Acids, Bases and Salts Class 9 Science Notes Maharashtra Board

Acids, Bases and Salts Class 9 Science Notes Maharashtra State Board

Ionic Compounds: Recapitulation
The molecule of an ionic compound has two constituents: cation (positive ion/basic radical) and anion (negative ion /acidic radical). There is a force of attraction between these ions as they are oppositely charged, called the ionic bond. The force of attraction between one positive charge on a cation and one negative charge on an anion makes one ionic bond.

While studying static electricity we have learned that any body naturally tends to change from an electrically charged state into an electrically neutral state. Why, then, is an electrically charged ion formed from an electrically balanced, that is, neutral atom? The explanation lies in the electronic configuration of atoms. Let us see once again how the sodium and chlorine atoms form the Na⁺ and Cl^– and as a result, how the NaCl salt is formed.

The outermost shell of the sodium and the chlorine atoms is not a complete octet. However outermost shell in both the Na⁺ and Cl^– ions is a complete octet. An electronic configuration with a complete octet indicates a stable state. Further, an ionic bond is formed between the oppositely charged Na⁺ and Cl^– ions, and therefore an ionic compound NaCl having very high stability is formed.

Dissociation of Ionic Compounds
On mixing the substances as shown here, what are the resulting mixtures formed by mixing the following substances called?

• Water and salt
• Water and sugar
• Water and sand
• Water and sawdust

On dissolving in water, an ionic compound forms an aqueous solution. In the solid state, the oppositely charged ions in the ionic compound are sitting side by side. When an ionic compound begins to dissolve in water, the water molecules push themselves in between the ions of the compound and separate them from each other. That is to say, an ionic compound dissociates while forming an aqueous solution. Each of the dissociated ions in the aqueous solution is surrounded by water molecules. This state is indicated by writing (aq), meaning aqueous, on the right of the symbol of the ion.

Arrhenius’s Theory of Acids and Bases
The Swedish scientist Arrhenius put forth a theory of Acids and Bases in the year 1887. This theory gives definitions of acids and bases as follows:
Acid: An acid is a substance which on dissolving in water gives rise to H⁺ ion as the only cation. For example, HCl, H₂SO₄, H₂CO₃.

Base: A base is a substance which on dissolving in water gives rise to the OH^– ion as the only anion. For example, NaOH, Ca(OH)₂

Classification of Acids and Bases

1. Strong and weak acids, bases, and alkali
Acids and bases are classified into strong and weak types based on the extent to which they dissociate in their aqueous solutions.

• Strong acid: On dissolving in water, a strong acid dissociates almost completely and the resulting aqueous solution contains mainly H⁺ ions and the concerned acidic radical. For example, HCl, HBr, HNO₃, H₂SO₄.
• Weak acid: On dissolving in water a weak acid does not dissociate completely, and the resulting aqueous solution contains H⁺ ion and the concerned acidic radical in small proportion along with large proportion of the undissociated molecules of the acid. For example, H₂CO₃, and CH₃COOH (Acetic Acid).
• Strong base: On dissolving in water, a strong base dissociates almost completely and the resulting aqueous solution contains mainly OH^– ions and the concerned basic radicals. For example, NaOH, KOH, Ca(OH)₂, Na₂O.
• Weak base: On dissolving in water a weak base does not dissociate completely, and the resulting aqueous solution contains a small proportion of OH^– ions and the concerned basic radical along with a large proportion of undissociated molecules of the base. For example, NH₄OH.
• Alkali: The bases which are highly soluble in water are called alkali. For example, NaOH, KOH, NH₃. Here, NaOH and KOH are strong alkalies while NH₃ is a weak alkali.

2. Basicity and Acidity
Acids and bases are also classified according to their basicity and acidity respectively.

• Basicity of acids: The number of H⁺ ions obtainable by the dissociation of one molecule of an acid is called its basicity.
• Acidity of bases: The number of OH^– ions obtainable by the dissociation of one molecule of a base is called its acidity.

Concentration of Acid and Base
Cut a lemon into two equal parts. Take the juice of each part into two separate beakers. Pour 10 of drinking water in one beaker and 20 in the second. Stir the solutions in both beakers and taste them. Is there any difference in the tastes of the solutions in the two beakers? What is that difference? In the above activity, the sour taste of the solutions is because of the solute, lemon juice, in them. The quantity of the lemon juice is the same in both the solutions. Yet their taste is different. The solution in the first beaker is more sour than the one in the second. Why is it so?

