Baking Soda - Preparation, Uses, Structure, Properties, FAQs
Have you ever wondered what is the use of baking soda? Why is it present in our kitchen? What makes it a key player not just in the kitchen, not just in cleaning, personal care, and even medicine? From helping dough rise to neutralizing odors, baking soda, or sodium bicarbonate, seems to do it all. You will get these answers after reading this article on Baking Soda.
This Story also Contains
- Chemical Name of Baking Soda
- Preparation of Baking Soda
- Properties of Baking Soda
- Structure of Baking Soda
- Baking Soda Uses
- Some Solved Examples
Ever wonder how cakes become fluffy, how biscuits puff up while baking, how stubborn stains are removed from clothes, or how a sour stomach soothens? The only answer to all these is a white powder called Baking soda, also known as Sodium Hydrogen Carbonate. This compound is widely used in industries, households, and laboratories. It reacts with readily available acids like lemon and curd, as it is a mild alkali, and releases carbon dioxide gas. Baking soda is also used in cleansing, fire extinguishers, deodorising, and as medicine. It is a non-toxic and biodegradable compound. It is the basic ingredient of every kitchen.
Chemical Name of Baking Soda
The chemical compound sodium bicarbonate formula, sometimes known as baking soda formula or bicarbonate of baking soda chemical formula, has the formula $\mathrm{NaHCO}_3$. A sodium cation (Na+) and a bicarbonate anion $\left(\mathrm{HCO}_3{ }^{-}\right)$ make up this salt. Sodium bicarbonate is a crystalline white substance that frequently appears as a fine powder. It tastes slightly salty and alkaline, similar to washing soda (sodium carbonate). The chemical name of baking soda is sodium hydrogen carbonate.
Nahcolite is the natural mineral form. It is found dissolved in many mineral springs as a component of the mineral natron. Sodium Bicarbonate's common name is baking soda or the chemical name of baking soda is sodium bicarbonate. Because of its long history and widespread use, baking soda, bread soda, cooking soda, and bicarbonate of soda are all common names for the salt, which can often be purchased beside baking powder in supermarkets.
Preparation of Baking Soda
The Solvay process is used to make sodium bicarbonate as well as sodium carbonate. Carbon dioxide, water, ammonia, as well as concentrated brine solution are employed as raw materials in this process. The important chemical reaction used in the production of baking soda (sodium hydrogen carbonate) and sodium carbonate is:
$\mathrm{CO}_2+\mathrm{H}_2 \mathrm{O}+\mathrm{NH}_3+\mathrm{NaCl} \rightarrow \mathrm{NaHCO}_3+\mathrm{NH}_4 \mathrm{Cl}$
$2 \mathrm{NaHCO}_3 \rightarrow \mathrm{Na}_2 \mathrm{CO}_3+\mathrm{CO}_2+\mathrm{H}_2 \mathrm{O}$
The carbon dioxide produced is recycled to make $\mathrm{NaHCO}_3$.
Read more :
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Commonly Asked Questions
Baking soda is the common name for sodium bicarbonate (NaHCO3). It's prepared industrially through the Solvay process, which involves reacting sodium chloride, ammonia, and carbon dioxide in water to produce sodium bicarbonate and ammonium chloride. The baking soda is then separated through filtration and purification steps.
Baking soda reacts with stomach acid (HCl) according to the equation:
$\mathrm{NaHCO}_3(a q)+\mathrm{HCl}(a q) \rightarrow \mathrm{NaCl}(a q)+\mathrm{H}_2 \mathrm{O}(l)+\mathrm{CO}_2(g)$
This reaction produces sodium chloride (NaCl), water (H₂O), and carbon dioxide (CO₂) gas.
It is important for Neutralizing Excess Stomach Acid, Temporary Relief from Acid-Related Issues , Carbon Dioxide Production.
In cooking, baking soda reacts with acidic ingredients (like buttermilk, yogurt, or vinegar) to produce carbon dioxide gas. This reaction not only helps leaven baked goods but also neutralizes some of the acid, affecting the flavor and texture of the final product. This is why recipes often balance acidic ingredients with baking soda.
Baking soda is added to toothpaste for several reasons:
Mild Abrasive: It helps scrub away plaque and surface stains from teeth without damaging enamel.
Neutralizes Acidity: It neutralizes acids in the mouth, helping to freshen breath and reduce tooth decay.
Whitening Effect: Its abrasive properties contribute to a whiter smile by removing surface stains.
Baking soda's thermal stability is due to its ionic structure. The strong ionic bonds between the sodium cation (Na+) and bicarbonate anion (HCO3-) require significant energy to break. However, when heated above about 50°C, it begins to slowly decompose, and at around 200°C, it decomposes more rapidly into sodium carbonate, water, and carbon dioxide.
