Sodium Carbonate, Sodium Chloride, Sodium Hydroxide — Explained

On this page

1. 1. Sodium Chloride (NaCl)
2. Key Principles/Laws:
3. Preparation/Extraction:
4. Purification of Crude Salt:
5. Physical Properties:
6. Chemical Properties:
7. Uses:
8. 2. Sodium Hydroxide (NaOH)
9. Key Principles/Laws:
10. Preparation (Chlor-alkali Process):
11. Process Details:
12. Products and Separation:
13. Physical Properties:
14. Chemical Properties:
15. Uses:
16. 3. Sodium Carbonate ($\text{Na}2\text{CO}3$)
17. Key Principles/Laws:
18. Preparation (Solvay Process / Ammonia-Soda Process):
19. Steps of the Solvay Process:
20. Physical Properties:
21. Chemical Properties:
22. Uses:
23. Common Misconceptions & NEET-Specific Angle:

Detailed Explanation

Let's delve deeper into the preparation, properties, and applications of these three crucial sodium compounds: Sodium Chloride, Sodium Hydroxide, and Sodium Carbonate.

1. Sodium Chloride (NaCl)

Conceptual Foundation: Sodium chloride is the most common ionic compound, formed by the electrostatic attraction between $\text{Na}^+$ and $\text{Cl}^-$ ions. Its high lattice energy contributes to its stability and high melting point. It's a neutral salt, meaning its aqueous solution has a pH of approximately 7.

Key Principles/Laws:

Ionic Bonding: — Formation of $\text{Na}^+$ and $\text{Cl}^-$ ions and their electrostatic attraction.
Solubility: — Governed by the balance between lattice energy and hydration energy. $\text{NaCl}$ is highly soluble in water due to the strong hydration of its ions.

Preparation/Extraction:

From Seawater: — This is the most common method. Seawater contains approximately 2.7-2.9% $\text{NaCl}$ by mass. Large shallow ponds are used to allow solar evaporation of water, leaving behind crude salt. This crude salt contains impurities like $\text{CaSO}_4$, $\text{MgCl}_2$, and $\text{CaCl}_2$.
From Underground Deposits (Rock Salt): — Large deposits of solid $\text{NaCl}$ are found in many parts of the world, formed from ancient dried-up seas. This rock salt is mined like coal.

Purification of Crude Salt:

Crude salt is dissolved in a minimum amount of water, and then filtered to remove insoluble impurities. The solution is then saturated with hydrogen chloride gas ($\text{HCl}$). Due to the common ion effect (presence of $\text{Cl}^-$ from $\text{HCl}$), the solubility of $\text{NaCl}$ decreases significantly, causing pure $\text{NaCl}$ to precipitate out. The more soluble impurities like $\text{MgCl}_2$ and $\text{CaCl}_2$ remain in the solution. This purified salt is then filtered and dried.

Physical Properties:

White crystalline solid.
Melting point: $801^\circ\text{C}$.
Boiling point: $1413^\circ\text{C}$.
Highly soluble in water (approx. $36\,\text{g}$ per $100\,\text{mL}$ at $20^\circ\text{C}$). Its solubility does not change significantly with temperature.
Slightly soluble in alcohol.

Chemical Properties:

Stability: — Thermally stable.
Reactions: — Primarily acts as a source of $\text{Na}^+$ and $\text{Cl}^-$ ions. For example, with concentrated $\text{H}_2\text{SO}_4$ at high temperatures, it produces $\text{HCl}$ gas:

$$\text{NaCl} + \text{H}_2\text{SO}_4 \xrightarrow{\text{Heat}} \text{NaHSO}_4 + \text{HCl}$$

$$\text{NaCl} + \text{NaHSO}_4 \xrightarrow{\text{Higher Heat}} \text{Na}_2\text{SO}_4 + \text{HCl}$$

Uses:

Dietary: — Essential component of food, acts as a preservative.
Chemical Industry: — Primary raw material for the manufacture of $\text{NaOH}$, $\text{Na}_2\text{CO}_3$, $\text{NaHCO}_3$, $\text{Cl}_2$, $\text{H}_2$, etc.
Refrigeration: — Used in freezing mixtures with ice.
Medicine: — Used in saline solutions.

2. Sodium Hydroxide (NaOH)

Conceptual Foundation: Sodium hydroxide is a strong electrolyte and a strong base. Its highly corrosive nature stems from its ability to readily donate hydroxide ions, which can hydrolyze proteins and fats.

