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How did Mendeleev Arrange the Periodic Table

November 30, 2020November 30, 2020 by Raju

How did Mendeleev Arrange the Periodic Table

Mendeleev’s periodic Law and Mendeleev’s periodic table
While working systematically on the physical and chemical properties of elements, Dmitri Invanovich Mendeleev noticed that properties of elements varied regularly with the atomic mass. He arranged the 63 elements then known in a table on the basis of similarities in properties. It was found that most of the elements occupied places in the table in order of their increasing atomic masses. In 1869, Mendeleeve formulated a law, now known as the periodic law. The law is stated as follows.
The properties of elements are periodic functions of their atomic masses. This means, if the elements are arranged in order of increasing atomic masses then those with similar properties are repeated at regular intervals.
On the basis of the periodic law, Mendeleev presented his classification in the form of a table, now known as Mendeleev’s periodic table. A simplified version of this periodic table is given below. In this table, copper, silver and gold find places in groups I as well as VIII.

Groups →

Periods ↓

III

VII

VIII

9.4

27.3

35.5

Fr Co Ni Cu

56 59 59 63

100

Ru Rh Pd Ag

104 104 106 108

108

112

113

118

122

125

127

133

137

138

140

178

180

182

184

Os Ir Pt Au

195 197 198 199

199

200

204

207

208

231

240

This table consists of vertical columns called groups and horizontal rows called periods. There are only eight groups in the table. Mendeleev left some vacant places (shown by question marks) for the yet undiscovered elements. Noble gases were not discovered then. So, he did not provide any place for them in his periodic table.
Mandeleev’s idea was remarkable in that he used a fundamental atomic property (atomic mass) as the basis of classification. While classifying elements he laid special emphasis on tow factors.
1. Similar elements were grouped together.
2. Elements were arranged in order of increasing atomic masses.

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Modified version of Mendeleev’s Periodic Table :

The elements which were undiscovered and for whom Mendeleev had left vacant places were discovered later. Some of these are scandium (Sc), gallium (Ga) and germanium (Ge). These elements were accommodated in their proper places in the table. The elements helium (He), neon (Ne), argon (Ar), Krypton (Kr), Xenon (Xe) and radon (Rn) became known only towards the end of the nineteenth century. These elements, called noble gases, were placed in the table as a separate group, called 0 group. The periodic table had to be modified then. The modified version of the table is shown below.
How did Mendeleev Arrange the Periodic Table 1

Lanthanide series* (along with langhanum)

Actinide series**(along with actinium)

Features of the modified version of Mendeleev’s periodic table :

1. Groups into subgroups : Each group of this periodic table is further divided into two subgroups A and B. The properties of elements within a subgroup resemble more markedly but they differ from those of the elements of the other subgroups. For example., lithium (Li), sodium (Na), potassium (K), etc., of subgroups IA have close resemblance of properties but they have hardly any resemblance to the coinage metals (Cu, Ag and Au) of subgroup IB.
Mendeleev allowed the subgroups to be represented within the same group.
2. Prediction of errors : This periodic table could predict errors in the atomic masses of some elements on the basis of their position in the periodic table. For example, when the periodic table was published, the experimental value of the atomic mass of beryllium (Be) we was supposed to be 13.65 and its valency, 3. So, the position of Be should have been somewhere else, but Mendeleev placed it at its appropriate position on the basis of its properties. He further suggested that the atomic mass of Be needed correction. Mendeleev predicted its atomic mass to be 9.1 and valency, 2. Latter investigations proved him right.
Similarly, the atomic mass of uranium was corrected from 120 to 240. Corrections were also made in the atomic masses of gold, platinum, etc.
3. Predictions of properties of higher to undiscovered element : We know that Mendeleev classified the elements in order of their increasing atomic masses. However, this order had to be ignored at some places to make sure that the elements with similar properties fell in the same group. In doing so, he left some vacant places in the table. These vacant places were kept reserved for elements not discovered till then. Mendeleev was confident that these elements would be discovered later and they would occupy these vacant places. Not only this, he also predicted the properties of these undiscovered elements on the basis of this study of his the properties of the neighboring elements. Amazingly, when the missing elements of Mendeleev’s periodic table were discovered subsequently, their properties were found to be very similar to those predicted by Mendeleev.