Properties of Baking Soda
- It is non-combustible.
- Powder dust is not as explosive as other types of dust.
- It has a melting point of 500°C and is an odourless white crystalline solid.
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Related Topics Link, |
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Sodium bicarbonate |
NaHCO3 |
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Molar Mass |
84.0066 g/ mol |
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Boiling Point |
851°C |
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Melting Point |
50°C |
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Density |
Solids: 2.20 g/cm3 |
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It is basic in nature.
$\mathrm{NaHCO}_3+\mathrm{H}_2 \mathrm{O} \rightarrow \mathrm{H}_2 \mathrm{CO}_3+\mathrm{NaOH}$
$\mathrm{H}_2 \mathrm{CO}_3 \rightarrow \mathrm{H}_2 \mathrm{O}+\mathrm{CO}_2$
The pH of baking soda is 8.3.
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Baking soda is sparingly soluble in water.
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NaHCO3 crystallizes in a monoclinic crystal lattice.
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When sodium bicarbonate is heated, it decomposes into sodium carbonate, water, and carbon dioxide gas. At temperatures exceeding 80°C, thermal decomposition occurs.
$2 \mathrm{NaHCO}_3 \rightarrow \mathrm{Na}_2 \mathrm{CO}_3+\mathrm{CO}_2+\mathrm{H}_2 \mathrm{O}$
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Baking soda produces carbon dioxide gas when it combines with acids. The following is the chemical reaction that occurs:
$\mathrm{NaHCO}_3+\mathrm{H}^{+} \rightarrow \mathrm{Na}^{+}+\mathrm{H}_2 \mathrm{O}+\mathrm{CO}_2$
Baking soda is mined as well as manufactured in factories. In its mineral form, it is called nahcolite.
$\mathrm{Na}_2 \mathrm{CO}_3+\mathrm{CO}_2+\mathrm{H}_2 \mathrm{O} \rightarrow 2 \mathrm{NaHCO}_3$
Commonly Asked Questions
When baking soda is heated, it undergoes thermal decomposition. The reaction is:
$2 \mathrm{NaHCO}_3(s) \xrightarrow{\Delta} \mathrm{Na}_2 \mathrm{CO}_3(s)+\mathrm{CO}_2(g)+\mathrm{H}_2 \mathrm{O}(g)$
Yes, when baking soda (NaHCO3) dissolves in water, it dissociates into sodium ions (Na+) and bicarbonate ions (HCO3-). These ions can carry an electric current, making the solution conductive. This property is common to many ionic compounds when dissolved in water.
Baking soda is amphoteric because it can act as both an acid and a base, depending on the reaction conditions. It can accept protons (act as a base) or donate protons (act as an acid) in chemical reactions, making it versatile in various applications.
A solution of baking soda in water is slightly alkaline. At room temperature, a 0.1 molar solution of baking soda typically has a pH around 8.3. This mild alkalinity contributes to its effectiveness in neutralizing acids and its use in various applications.
Baking soda reacts with vinegar (acetic acid) to produce sodium acetate, water, and carbon dioxide gas. The reaction is:
$\mathrm{NaHCO}_3(s)+\mathrm{CH}_3 \mathrm{COOH}(a q) \rightarrow \mathrm{CH}_3 \mathrm{COONa}(a q)+\mathrm{H}_2 \mathrm{O}(l)+\mathrm{CO}_2(g)$
What Happens:
Carbon Dioxide Gas (CO₂): The bubbling or fizzing from the release of gas makes the reaction visually dramatic.
Water (H₂O): Produced as a byproduct of the acid-base neutralization.
Sodium Acetate (CH₃COONa): A salt that dissolves in water.
Structure of Baking Soda
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The chemical formula for sodium bicarbonate is NaHCO3.
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It is made up of the sodium cation (Na+) and the bicarbonate anion (HCO3-).
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Its lattice structure is monoclinic.
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One sodium atom, one carbon atom, one hydrogen atom, and three oxygen atoms make up this compound.
NCERT Chemistry Notes:
Commonly Asked Questions
The structure of baking soda (NaHCO3) consists of a sodium ion (Na+) and a bicarbonate ion (HCO3-). This ionic structure allows it to dissolve easily in water and participate in acid-base reactions. The presence of both hydrogen and carbonate in the bicarbonate ion contributes to its amphoteric nature.
Baking soda (NaHCO3) is less alkaline than sodium carbonate (Na2CO3, washing soda). Baking soda has one hydrogen atom, making it a bicarbonate, while washing soda has two sodium atoms. This results in different properties:
Baking soda helps relieve insect bites and stings due to its alkaline nature. Many insect venoms are acidic, so applying a paste of baking soda and water can help neutralize the venom, reducing pain and itching. Its mild anti-inflammatory properties also contribute to soothing the affected area.