Key Principles/Laws:

Arrhenius Base: — Produces $\text{OH}^-$ ions in aqueous solution.
Electrolysis: — Decomposition of an ionic compound using electrical energy.

Preparation (Chlor-alkali Process):

Sodium hydroxide is primarily manufactured by the electrolysis of an aqueous solution of sodium chloride (brine). This process is called the Chlor-alkali process because of the products formed: chlorine (chlor) and alkali (sodium hydroxide).

Process Details:

An aqueous solution of $\text{NaCl}$ (brine) is electrolyzed using a diaphragm cell or a mercury cell.

At Anode (Oxidation): — Chloride ions are oxidized to chlorine gas.

$$2\text{Cl}^- (\text{aq}) \rightarrow \text{Cl}_2 (\text{g}) + 2\text{e}^-$$

At Cathode (Reduction): — Water molecules are reduced to hydrogen gas and hydroxide ions.

$$2\text{H}_2\text{O} (\text{l}) + 2\text{e}^- \rightarrow \text{H}_2 (\text{g}) + 2\text{OH}^- (\text{aq})$$

Overall Reaction:

$$2\text{NaCl} (\text{aq}) + 2\text{H}_2\text{O} (\text{l}) \xrightarrow{\text{Electrolysis}} 2\text{NaOH} (\text{aq}) + \text{Cl}_2 (\text{g}) + \text{H}_2 (\text{g})$$

Products and Separation:

$\text{NaOH}$: — Formed at the cathode compartment. The solution is concentrated by evaporation to obtain solid $\text{NaOH}$.
$\text{Cl}_2$: — Collected at the anode.
$\text{H}_2$: — Collected at the cathode.

Physical Properties:

White, translucent, deliquescent solid.
Melting point: $318^\circ\text{C}$.
Highly soluble in water, with significant heat evolution (exothermic dissolution).
Also soluble in ethanol and methanol.

Chemical Properties:

Strong Base: — Neutralizes acids to form salt and water.

$$\text{NaOH} + \text{HCl} \rightarrow \text{NaCl} + \text{H}_2\text{O}$$

Reaction with Acidic Oxides: — Reacts with non-metal oxides (acidic oxides) like $\text{CO}_2$, $\text{SO}_2$.

$$2\text{NaOH} + \text{CO}_2 \rightarrow \text{Na}_2\text{CO}_3 + \text{H}_2\text{O}$$

Reaction with Amphoteric Metals/Oxides: — Reacts with metals like $\text{Al}$, $\text{Zn}$ and their oxides/hydroxides.

$$2\text{Al} + 2\text{NaOH} + 2\text{H}_2\text{O} \rightarrow 2\text{NaAlO}_2 (\text{Sodium meta-aluminate}) + 3\text{H}_2$$

Saponification: — Hydrolyzes esters (fats/oils) to form soaps and glycerol.

Uses:

Soap and Detergent Industry: — Key ingredient in soap making.
Pulp and Paper Industry: — Used in pulping wood.
Textile Industry: — Mercerizing cotton (improving strength and luster).
Petroleum Refining: — Removing sulfur compounds.
Bauxite Purification: — In the Bayer process for extracting alumina from bauxite.
Laboratory Reagent: — Common strong base.

3. Sodium Carbonate ($\text{Na}_2\text{CO}_3$)

Conceptual Foundation: Sodium carbonate is a salt of a strong base ($\text{NaOH}$) and a weak acid ($\text{H}_2\text{CO}_3$). Consequently, its aqueous solution is alkaline due to the hydrolysis of the carbonate ion.

Key Principles/Laws:

Hydrolysis of Salts: — $\text{CO}_3^{2-}$ reacts with water to produce $\text{HCO}_3^-$ and $\text{OH}^-$, making the solution basic.

$$\text{CO}_3^{2-} (\text{aq}) + \text{H}_2\text{O} (\text{l}) \rightleftharpoons \text{HCO}_3^- (\text{aq}) + \text{OH}^- (\text{aq})$$

Solvay Process: — An elegant industrial process that recycles ammonia, making it economically viable.

Preparation (Solvay Process / Ammonia-Soda Process):

This is the most important industrial method for producing sodium carbonate. The raw materials are common salt ($\text{NaCl}$), limestone ($\text{CaCO}_3$), and ammonia ($\text{NH}_3$).