Although the quantity of the solute is the same in both solutions, the quantity of the solvent is different. The ratio of the quantity of the solute to the quantity of the resulting solution is different. This ratio is larger for the solution in the first beaker and, therefore, that solution tastes more sour. On the other hand, the proportion of the lemon juice in the total solution in the second beaker is smaller and the taste is less sour.

The taste of foodstuff depends upon the nature of the taste-giving ingredient and its proportion in the foodstuff. Similarly, all the properties of a solution depend on the nature of the solute and solvent and also on the proportion of the solute in the solution. The Proportion of a solute in a solution is called the concentration of the solute in the solution. When the concentration of a solute in its solution is high, it is a concentrated solution, while the solution is called a dilute solution when the concentration of the solute is low.

Several units are used to express the concentration of a solution. Two of these units are used more frequently. The first unit is the mass of solute in grams dissolved in one liter of the solution. (grams per liter, g/L). The second unit is the number of moles of the solute dissolved in one liter of the solution. This is also called the molarity (M) of the solution. The molarity of a solute is indicated by writing its molecular formula inside a square bracket. For example [NaCl] = 1 means the molarity of this solution of common salt is 1M (1 Molar).

The pH of the Solution
We have seen that acids and bases dissociate to a smaller or larger extent on dissolving in water forming H⁺ and OH^– ions respectively. H⁺ and OH^– ions are found in different proportions in all-natural aqueous solutions, and that determines the properties of those solutions.

For example, the proportion of H⁺ and OH^– ions divides soil into acidic, neutral, and basic types of soil. Blood, cell sap, etc. must have H⁺ and OH^– ions in certain definite proportions for their proper functioning. Fermentation carried out with the help of micro-organisms, other biochemical processes, and also many chemical processes requires the proportion of H⁺ and OH^– ions to be maintained within certain limits. Pure water, also, undergoes dissociation to a very small extent and gives rise to H⁺ and OH^– ions in equal proportion.

Due to this property of water to undergo dissociation, there exist both H⁺ and OH^– ions in any aqueous solution. However, their concentration may be different.

The concentration of H⁺ ions formed by dissociation of water at 25°C is 1 × 10^-7 mol/L. At the same temperature, the concentration of H⁺ ions in 1M solution of HCl is 1 × 100 mol/L. While in a 1M NaOH solution, the concentration of H+ ions is 1 × 10^-14 mol/L. Thus, we see that in common aqueous solutions, the range of H+ ion concentration is very wide from 10⁰ to 10^-14 mol/L. In 1909, the Danish scientist Sorensen introduced a convenient new scale of expressing H⁺ ion concentration which is found to be very useful in chemical and biochemical processes. It is the pH scale (pH: power of hydrogen) The pH scale extends from 0 to 14. According to this scale, pure water has a pH of 7 meaning pure water has [H⁺] = 1 × 10^-7 mol/L. pH 7 indicates a neutral solution. This pH is the midpoint of the scale. The pH of an acidic solution is less than 7 and that of a basic solution is greater than 7.

Universal Indicators
We know that some natural and synthetic dyes show two different colors in acidic and basic solutions, and such dyes are used as acid-base indicators. In the pH scale, the pH of solutions varies from 0 to 14 by the strength of the acid or base. To show these variations in pH, a universal indicator is used. A universal indicator shows different colors at different values of pH.

A universal indicator is made by mixing several synthetic indicators in specific proportions. The pH of a solution can be determined using a universal indicator solution or the pH paper made from it. However, the most accurate method of measuring the pH of a solution is to use an electrical instrument called a pH meter. In this method, pH is measured by dipping electrodes into the solution.

Reactivity of Acids and Bases

1. Neutralization
Take 10ml dilute HCl in a beaker. Use a glass rod to put a drop of this solution on a pH paper and record the pH of the solution. Add to it a few drops of dilute NaOH solution using a dropper and stir the solution with the glass rod. Measure the pH of the resulting solution by putting a drop of this solution on another pH paper. In this manner, go on adding dilute NaOH drop by drop and recording the pH. What do you find? Stop adding NaOH when a green color appears on the pH paper, that is when the pH of the solution becomes 7.