The solubility of baking soda increases with temperature. At 0°C, about 6.9 grams of baking soda can dissolve in 100 mL of water, while at 20°C, this increases to about 9.6 grams. This property is important in various applications, including cooking and cleaning, where warm water can help dissolve baking soda more effectively.
Yes, baking soda is effective at removing odors from refrigerators. It works through a process called adsorption, where odor molecules stick to the surface of baking soda particles. Additionally, baking soda can neutralize acidic and basic odor-causing molecules through chemical reactions. Its large surface area and slightly alkaline nature make it particularly effective for this purpose.
Baking Soda Uses
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Baking soda has antifungal and antibacterial properties, making it an excellent natural solution to a variety of aesthetic problems. It is mildly abrasive, so it will exfoliate the face, feet, hands, and body softly.
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Baking soda is used as an antacid to treat indigestion and heartburn. Its fast action reduces stomach acid, providing temporary relief. Its alkaline composition helps to reduce indigestion by neutralising excess hydrochloric acid in the stomach.
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It is a household wonder chemical that is generally used as a cleaning agent, a cooking component, and a disinfectant.
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It is used to raise flour batter. Baking soda is used to make baking powder, which is made by mixing baking soda with a moderate acid like tartaric acid. In creating bread, cakes, cookies, pancakes, patties, and other baked goods, baking powder is used as a leavening agent (a chemical that releases a gas and causes dough to rise and expand).
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Baking soda can be used as a natural pesticide in the garden to kill dangerous insects and fungi that attack plants. It can be mixed into soil to raise the pH level and make the soil alkaline. Alkaline soils are preferred by several plants.
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Some Solved Examples
Question 1: An ingredient of baking powder is:
1) (correct) $\mathrm{NaHCO}_3$
2)$\mathrm{Na}_2 \mathrm{CO}_3$
3) $\mathrm{Na}_2 \mathrm{SO}_4$
4) NaCl
Solution: The Common name of Sodium bicarbonate $\left(\mathrm{NaHCO}_3\right)$ is baking powder.
Hence, the answer is option (1).
Question 2: Solvay's process is used for the preparation of sodium carbonate. Which among the following raw materials are used in Solvay's process?
1) (correct) $\mathrm{CaCO}_3, \mathrm{NH}_3, \mathrm{NaCl}$
2) $\mathrm{NaOH}, \mathrm{CO}_2$
3) $\mathrm{NaCl}, \mathrm{CaCO}_3, \mathrm{C}, \mathrm{H}_2 \mathrm{SO}_4$
4) $\mathrm{NH}_3, \mathrm{H}_2 \mathrm{O}, \mathrm{NaCl}$
Solution:
The raw materials used in solvay's process are: $\mathrm{CaCO}_3, \mathrm{NH}_3, \mathrm{NaCl}$
The following reactions take place during solvay's process.
First of all calcium carbonate is heated and decomposed into calcium oxide and carbon dioxide.
$\mathrm{CaCO}_3 \rightarrow \mathrm{CaO}+\mathrm{CO}_2$
Ammonia reacts with carbon dioxide to form ammonium carbonate.
$2 \mathrm{NH}_3+\mathrm{CO}_2+\mathrm{H}_2 \mathrm{O} \rightarrow\left(\mathrm{NH}_4\right)_2 \mathrm{CO}_3$
Excess of carbon dioxide is formed to convert ammonium carbonate into ammonium hydrogencarbonate .$\begin{aligned} & \left(\mathrm{NH}_4\right)_2 \mathrm{CO}_3+\mathrm{CaCl}_2 \rightarrow \mathrm{CaCO}_3 \downarrow+2 \mathrm{NH}_4 \mathrm{Cl} \\ & \mathrm{NH}_3+\mathrm{CO}_2+\mathrm{H}_2 \mathrm{O} \rightarrow \mathrm{NH}_4 \mathrm{HCO}_3\end{aligned}$
Now the ammonium bicarbonate is reacted with sodium chloride. Sodium from sodium chloride replaces ammonia from ammonium bicarbonate and sodium bicarbonate is formed.
$\mathrm{NH}_4 \mathrm{HCO}_3+\mathrm{NaCl} \rightarrow \mathrm{NaHCO}_3+\mathrm{NH}_4 \mathrm{Cl}$
Sodium hydrogencarbonate is obtained from here. It is then further heated to give sodium carbonate i.e. washing soda.$2 \mathrm{NaHCO}_3 \rightarrow \mathrm{Na}_2 \mathrm{CO}_3+\mathrm{H}_2 \mathrm{O}+\mathrm{CO}_2$
Hence, the answer is option (1).
Question 3: Which one is known as a fusion mixture?