Steps of the Solvay Process:

1
Ammoniation of Brine: — Saturated brine solution ($\text{NaCl}$) is saturated with ammonia gas ($\text{NH}_3$).

$$\text{NaCl} (\text{aq}) + \text{NH}_3 (\text{g}) + \text{H}_2\text{O} (\text{l}) \rightarrow \text{Ammoniated Brine}$$

1
Carbonation: — The ammoniated brine is then carbonated by passing carbon dioxide gas ($\text{CO}_2$) through it. $\text{CO}_2$ is obtained by heating limestone ($\text{CaCO}_3$).

$$\text{CaCO}_3 (\text{s}) \xrightarrow{\text{Heat}} \text{CaO} (\text{s}) + \text{CO}_2 (\text{g})$$

The $\text{CO}_2$ reacts with ammonia and water to form ammonium bicarbonate:

$$\text{NH}_3 (\text{g}) + \text{H}_2\text{O} (\text{l}) + \text{CO}_2 (\text{g}) \rightarrow \text{NH}_4\text{HCO}_3 (\text{aq})$$

Ammonium bicarbonate then reacts with sodium chloride to form sodium bicarbonate, which is sparingly soluble and precipitates out:

$$\text{NH}_4\text{HCO}_3 (\text{aq}) + \text{NaCl} (\text{aq}) \rightarrow \text{NaHCO}_3 (\text{s}) \downarrow + \text{NH}_4\text{Cl} (\text{aq})$$

1
Filtration and Heating of Sodium Bicarbonate: — The precipitated sodium bicarbonate ($\text{NaHCO}_3$) is filtered, washed, and then heated to produce sodium carbonate (soda ash).

$$2\text{NaHCO}_3 (\text{s}) \xrightarrow{\text{Heat}} \text{Na}_2\text{CO}_3 (\text{s}) + \text{H}_2\text{O} (\text{g}) + \text{CO}_2 (\text{g})$$

The $\text{CO}_2$ released here is recycled back into the carbonation step.

1
Ammonia Recovery: — The ammonium chloride ($\text{NH}_4\text{Cl}$) solution from step 2 is treated with calcium hydroxide ($\text{Ca(OH)}_2$), which is obtained by slaking quicklime ($\text{CaO}$) from step 2. This regenerates ammonia, which is recycled.

$$\text{CaO} (\text{s}) + \text{H}_2\text{O} (\text{l}) \rightarrow \text{Ca(OH)}_2 (\text{aq})$$

$$2\text{NH}_4\text{Cl} (\text{aq}) + \text{Ca(OH)}_2 (\text{aq}) \rightarrow 2\text{NH}_3 (\text{g}) + \text{CaCl}_2 (\text{aq}) + 2\text{H}_2\text{O} (\text{l})$$

The $\text{NH}_3$ is recycled, making the process very efficient.

Physical Properties:

Anhydrous ($\text{Na}_2\text{CO}_3$): — White powder, melting point $851^\circ\text{C}$, called 'soda ash'.
Decahydrate ($\text{Na}_2\text{CO}_3 \cdot 10\text{H}_2\text{O}$): — White crystalline solid, commonly known as 'washing soda'. It is efflorescent, meaning it loses water of crystallization on exposure to air.

$$\text{Na}_2\text{CO}_3 \cdot 10\text{H}_2\text{O} (\text{s}) \xrightarrow{\text{Air}} \text{Na}_2\text{CO}_3 \cdot \text{H}_2\text{O} (\text{s}) + 9\text{H}_2\text{O} (\text{g})$$

Highly soluble in water, forming an alkaline solution.

Chemical Properties:

Alkaline Solution: — Due to hydrolysis of carbonate ion.
Reaction with Acids: — Reacts with acids to produce $\text{CO}_2$ gas.

$$\text{Na}_2\text{CO}_3 (\text{aq}) + 2\text{HCl} (\text{aq}) \rightarrow 2\text{NaCl} (\text{aq}) + \text{H}_2\text{O} (\text{l}) + \text{CO}_2 (\text{g})$$

Water Softening: — Precipitates $\text{Ca}^{2+}$ and $\text{Mg}^{2+}$ ions as carbonates, thus removing hardness from water.

$$\text{CaSO}_4 (\text{aq}) + \text{Na}_2\text{CO}_3 (\text{aq}) \rightarrow \text{CaCO}_3 (\text{s}) \downarrow + \text{Na}_2\text{SO}_4 (\text{aq})$$

Uses:

Glass Industry: — Used in large quantities to lower the melting point of silica.
Detergents and Soaps: — As a builder and cleaning agent.
Water Softening: — Removes temporary and permanent hardness of water.
Paper Industry: — Used in pulping.
Textile Industry: — Used in dyeing and bleaching.
Manufacture of other Sodium Compounds: — Like borax, caustic soda, etc.