The Neutralization Reaction:
Why does the pH increase as NaOH solution is added drop by drop to the HCl solution? The answer lies in the process of dissociation. Both HCl and NaOH dissociate in their aqueous solutions. The addition of NaOH solution to HCl solution is like adding a large concentration of OH^– ions to a large concentration of H+ ions. However, water dissociates into H⁺ and OH^– ions to a very small extent. Therefore, on mixing, the excess OH- ions combine with the excess H⁺ ions to form H₂O molecules which mix with the solvent water. This change can be represented by the ionic equation shown as follows.
H⁺ + Cl^– + Na⁺ + OH^– → Na⁺ + Cl^– + H₂O
It can be seen from the above equation that the Na⁺ and Cl^– ions are on both sides. Therefore the net ionic reaction is H⁺ + OH^– → H₂O
As the NaOH solution is added drop by drop to the HCl solution, the concentration of H⁺ decreases due to combination with added OH^– ions, and that is how the pH goes on increasing.

When enough NaOH is added to HCl, the resulting aqueous solution contains only Na⁺ and Cl^– ions, that is, NaCl, a salt, and the solvent water. The only source of H⁺ and OH^– ions in this solution is the dissociation of water. Therefore, this reaction is called the neutralization reaction. The neutralization reaction is also represented by the following simple equation.
HCl (Acid) + NaOH (Base) → NaCl (Salt) + H₂O

2. Reaction of Acids with Metals
The reaction of acids with metals is determined by the strength and the concentration of the acid and also by the reactivity of the metal and the temperature. It is easy to bring about the reaction of a dilute solution of strong acids with moderately reactive metals at normal temperatures.

Activity: Take a big test tube. Choose a rubber stopper in which a gas tube can be fitted. Take a few pieces of magnesium ribbon in the test tube and add some dilute HCl to it. Take a lighted candle near the end of the gas tube and observe. What did you observe? Magnesium metal reacts with dilute hydrochloric acid and an inflammable gas, hydrogen, is formed. During this reaction, the reactive metal displaces hydrogen from the acid to release hydrogen gas. At the same time, the metal is converted into basic radical which combines with the acidic radical from the acid to form the salt.

3. Reaction of Acids with Oxides of Metals
Take some water in a test tube and add a little red oxide (the primer used before painting iron articles) to it. Now add a small quantity of dilute HCl to it, shake the test tube, and observe.
1. Does the red oxide dissolve in water?
2. What change takes place in the particles of red oxide on adding dilute HCl?
The chemical formula of red oxide is Fe₂O₃. The water-insoluble red oxide reacts with HCl to produce a water-soluble salt FeCl₃. This gives a yellowish color to the water. The following chemical equation can be written for this chemical change.
Fe₂O₃ (s) + 6HCl (aq) → 2FeCl₃ (aq) + 3H₂O (l)

4. Reaction of Bases with Oxides of Non-metals
Bases react with oxides of non-metals to form salt and water. Hence, oxides of non-metals are said to be acidic. Sometimes the oxides of non-metals themselves are said to be examples of acids. Zinc oxide reacts with sodium hydroxide to form sodium zincate (Na₂ZnO₂) and water. Similarly, aluminium oxide reacts with sodium hydroxide to form sodium aluminate (NaAlO₂) and water.

5. Reaction of Acids with Carbonates and Bicarbonates of Metals
Activity: Fit a bent tube in a rubber cork. Take some lime water in a test tube and keep it handy. Take some baking soda in another test tube and add some lemon juice to it. Immediately fit the bent tube over it. Insert its other end into the lime water. Note down your observations of both test tubes. Repeat the procedure using washing soda, and vinegar and dilute HCl properly. What do you see?

In this activity, when limewater comes in contact with the gas released in the form of effervescence, it turns milky. This is a chemical test for carbon dioxide gas. When lime water turns milky, we infer that the effervescence is of carbon dioxide gas. This gas is produced by the reaction of acids with carbonate and bicarbonate salts of metals. A precipitate of CaCO₃ is produced in its reaction with the limewater Ca(OH)₂. This reaction can be represented by the following chemical equation.
Ca(OH)₂ (aq) + CO₂ (g) → CaCO₃ (s) + H₂O (l)

Salts

Types of Salts: Acidic, Basic and Neutral Salts
Activity: Prepare 10 ml aqueous solutions from 1gm each of sodium chloride, ammonium chloride, and sodium bicarbonate. Measure the pH of each solution using pH paper. Are the values the same for all three? Classify the salts based on the pH values. We have seen that salts are formed by the reaction between acids and bases. Though this reaction is called a neutralization reaction, the resulting salts are not always neutral. A neutral salt is formed by the neutralization of a strong acid by a strong base. The aqueous solution of a neutral salt has a pH equal to 7.

