, so acid-base indicators are widely used in the field of biological chemistry and analytical chemistry. The mechanism of color change by indicator is acid-base reaction, complex formation, and redox reaction (anonym: 2015)

The acid (which is often represented by the general formula HA) is generally a chemical compound which, when dissolved in water, results in a solution with a pH less than 7. In the modern definition, acid is a substance that can give protons (H ⁺ ions) to other substances Called bases), or can accept free electron pairs of a base. An acid reacts with a base in the neutralizing reaction to form a salt. Examples of acids are acetic acid (found in vinegar) and sulfuric acid (used in batteries or car batteries). Acids generally taste sour, but highly concentrated acidic liquids can damage the skin and be careful eyes, if splashed acid concentrated can result in blindness. If you get concentrated acid should be washed with running water until completely clean (Anonym: 2015)

Bases are chemical compounds that absorb hydronium ions when dissolved in water.Basa is opposite of acid, which is intended for elements / chemicals that have a pH of more than 7. Kostik is a term used for strong bases (Anonym: 2015)

Salt is an ionic compound consisting of positive ions (cations) and negative ions (anions), thus forming a neutral compound (without charge). Salt is formed from the reaction of acids and bases (Anonym : 2015)

CHAPTER III

METHODELOGY

3.1 Tools and Materials

1.      Tool

a.    Test tube

b.    Erlenmeyer 50 ml

c.    10 ml measuring pipette

d.   5 ml pipette

e.    Watch glass

f.     The glass funnel

g.    Tube shelf reaction

h.    Ordinary pipette

i.      Universal indicator pH

2.      Materials

a.       HCL

b.      H₂SO₄

c.       HCH₃COO

d.      NaOH

e.       NH₄OH

f.       NaCH₃COO

g.      Boracic Acid

h.      NH₄CL

i.        Na₂SO₃

j.        NaCL

3.2   How it Works

1.    Clean 10 test tubes with detergent and dry

2.    Put on the reaction test rack with the mouth of the tube up

3.    Pipette more or less 2 ml of solution which have been provided to each of the test tube

4.    Determine pH by using universal pH indicator paper

5.    Compute each of the above solutions (in the full report)

CHAPTER IV

RESULTS OF OBSERVATIONS AND DISCUSSIONS

4.1 Observation Results

No	Name of solution	pH	Group	concentration (m)
1	HCL	1	Strong acids	0,1 m
2	H3BO3	5	Weak acid	1
3	Na2SO3	7	Neutral	0,1 m
4	H2SO4	1	Strong acids	0,1 m
5	NaOH	14	Strong base	10
6	NH4CL	5	Weak acids	0,1 m
7	NaCL	7	Neutral	2
8	CH3COO	3	Strong acids	1 m

4.2 Discussion

In the first experiment, dipping the pH of the universal indicator into a glass cup containing the HCL solution, then the pH of the universal indicator changed color and matched with the acidic acid pH tebel. It turns out that HCL has a pH of 1 which means strong acid. And the concentration (molality) = 0.1 m

Molality of PH HCL = 1

PH = - log (H ⁺)

 1 = - log (H ⁺)

H ⁺ = 1 x 10^-1 M

The second experiment, dipping the pH of the universal indicator into the glass of the cup containing the H₃BO₃ solution (boric acid), then the pH of the universal indicator changes color and is matched with the acid-base pH thickness. It turns out that H₃BO₃ (boric acid) has a pH of 5 which means weak acid. And concentration (molality) = 1%

Molality of PH H₃BO₃ = 5

PH = - log (H⁺)

5 = - log (H⁺)

H⁺ = 1 x 10^-5 M

The third experiment, dipping the pH of the universal indicator into a glass cup containing the Na₂SO₃ solution, then the pH of the universal indicator changes color and is matched with the acidic acid pH tebel. It turns out Na₂SO₃ has a pH of 7 which means neutral. And the concentration (molality) = 0.1 m

Molality of PH Na₂SO₃ = 7

 PH = - log (H⁺)

 7 = - log (H⁺)

 H⁺ = 1 x 10^-7 M

The fourth experiment, dipping the pH of the universal indicator into a glass cup containing the H₂SO₄ solution, then the pH of the universal indicator changes color and is matched with the acid-base pH tebel. Apparently H₂SO₄ has a pH of 1 which means strong acid. And the concentration (molality) = 0.1 m

Molality of pH H₂SO₄ = 1

PH = - log (H⁺)

1 = - log (H⁺)

H⁺ = 1 x 10^-1 M

In the fifth experiment, dipping the pH of the universal indicator into the glass of the cup containing the NaOH solution, then the pH of the universal indicator changed color and matched with the acidic acid pH tebel. It turns out that NaOH has a pH of 14 which means a strong base. And concentration (molality) = 10%

Molality of PH NaOH = 14

PH = - log (H⁺)

14 = - log (H⁺)

 H⁺ = 1 x 10^-14 M

In the sixth experiment, dipped the pH of the universal indicator into a glass cup containing the NH₄CL solution, then the pH of the universal indicator changed color and matched with the acidic acid pH tebel. It turns out that NH₄CL has a pH of 5 which means weak acid. And the concentration (molality) = 0.1 m

Molality of pH NH₄CL = 5

PH = - log (H⁺)

 5 = - log (H⁺)

 H⁺ = 1 x 10^-5 M

In the seventh experiment, dipped the pH of the universal indicator into the glass of the cup containing the NaCl solution, then the pH of the universal indicator changed color and matched with the acidic acid pH tebel. It turns out that NaCL has a pH of 7 which means neutral. And concentration (molality) = 2%

Molality of PH NaCL = 7

PH = - log (H⁺)

7 = - log (H⁺)

H⁺ = 1 x 10^-7 M

In the last experiment, dipping the pH of the universal indicator into a trophy glass containing the CH₃COO solution, then the pH of the universal indicator changes color and is matched with the acidic acid pH tebel. It turns out that CH₃COO has a pH of 3 which means strong acid. And concentration (molality) = 1 m

Molality of PH CH₃COO = 3

PH = - log (H⁺)

3 = - log (H⁺)

H⁺ = 1 x 10^-3 M

CHAPTER V

COVER

5.1  Conclusions

1.    Determine the pH of the solution by using universal pH indicator

2.    Calculate the concentration of the solution with a certain pH value

5.2 Suggestions

Suggestions in this experiment Practice should follow the rules of the practicum well. Pratikan must be careful to measure or weigh a substance so that the results can be more accurate measuring. Because in this lab, many data are not the same between group

BIBLIOGRAPHY

Achmad, Hizkia. 1996. Kimia larutan. Bandung: PT.Citra Aditya Bakti

Anonim, 2015. Asam.  https://id.wikipedia.org/wiki/Asam Diakses pada 16/05/2017

Anonim, 2015. Basa. https://id.wikipedia.org/wiki/Basa Diakses pada 16/05/2017

Anonim, 2015. Garam.  https://id.wikipedia.org/wiki/Garam_(kimia) diakses pada 16/05/2017

Anonim, 2015. Indikator Asam Basa.  https://id.wikipedia.org/wiki/Indikator_ asam-basa diakses pada 16/05/2017

Pudjatmaka, Aloisius Hadyana. 1980. Ilmu Kimia Untuk Universitas. Jakarta: Erlangga