Common Misconceptions & NEET-Specific Angle:

$\text{NaCl}$ purity: — Students often forget the $\text{HCl}$ gas method for purification of crude salt. This is a common NEET question point.
Chlor-alkali products: — Remember all three products ($\text{NaOH}$, $\text{Cl}_2$, $\text{H}_2$) and their respective uses. The environmental impact of mercury cells (though largely phased out) is also a conceptual point.
Solvay process intermediates: — Understanding the role of $\text{NH}_4\text{HCO}_3$ and the precipitation of $\text{NaHCO}_3$ due to its low solubility is key. The recycling of $\text{NH}_3$ and $\text{CO}_2$ is a highlight of its efficiency. $\text{CaCl}_2$ is a byproduct, which has limited commercial value, making it a disadvantage of the process.
Hydrates of $\text{Na}_2\text{CO}_3$: — Differentiating between soda ash ($\text{Na}_2\text{CO}_3$) and washing soda ($\text{Na}_2\text{CO}_3 \cdot 10\text{H}_2\text{O}$) and understanding efflorescence is important.
Nature of solutions: — $\text{NaCl}$ solution is neutral, $\text{NaOH}$ solution is strongly basic, and $\text{Na}_2\text{CO}_3$ solution is basic (due to hydrolysis). These pH differences are frequently tested.

Often confused with

Side-by-side differences the NEET paper likes to test.

Sodium Carbonate, Sodium Chloride, Sodium Hydroxide vs Sodium Carbonate vs. Sodium Bicarbonate

Aspect	Sodium Carbonate, Sodium Chloride, Sodium Hydroxide	Sodium Carbonate vs. Sodium Bicarbonate
Chemical Formula	$\text{Na}_2\text{CO}_3$ (anhydrous) or $\text{Na}_2\text{CO}_3 \cdot 10\text{H}_2\text{O}$ (decahydrate)	$\text{NaHCO}_3$
Common Name	Washing Soda (decahydrate), Soda Ash (anhydrous)	Baking Soda, Cooking Soda
Nature in Solution	Strongly alkaline (pH approx. 11-12 for typical concentrations)	Mildly alkaline (pH approx. 8-9 for typical concentrations)
Thermal Decomposition	Stable at high temperatures (anhydrous form). Decahydrate loses water first.	Decomposes readily on heating to produce $\text{Na}_2\text{CO}_3$, $\text{H}_2\text{O}$, and $\text{CO}_2$. $2\text{NaHCO}_3 \xrightarrow{\text{Heat}} \text{Na}_2\text{CO}_3 + \text{H}_2\text{O} + \text{CO}_2$
Primary Uses	Glass manufacturing, detergents, water softening, paper industry.	Baking (leavening agent), antacid, fire extinguishers, mild abrasive.
Solubility in Water	Highly soluble	Less soluble than $\text{Na}_2\text{CO}_3$, especially in the presence of $\text{NH}_4\text{Cl}$ (Solvay process).

Sodium carbonate ($\text{Na}_2\text{CO}_3$) and sodium bicarbonate ($\text{NaHCO}_3$) are both sodium salts of carbonic acid, but they differ significantly in their chemical properties and uses. Sodium carbonate is a stronger base and is primarily used in heavy industries like glass and detergents, as well as for water softening.

It is thermally stable as an anhydrous compound. Sodium bicarbonate, on the other hand, is a milder base, commonly known as baking soda, and is used as a leavening agent due to its thermal decomposition producing $\text{CO}_2$ gas.

It also acts as an antacid. Their differing solubilities and thermal stabilities are key to their industrial production and applications.

Why it is tested: For NEET, understanding the distinct properties, particularly their basicity, thermal stability, and primary applications, is crucial. Questions often test the products of their decomposition or their roles in specific industrial processes (e.g., Solvay process for $\text{Na}_2\text{CO}_3$, baking for $\text{NaHCO}_3$). The difference in their basicity and how it relates to their hydrolysis in water is also a common conceptual point.