An acidic salt is formed by the neutralization reaction between a strong acid and a weak base. The pH of the aqueous solution of an acidic salt is less than 7. On the contrary, a basic salt is formed by a neutralization reaction between a weak acid and a strong base. The pH of an aqueous solution of such a basic salt is greater than 7. Classify the following salts into the types acidic, basic, and neutral. Sodium sulphate, potassium chloride, ammonium nitrate, sodium carbonate, sodium acetate, sodium chloride.

Water of Crystallisaton
Activity: Take some crystals of blue vitriol in two test tubes. Add some water to one test tube and shake it. What did you see? What is the colour of the solution formed? Heat the other test tube on the low flame of a burner. What did you see? What change did occur in the colour of blue vitriol? What did you see in the upper part of the test tube? When the second test tube cools down add some water in it and shake. What is the colour of the resulting solution? What inference can be drawn from this observation?

On heating, the crystalline structure of blue vitriol broke down to form a colourless powder and water came out. This water was part of the crystal structure of blue vitriol. It is called water of crystallization. On adding water to the white powder a solution was formed which had the same colour as the solution in the first test tube. From this, we come to know that no chemical change has occurred in the crystals of blue vitriol due to heating. Losing water on heating blue vitriol, breaking down of the crystal structure, losing blue color, and regaining blue color on adding water are all physical changes. Repeat the above activity for Ferrous sulphate, and sodium carbonate and write chemical equations.

Apparatus: Evaporating dish, Bunsen burner, tripod stand, wire gauze, etc.
Chemicals: Alum.
Procedure: Take a small stone of alum in the evaporating dish. Keep the dish on the tripod stand and heat it with the help of a burner. What did you see in the dish? What is meant by puffed alum?
Ionic compounds are crystalline. These crystals are formed as a result of a definite arrangement of ions. In the crystals of some compounds, water molecules are also included in this arrangement. That is the water of crystallization. The water of crystallization is present in a definite proportion of the chemical formula of the compound. It is indicated in the chemical formula as shown below.

• Crystalline Blue Vitriol – CuSO₄.5H₂O
• Crystalline Ferrous Sulphate (Green Vitriol) – FeSO₄.7H₂O
• Crystalline Washing Soda – Na₂CO₃.10H₂O
• Crystalline Alum – K₂SO₄.Al₂(SO₄)₃.24H₂O
• Crystalline substances contain water for crystallization.
• The molecules of water of crystallization are part of the internal arrangement of the crystal.
• On heating or just by keeping, the water of crystallization is lost and the crystalline shape of that part is lost.

Ionic Compounds and Electrical Conductivity
Activity: Prepare a solution of 1g sodium chloride in 50ml water. Take two electrical wires. Connect one wire to the positive terminal of a 6V battery. While connecting the other wire to the negative terminal of the battery, include one switch and one holder with an electric bulb. Remove the insulating cladding from the 3 cm portion of the other free ends of the two wires. Take the salt solution in a 100ml capacity beaker and immerse the uncovered ends of the two wires in it keeping the wire erect with the help of a support. Switch on the current. Note whether the bulb glows. Repeat the same procedure using solutions of 1g copper sulphate, 1g glucose, 1g urea, 5 ml dilute H₂SO₄, and 5 ml dilute NaOH each in 50 ml water. Record your observations in a table. (Do not forget to clean the beaker and uncovered part of the wires with water, every time you change the solution.)
1. With which solutions did the bulb glow?
2. Which solutions are electrical conductors?

The bulb glows only when an electric current passes through it. And this can happen only when the electric circuit is complete. In the above activity, the circuit is found to be complete when the aqueous solutions of NaCl, CuSO₄, H₂SO₄, and NaOH are used. It means that these solutions are conductors of electricity. Electrons conduct electricity through electrical wires, and ions conduct electricity through a liquid or a solution. Electrons leave the battery at the negative terminal, complete the electric circuit, and enter the battery at the positive terminal. When there is a liquid or a solution in the circuit, two rods, wires, or plates are immersed in it. These are called electrodes. Electrodes are usually made of a conducting solid. The electrode connected to the negative terminal of a battery using a conducting wire is called a cathode and the electrode connected to the positive terminal of a battery is called an anode. Why does the electric circuit get completed by immersing the electrodes in certain liquids or solutions? To understand this phenomenon, let us look more closely at the solutions in the above activity, which were found to be electrical conductors.