The elements scandium, gallium and germanium were not known in 1871 but their existence was predicted by mendelev. He named these elements as eka-boron, eka-Aluminium and eka silicon when these elements were discovered, they were named scandium, gallium and germanium respectively and their properties were found to be in good agreement with those predicted by Mendeleev. Properties of ka-aluminium (predicted by Mendeleev) and those of the gallium (discovered later) are given in table.

Property	Eka-aluminium	Gallium
Atomic mass	68	69.7
Formula of oxide	E₂O₃	Ga₂O₃
Formula of chloride	ECl₃	GaCl₃

Considering its atomic mass, titanium (Ti) should have been placed below aluminium in the periodic table, but Mendeleev placed is below silicon (Si) because the properties of titanium were similar to those of silicon. Thus, a gap was left below aluminium in the periodic table. This gap was filled up by gallium which was discovered later. The properties of gallium (Ga) were found to be similar to those of boron and aluminium.
4. Basic features intact : All the basic features of Mendeleev’s periodic table are intact even today. Even when a new class of elements, i.e., noble gases, were discovered, they found place in a separate group called the zero group. The existing order of the periodic table was not at all disturbed.
Discrepancies in Mendeleev’s periodic table :
Mendeleev’s periodic table has the following defects.
1. Position of hydrogen : The position of hydrogen in the periodic table is anomalous. Hydrogen resembles alkali metals (Li, Na, K, etc). So it may be placed in the group of the halogens (VII A)
2. Position of lanthanides and actinides : The elements from atomic number 57 to 71 are collectively known as lanthanides. They do not have a proper place in the periodic table. They all have been placed at the same position in group III and period 6. Similarly, the actinides (atomic numbers 89-103) also have no proper place in the periodic table. These elements have also been placed in the same position, in group III and period 7.
3. Some similar elements are separated, while some dissimilar elements have been placed in the group : Some similar elements are separated in the periodic table. For example, copper (Cu) and mercury (Hg), silver (Ag) and thallium (Tl), and barium (Ba) and lead (Pb). On the other hand, some dissimilar elements have been placed together in the same group. For example, copper (Cu), silver (Ag) and gold (Au) have been placed in group I along with the alkali metals. Similarly, manganese (Mn) is placed in the group of the halogens.
4. Presence of some anomalous pairs of elements : In Mendeleev’s periodic table, elements are arranged in order of increasing atomic mass. In some places, this order has been ignored.
(a) The atomic mass of argon is 40 and that of potassium is 39. But argon is placed before potassium in the periodic table.
(b) The positions of cobalt and nickel are not in proper order. Cobalt (at. mass = 58.9) is placed before nickel (at. mass = 58.6).
(c) Tellurium (at. mass = 127.6) is placed before iodine (at. mass = 126.9).
(d) Thorium (at. mass = 232.12) is placed before protactinium (at. mass = 231)
5. Position of isotopes : The isotopes of an element have no place in the periodic table.
The failure of Mendeleev’s periodic law to explain the wrong order of the atomic masses of some elements and the position of isotopes led scientists working in this field to conclude that atomic mass cannot be the basis for the classification of elements. There must be a more fundamental property of elements which can be the basis of classification.
Anomalous pairs of elements

Element →	Ar	K	Co	Ni	Te	I	Th	Pa
Atomic mass	40	39	59.9	58.6	127.6	126.9	232.12	231
Group	0	IA	VIII	VIII	VI B	VII B	III B	III B

What is meant by the Kinetic Theory of Matter?

November 30, 2020November 30, 2020 by Raju

What is meant by the Kinetic Theory of Matter?