Questions students ask

6 answered on this topic.

Why is sodium chloride purified using $\text{HCl}$ gas?

Crude sodium chloride obtained from seawater or rock salt contains impurities like $\text{CaCl}_2$ and $\text{MgCl}_2$, which are deliquescent and make the salt sticky. To purify it, crude salt is dissolved in minimal water, and then $\text{HCl}$ gas is passed through the saturated solution.

This works on the principle of the common ion effect. The added $\text{HCl}$ increases the concentration of $\text{Cl}^-$ ions, shifting the solubility equilibrium of $\text{NaCl}$ to the left, causing pure $\text{NaCl}$ to precipitate out.

The impurities, being more soluble, remain in the solution.

What is the Chlor-alkali process, and what are its main products?

The Chlor-alkali process is an industrial method for producing sodium hydroxide, chlorine gas, and hydrogen gas by the electrolysis of an aqueous solution of sodium chloride (brine). The name 'Chlor-alkali' refers to chlorine and the alkali metal hydroxide (sodium hydroxide) produced. The main products are $\text{NaOH}$ (at cathode), $\text{Cl}_2$ (at anode), and $\text{H}_2$ (at cathode). Each of these products has significant industrial applications, making this process highly valuable.

Explain the role of ammonia in the Solvay process.

Ammonia plays a crucial role in the Solvay process. First, it reacts with $\text{CO}_2$ and water to form ammonium bicarbonate ($\text{NH}_4\text{HCO}_3$). This ammonium bicarbonate then reacts with $\text{NaCl}$ to precipitate sodium bicarbonate ($\text{NaHCO}_3$).

Crucially, ammonia is regenerated at the end of the process from ammonium chloride ($\text{NH}_4\text{Cl}$) by reacting it with calcium hydroxide ($\text{Ca(OH)}_2$). This regeneration makes the Solvay process highly economical and environmentally efficient, as ammonia is a relatively expensive raw material.

Why is an aqueous solution of sodium carbonate alkaline?

Sodium carbonate ($\text{Na}_2\text{CO}_3$) is a salt formed from a strong base ($\text{NaOH}$) and a weak acid ($\text{H}_2\text{CO}_3$). When dissolved in water, it dissociates into $\text{Na}^+$ and $\text{CO}_3^{2-}$ ions.

The $\text{Na}^+$ ions are spectator ions, but the carbonate ions ($\text{CO}_3^{2-}$) are the conjugate base of a weak acid. They react with water (hydrolyze) to produce bicarbonate ions ($\text{HCO}_3^-$) and hydroxide ions ($\text{OH}^-$), as shown: $\text{CO}_3^{2-} (\text{aq}) + \text{H}_2\text{O} (\text{l}) \rightleftharpoons \text{HCO}_3^- (\text{aq}) + \text{OH}^- (\text{aq})$.

The excess $\text{OH}^-$ ions in the solution make it alkaline.

What is the difference between soda ash and washing soda?

Soda ash refers to anhydrous sodium carbonate ($\text{Na}_2\text{CO}_3$), which is a white powder. It is typically obtained by heating sodium bicarbonate or by dehydrating washing soda. Washing soda, on the other hand, is the decahydrate form of sodium carbonate, $\text{Na}_2\text{CO}_3 \cdot 10\text{H}_2\text{O}$.

It is a white crystalline solid and is efflorescent, meaning it loses water of crystallization when exposed to air. Both are used for similar purposes, but washing soda is the common form used in households for cleaning and water softening.

How does sodium carbonate help in softening hard water?

Hard water contains dissolved salts of calcium and magnesium, primarily as bicarbonates, chlorides, or sulfates. Sodium carbonate helps soften water by reacting with these dissolved calcium ($\text{Ca}^{2+}$) and magnesium ($\text{Mg}^{2+}$) ions to form insoluble calcium carbonate ($\text{CaCO}_3$) and magnesium carbonate ($\text{MgCO}_3$).

These insoluble carbonates precipitate out of the water, effectively removing the hardness-causing ions. For example: $\text{CaSO}_4 (\text{aq}) + \text{Na}_2\text{CO}_3 (\text{aq}) \rightarrow \text{CaCO}_3 (\text{s}) \downarrow + \text{Na}_2\text{SO}_4 (\text{aq})$.

The softened water is then suitable for washing and other uses.