Dissociation of Ions and Electrical Conductivity
In the above activity, it was found that the aqueous solutions of the compounds NaCl, CuSO₄, H₂SO₄, and NaOH are electricity conductors. Out of these NaCl and CuSO₄ are salts, H₂SO₄ is a strong acid and NaOH is a strong base. We have seen that salts, strong acids, and strong bases dissociate almost completely in their aqueous solutions. Therefore, the aqueous solutions of all these three contain large numbers of cations and anions.

A characteristic of the liquid state is the mobility of its particles. Due to this mobility, the positively charged cations in the solution are attracted toward the negative electrode or cathode and move toward the cathode; on the other hand, the negatively charged anions move in the direction of the anode. The movement of ions in the solution towards the respective electrodes amounts to the conduction of electricity through the solution. From this, you will understand that those liquids or solutions that contain a large number of dissociated ions conduct electricity.

Electrolysis
Procedure: Take a solution of 1g copper sulphate in 50 ml water in a 100 ml capacity beaker. Use a thick plate of copper as an anode and a carbon rod as a cathode. Arrange the apparatus as shown in the figure and pass an electric current through the circuit for some time. Do you see any changes?

In the above activity, copper appears to have deposited on the portion of the cathode immersed in the solution. How did this happen? When an electric current started flowing through the circuit, the cations, that is, Cu⁺⁺ ions in the solution got attracted toward the cathode. Cu atoms are formed when electrons coming out from the cathode combine with the Cu⁺⁺ ions. A deposit of the copper appeared on the cathode.

Even though the Cu⁺⁺ ions in the solution were used up in this manner, the colour of the solution remained the same. Because, while the electric current was on, electrons were removed from the Cu atoms of the anode and sent to the battery through the electric wire. The Cu⁺⁺ ions formed in this manner entered the solution. In this way, decomposition of the solute in the solution took place due to the electric current. This is called electrolysis. There are two parts to the electrolysis process. These are the cathode reaction and the anode reaction. The two parts of the electrolysis process that take place in the above activity are shown below.

Cathode Reaction: Cu²⁺ (aq) + 2e^– → Cu(s)
Anode Reaction: Cu (s) → Cu²⁺ (aq) + 2e^–

The liquid/solution must have a large number of dissociated ions for electrolysis to take place. Therefore, substances that undergo dissociation to a great extent in the liquid state or a solution are called electrolytes. Salts, strong acids, and strong bases are electrolytes. Their solutions have high electrical conductivity. In other words, electrolytes are good conductors of electricity in their liquid or solution state. An assembly that consists of a container electrolyte and the electrodes dipped in it, is called an electrolytic cell.

If pure water is used in an electrolytic cell, current does not flow even on putting on the switch. From this, we learn that pure water is a bad conductor of electricity. And we have already seen the reason behind this. The concentration of H⁺ and OH^– ions formed by dissociation of water is very low, only 1 × 10^-7 mol/L for each ion. However, the electrical conductivity of water increases by mixing a small amount of salt or a strong acid/base in it due to their dissociation and electrolysis of water taking place.

Electrolysis of Water
Activity: Dissolve 2g salt in 500 ml pure water. Take 250 ml of this solution in a 500 ml capacity beaker. Connect two electrical wires to the positive and negative terminals of a power supply. Remove the insulating cladding from about 2 cm portions at the other ends of the wires. These are the two electrodes. Fill two test tubes upto the brim with the prepared dilute salt solution. Invert them on the electrodes without allowing any air to enter. Start the electric current under 6V potential difference from the power supply. Observe what happens in the test tubes after some time.

It is found in the above activity that the volume of the gas formed near the cathode is double that of the gas formed near the anode. Scientists have shown that hydrogen gas is formed near the cathode and oxygen gas near the anode. From this, it is clear that electrolysis of water has taken place and its constituent elements have been released. The concerned electrode reactions are as follows.

Cathode Reaction: 2H₂O (l) + 2e^– → H₂ (g) + 2OH^– (aq)
Anode Reaction: 2H₂O (l) → O₂ (g) + 4H⁺ (aq) + 4e^–

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