The Kinetic Theory of Matter:

The arrangement and movement of particles in solids, liquids and gases are described in the kinetic theory of matter.
The kinetic theory of matter is used to explain the changes in the states of matter.
The changes in the states of matter are caused by heating or cooling. For example, ice melts when it is heated and water changes into ice when it is frozen.
The kinetic energy of particles increases during heating.
The kinetic energy of particles decreases during cooling.

Arrangement and movement of particles in a gas:

Arrangement of particles:
The particles are very far apart from each other and are in a random arrangement.
Forces of attraction between particles:
There are weak forces between the particles. Movement of particles The particles can vibrate, rotate and move freely. The rate of collision is greater than the rate of collision in a liquid.
Energy content of particles:
Highest energy content as movement is at random.
Why does a gas not have a fixed shape or volume?
Gas can be easily compressed because the particles have more space between them compared to the particles of liquids or solids. Thus, it has no fixed shape or volume.

What is meant by the Kinetic Theory of Matter 1

Arrangement and movement of particles in a liquid:

Arrangement of particles:
The particles are packed closely together but not in an orderly arrangement.
Forces of attraction between particles:
The particles are held together by strong forces but weaker than the forces in a solid.
Movement of particles:
The particles can vibrate, rotate and move throughout the liquid. They collide against each other.
Energy content of particles:
Higher energy content as particles can move easily.
A liquid cannot be compressed easily because the particles are packed closely even though are arranged k in disorderly manner. Thus, it has a fixed volume.
It does not have a fixed shape but takes the shape of the container.

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Arrangement and movement of particles in a solid:

Arrangement of particles:
The particles are packed closely together in an orderly manner.
Forces of attraction between particles:
There are strong forces between the particles.
Movement of particles:
The particles can only vibrate and rotate about their fixed positions.
Energy content of particles:
Low energy content as movement is restricted.
Why does a solid have a fixed shape or volume?
A solid cannot be compressed because its particles are very close to one another. Thus, it has a fixed shape or volume.

How can you change matter from one state to another?

Changes in the states of matter:
What is meant by the Kinetic Theory of Matter 2 Boiling/Evaporation:

When a liquid is heated, the particles of the liquid gain kinetic energy and move faster as the temperature increases.
Eventually, the particles have enough energy to completely break the forces holding them together.
The particles are now able to move freely and far apart.
A gas is formed. The temperature at which this happens is called the boiling point.
The boiling point is the temperature at which a liquid changes into A a gas at a particular pressure.

Sublimation:

Sublimation is a process by which a solid changes directly into a gas without passing through the liquid state.
Examples of substances that undergo sublimation are iodine, ammonium chloride, NH₄Cl and dry ice (solid carbon dioxide).

Freezing:

When a liquid is cooled, the particles in the liquid lose energy and move slower.
As the temperature continues to drop, the particles continue to lose more energy until they do not have enough energy to move freely.
At this point, the liquid changes into a solid.
The temperature at which this happens is called the freezing point.
The freezing point is the temperature at which a liquid changes into a solid at a particular pressure.

Condensation:

When a gas is cooled, the particles in the gas lose energy and move slower.
As the temperature drops, the gas particles lose energy and M move more slowly.
Eventually, the movements of the particles become slow enough for the gas to change into a liquid.
This change occurs at the boiling point of the substance.

Melting:

When a solid is heated, X the particles in the solid gain kinetic energy and vibrate more vigorously.
The particles vibrate faster as the temperature increases until the energy they gain is able to overcome the forces, that hold them at their fixed positions.
At this point, the solid becomes a liquid.
The temperature at which this happens is called the melting point.
The melting point is the temperature at which a solid changes into a liquid at a particular pressure.

Melting and Freezing points of Naphthalene Experiment

Aim: To determine the melting and freezing points of naphthalene.
Materials: Naphthalene and tap water.
Apparatus: Boiling tube, 250 cm³ beaker, thermometer, tripod stand, retort stand and clamp, Bunsen burner, stopwatch, conical flask and wire gauze.
Procedure:
A. Heating of naphthalene

A boiling tube is filled with naphthalene to a depth of 3 cm and a thermometer is put into it.
The boiling tube is suspended in a beaker half-filled with water using a retort stand and a clamp as shown in Figure A. The level of naphthalene in the boiling tube is ensured to be below the level of water in the beaker.
The water is heated and the naphthalene (highly flammable) is stirred slowly with the thermometer.
When the temperature of the naphthalene reaches 60°C, the stopwatch is started. The temperature and the state(s) of the naphthalene are recorded at half-minute intervals until the temperature of the naphthalene reaches 90°C.

B. Cooling of naphthalene

The boiling tube in section A is removed from the water bath. The outer surface of the boiling tube is dried and immediately it is put in a conical flask, as shown in Figure B. The naphthalene is stirred continuously.
The temperature and state(s) of the naphthalene are recorded at half¬minute intervals until the temperature drops to about 60°C.

Results:

Heating of naphthalene			Cooling of naphthalene
Time (min)	Temperature (°C)	State	Time (min)	Temperature (°C)	State
0.0	61.0	Solid	0.0	87.0	Liquid
0.5	65.0	Solid	0.5	84.0	Liquid
1.0	67.0	Solid	1.0	83.0	Liquid
1.5	71.0	Solid	1.5	81.0	Liquid
2.0	74.0	Solid	2.0	80.0	Liquid and solid
2.5	76.0	Solid	2.5	80.0	Liquid and solid
3.0	79.0	Solid	3.0	80.0	Liquid and solid
3.5	80.0	Solid and liquid	3.5	80.0	Liquid and solid
4.0	80.0	Solid and liquid	4.0	80.0	Liquid and solid
4.5	80.0	Solid and liquid	4.5	80.0	Liquid and solid
5.0	80.0	Solid and liquid	5.0	80.0	Liquid and solid
5.5	80.0	Solid and liquid	5.5	76.0	Solid
6.0	80.0	Solid and liquid	6.0	73.0	Solid
6.5	83.0	Liquid	6.5	69.0	Solid
7.0	86.0	Liquid	7.0	66.0	Solid
7.5	89.0	liquid	7.5	64.0	Solid

Discussion:

A graph of temperature against time is plotted for the heating of naphthalene, as shown in Figure C.
Notice that there is a certain part of the curve where there is no change in the temperature with time during heating. At this temperature, both solid and liquid are present. It is the melting point of naphthalene. Hence, the melting point of naphthalene is 80.0°C.
(a) At point A, naphthalene exists as a solid.
(b) When the solid is heated, heat energy is absorbed. This causes the particles to gain kinetic energy and vibrate faster. The temperature increases from point A to point 8.
(c) At point 8, solid naphthalene begins to melt. During the melting process, the temperature of naphthalene does not rise even though heating continues. The temperature remains constant because the heat energy absorbed by the particles is used to overcome the forces between particles so that the solid can turn into a liquid. At this temperature, both solid and liquid are present.
(d) At point C, all the solid naphthalene has melted.
(e) From point C to point D, the particles in liquid naphthalene absorb heat energy and move faster. The temperature increases from point C to point D.
A graph of temperature against time is plotted for the cooling of naphthalene, as shown in Figure D.
Notice that, there is a certain part of the curve where the temperature is constant with time during the cooling. At this temperature, both solid and liquid are present. It is the freezing point of naphthalene. Hence, the freezing point of naphthalene is 80.0°C.
(a) At point E, naphthalene exists as a liquid.
(b) When the liquid is cooled, the particles in the liquid lose their kinetic energy. They move slower as the temperature decreases from point E to point F.
(c) At point F, liquid naphthalene begins to freeze. During the freezing process, the temperature of naphthalene remains constant because the heat loss to the surroundings is exactly balanced by the heat energy liberated as the particles attract one another to form a solid. At this temperature, both solid and liquid are present.
(d) At point C, all the liquid naphthalene has frozen.
(e) From point C to point H, the particles in solid naphthalene release heat energy and vibrate slower. The temperature decreases from point C to point H.
During the heating of naphthalene,
(a) a water bath is used instead of direct heating with a Bunsen flame. This is to ensure that the naphthalene is
heated evenly. Furthermore, the naphthalene is flammable.
(b) the naphthalene is stirred continuously to ensure an even heating.
During the cooling of naphthalene,
(a) the boiling tube containing liquid naphthalene is placed in a conical flask. This is to ensure an even cooling process and to minimise heat loss to the surroundings.
(b) the naphthalene is stirred continuously to avoid supercooling.
Supercooling is a condition in which the temperature of a cooling liquid drops below its normal freezing point, without the appearance of a solid.
A water bath is used in this experiment because the melting point of naphthalene is below 100°C, the maximum temperature that can be attained by the water bath. For solids with melting points above 100°C, a liquid with a higher boiling point than water such as oil must be used.

Conclusion:
The melting and freezing points of naphthalene are the same, that is 80.0°C.

What is stoichiometry and why is it used in chemistry?

November 30, 2020November 30, 2020 by Veerendra

What is stoichiometry and why is it used in chemistry?

Stoichiometry is a study of quantitative composition of substances involved in the chemical reactions.
A balanced chemical equation can be used to calculate number of moles, number of particles and mass or volume of a reactant or product.
By using the information obtained from a balanced chemical equation, it is possible to calculate the quantities of reactants used or the quantities of products formed in the reaction.
Generally, the steps involved in the stoichiometric calculations are as follows.
(1) Write down the balanced equation of the reaction.
(2) Gather information from the question. If necessary, convert the given unit to the number of moles.
(3) Based on the equation, compare the ratio of moles of the related substances.
(4) Calculate the answer proportionately. Then, convert the answer to the required unit.

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Stoichiometry Problems with Answers

1. How many moles of potassium are needed to react with 0.5 mole of bromine gas?
2K(s) + Br₂(g) ⟶ 2KBr(s)
Solution:
What is stoichiometry and why is it used in chemistry 1

2. Ethene gas burns in excessive oxygen according to the following equation.
C₂H₄(g) + 3O₂(g) ⟶ 2CO₂(g) + 2H₂O(l)
Find the volume of carbon dioxide released at STP if 42 g of ethene is burnt completely. [Relative atomic mass: H, 1; C, 12. Molar volume: 22.4 dm³ mol^-1 at STP]
Solution:
What is stoichiometry and why is it used in chemistry 2

3. What is the mass of zinc needed to produce 2.4 dm³of hydrogen gas at room conditions?
Zn(s) + 2HNO₃(aq) ⟶ Zn(NO₃)₂(aq) + H₂(g)
[Relative atomic mass: Zn, 65. Molar volume: 24 dm³ mol^-1 at room conditions]
Solution:
What is stoichiometry and why is it used in chemistry 3

4. Aluminium reacts with copper(II) oxide to produce aluminium oxide and copper. If 2.0 g of excess aluminium is reacted with 0.06 mole of copper(II) oxide, find the mass of aluminium left after the reaction.
[Relative atomic mass: Al, 27]
Solution:
What is stoichiometry and why is it used in chemistry 4

5. Excess sodium chloride is added to 50.0 cm³ of silver nitrate solution. 2.87 g of silver chloride is precipitated. Calculate the concentration of the silver nitrate solution in mol dm^-3.
[Relative atomic mass: Cl, 35.5; Ag, 108]
Solution:

6. In the preparation of copper(II) sulphate, a student added 4.0 g of copper(II) oxide to 1.25 mol dm^-3 sulphuric acid. Calculate the volume of the acid needed to react completely with the copper(II) oxide. [Relative atomic mass: O, 16; Cu, 64]
Solution:

7. Excess aluminium powder is added to 300 cm³ of 2.0 mol dm^-3 hydrochloric acid. The mixture is then warmed to speed up the reaction. Calculate the mass of the salt formed. [Relative atomic mass: Al, 27; Cl, 35.5]
Solution:

8. 150 cm³ of 1.0 mol dm^-3 ammonia solution is completely neutralised with phosphoric acid using a titration method. Calculate the mass of ammonium phosphate formed. [Relative atomic mass: H, 1; N, 14; O, 16; P, 31]
Solution:

9. 6.20 g of copper(II) carbonate is added to 100 cm³ of 14.6 g dm^-3 hydrochloric acid. Calculate the mass of copper(II) chloride produced. [Relative atomic mass: H, 1; C, 12; O, 16; Cl, 35.5; Cu, 64]
Solution:
What is stoichiometry and why is it used in chemistry 9

What is the Haber process used for?

November 30, 2020November 30, 2020 by Veerendra

What is the Haber process used for?

Manufacture of ammonia in industry

Most of the world supply of ammonia is manufactured through Haber process.
The raw materials for the manufacture of ammonia are hydrogen gas and nitrogen gas. The ratio for the raw materials is one portion of nitrogen to three portions of hydrogen.
(a) Nitrogen is obtained from the fractional distillation of liquid air.
(b) Hydrogen can be obtained by two methods: The reaction between methane (from natural gas) or heated coke with steam.
The optimum conditions for Haber process is
(a) Temperature: 450°C
(b) Pressure: 200 atmosphere
(c) Catalyst: red hot iron
During Haber process:
(a) A mixture of one volume of dry nitrogen gas and three volume of pure hydrogen gas are mixed and passed to the compressor and compressed to a pressure of about 200 atm.
(b) The mixture is then passed through layers of heated and finely divided iron catalyst in the reactor at a temperature of about 450°C.
(c) Ammonia is produced in the reactor but the reaction is reversible.

(d) The production of ammonia is exothermic and gives out heat. It is passed into the cooling chamber, then liquefied and separated to get a better yield.
(e) The unreacted nitrogen and hydrogen are recycled and passed back into the reactor converted into ammonia,
together with the new source of nitrogen and hydrogen.
About 98% of nitrogen and hydrogen are converted into ammonia.

What is the Haber process used for 3

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Preparation of ammonium sulphate experiment

Aim: To prepare ammonium sulphate.
Materials: 1 mol dm^-3 sulphuric acid, 2 mol dm^-3 ammonia solution, methyl orange, filter paper.
Apparatus: 25.0 cm³ pipette, burette, conical flask, white tile, retort stand and clamp, beaker, glass rod, evaporating dish, filter funnel, Bunsen burner, tripod stand, wire gauze.
Procedure:
A. Determining the volume of sulphuric acid that will neutralise 25.0 cm³ of ammonia solution

Safety Measures

Concentrated sulphuric acid is corrosive.
Do not inhale ammonia gas.

25.0 cm³ of 2 mol dm^-3 ammonia solution is measured and transferred by a pipette to a clean conical flask.
Three drops of methyl orange indicator are added to the alkali. The solution turns yellow.
A clean burette is filled with 1 mol dm^-3 sulphuric acid and clamped to a retort stand.
The initial burette reading is recorded.
The conical flask with its contents is placed on a white tile below the burette as shown in Figure.
The sulphuric acid is added slowly into the conical flask. The conical flask is swirled gently throughout the titration.
The addition of the sulphuric acid is stopped when the indicator changes from yellow to orange.
The final burette reading is recorded.
The volume of acid needed to completely neutralise the 25.0 cm³ of 2 mol dm^-3 ammonia solution is alculated. Let this volume be V cm³.

B. Preparing ammonium sulphate salt

What is the Haber process used for 5

25.0 cm³ of 2 mol dm^-3 ammonia solution is pipetted into a clean beaker. No indicator is added.
V cm³ of 1 mol dm^-3 sulphuric acid is added from the burette to the ammonia solution and stirred.
The mixture in the beaker is transferred to an evaporating dish and heated until a saturated solution is formed.
The hot, saturated salt solution is left to cool for crystallisation to occur.
The crystals of ammonium sulphate formed are filtered and pressed between sheets of filter paper.

Observations:

A colourless solution is formed when sulphuric acid is added to ammonia solution.
The crystals obtained are white in colour.

Discussion:

The equation for the reaction is
H₂SO₄(aq) + 2NH₃(aq) → (NH₄)₂SO₄(aq)
Methyl orange is an acid-base indicator used to determine the end point of the titration.
The first titration is carried out to determine the exact volume of sulphuric acid required to completely neutralise the 25.0 cm³ of ammonia solution.
The salt solution in the first titration is discarded because it is contaminated by methyl orange.
The ammonium sulphate solution should not be heated until dryness because ammonium sulphate decomposes when it is overheated.
The weight of ammonium sulphate obtained from the activity is always less than the theoretical value. This is because some of the salt is not fully crystallised out and still remains in the solution.
Other ammonium fertilisers such as ammonium nitrate can be prepared from the reaction between nitric acid and ammonia solution.

Conclusion:
Ammonium sulphate and other ammonium fertilisers can be prepared by neutralising ammonia solution with the respective acids.

What is meant by a neutralization reaction?

November 30, 2020November 30, 2020 by Veerendra

What is meant by a neutralization reaction?

The reaction of an acid and a base is called a neutralisation reaction. In this reaction, the acidity of an acid is neutralised by an alkali. At the same time, the alkalinity of the alkali is neutralised by the acid. A salt and water are the only products of a neutralisation reaction.
Acid + alkali → salt + water

What happens in a neutralization reaction?

A neutralisation reaction occurs when an alkali reacts with an acid to form a salt and water.
For example:
(a) Acidic solutions contain hydrogen ions. Alkaline solutions contain hydroxide ions.
(b) When an alkali is added to an acid to neutralise the acid, it is the hydroxide ion which combines with the hydrogen ion and ‘cancel each other out’. A water molecule is formed.
H⁺(aq) + OH^–(aq) → H₂O(l)
The above ionic equation shows what happens in a neutralisation reaction.
When writing equations involving the neutralisation of ammonia solution by different acids, do not show the formation of water.
For example:

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What are the applications of neutralization in our everyday life

Neutralisation in agriculture

Soils from different sources have different pH values. Soils can be acidic, neutral or alkaline.
Farmers add powdered lime or limestone to neutralise acidity in soil.
The traditional way of adding ashes of burnt wood is also effective. These ashes contain the alkalis such as sodium hydroxide and potassium hydroxide.
Farmers use a compost of rotting vegetables or leaves to treat basic soils. As the vegetables and leaves decompose, carbon dioxide is given out. This acidic gas dissolves in water to form carbonic acid which can then neutralise the alkalis in basic soils.

Neutralisation in industry

Electroplating industry
Effluent from the electroplating industry contains acids such as sulphuric acid and must be treated before it is discharged into rivers and streams. The acids in the effluent are neutralised by adding lime.
Energy industry
Power stations burn coal to produce electricity. Coals contain sulphur and burning sulphur in air produces sulphur dioxide which is responsible for the formation of acid rain.
S(s) + O₂(g) → SO₂(g)
When a mixture of coal and limestone is heated, the limestone decomposes to form lime.
CaCO₃(s) → CaO(s) + CO₂(g)
The lime neutralises the acidic sulphur dioxide.
2CaO(s) + 2SO₂(g) + O₂(g) → 2CaSO₄(s)
Chemical industry
Sulphuric acid plants use the Contact process to produce sulphuric acid. Sulphur dioxide gas is produced from the combustion of sulphur or from the roasting of sulphide ores. To prevent sulphur dioxide gas from escaping into the atmosphere, waste gases are scrubbed by passing through powdered lime. Lime neutralises the acidic sulphur dioxide.
CaO(s) + SO₂(g) → CaSO₃(s)

Neutralisation in medicine

Indigestion is caused by excess acid secreted by the stomach. It can be treated by neutralising the excess acid.
Anti-acid indigestion medicines contain bases like calcium carbonate, sodium hydrogen carbonate, aluminium hydroxide and magnesium hydroxide to neutralise the hydrochloric acid in the stomach.