1)$\mathrm{Na}_2 \mathrm{CO}_3+\mathrm{NaHCO}_3$
2)$\mathrm{Na}_2 \mathrm{CO}_3+\mathrm{NaOH}$
3)$\mathrm{K}_2 \mathrm{CO}_3+\mathrm{K}_2 \mathrm{SO}_4$
4) (correct) $\mathrm{Na}_2 \mathrm{CO}_3+\mathrm{K}_2 \mathrm{CO}_3$
Solution:
Fusion mixture is the mixture of potassium carbonate and sodium carbonate.
The mixture is fused with the organic compounds, and various tests for the group analysis are done using this mixture. It is very much effective for the qualitative analysis for the organic compounds for different groups.
Since Na and K belong to the first group, i.e., the alkali metals, which are the most reactive elements in the periodic table. They have the potential to break the covalent bonds formed between the carbon atom and other atoms like nitrogen, oxygen, sulphur, halides, etc., and after breaking these covalent bonds, ionic bonds are introduced between the respective atoms and the Na or K in the fusion mixture.
Like with the halides, they form the halides and with sulphur, they form the sulphides, etc.
So, a mixture of sodium carbonate and potassium carbonate is called the fusion mixture.
Hence, the answer is option (4).
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Frequently Asked Questions (FAQs)
Baking soda is sometimes added to municipal water supplies to:
Raise pH: It helps neutralize acidic water, making it more alkaline and safe for consumption.
Improve taste: By reducing water acidity, it can enhance the flavor of the water.
Prevent corrosion: It helps reduce corrosion in pipes by maintaining a balanced pH level.
Baking soda (sodium bicarbonate) is used in electroplating for the following reasons:
Buffering Agent: It helps maintain a stable pH in the electrolyte solution, ensuring consistent plating quality.
Improves Conductivity: It enhances the electrical conductivity of the solution, promoting efficient metal deposition.
Prevents Oxidation: It can help reduce oxidation of the metal being plated, ensuring smoother and more even coatings.
Baking soda interacts with fats and oils in the following ways:
Mild Abrasive: It helps break down grease and remove oily stains due to its abrasive properties.
Emulsification: In some cases, it can act as a mild emulsifier, helping to break down and mix oils with water.
Neutralization: It can neutralize acidic compounds present in fats and oils, improving cleaning and deodorizing.
Baking soda (sodium bicarbonate) is used in firefighting for the following reasons:
Releases Carbon Dioxide (CO₂): When heated, baking soda decomposes to release CO₂, which helps suffocate the fire by displacing oxygen around the flames.
Works on Small Grease Fires: It’s effective for grease fires (common in kitchens) because CO₂ prevents oxygen from feeding the fire.
Non-Toxic and Safe: It’s non-toxic and safe for use in home firefighting situations, especially for small fires
In non-aqueous solvents, baking soda (sodium bicarbonate) behaves differently compared to water:
Reduced Dissociation: It does not dissociate as easily, since the solvent may not effectively stabilize the ions (Na⁺ and HCO₃⁻).
Lower Reactivity: The acid-base reactivity is reduced because the solvent can't efficiently support the ionization of NaHCO₃.
Solubility: It has lower solubility in non-aqueous solvents compared to water.
Baking soda (sodium bicarbonate) compares to other common lab bases as follows:
Strength: It is a weak base, much milder than stronger bases like sodium hydroxide (NaOH) or potassium hydroxide (KOH).
Reactivity: Reacts more slowly and less aggressively than strong bases, making it safer to handle for mild reactions.
Uses: Commonly used for neutralizing acids, buffer solutions, and mild cleaning, unlike strong bases which are used in more reactive processes.
The crystal structure of baking soda affects its:
Solubility: Easily dissolves in water due to its ionic lattice.
Thermal stability: Breaks down at high temperatures to form sodium carbonate, CO₂, and water.
Abrasiveness: Mildly abrasive, useful in cleaning.
Granularity: Crystal size affects its use in baking and mixing.
Baking soda is used in swimming pool maintenance to:
Raise pH and stabilize alkalinity.
Clean pool tiles and remove stains.
Soften hard water, reducing mineral buildup.
It helps maintain balanced water chemistry and improve overall pool quality.
Baking soda is used in agriculture for:
Fungicide: Prevents fungal growth, especially powdery mildew.
Soil pH Adjustment: Slightly raises the pH of acidic soils.
Pest Control: Repels pests like ants and cockroaches.
Promotes Growth: Improves seed germination and plant strength.
It’s a safe, natural alternative for controlling pests and improving plant health
Yes, baking soda can be used to generate carbon dioxide in a lab. This is typically done by reacting baking soda with an acid, such as vinegar or hydrochloric acid. The reaction produces carbon dioxide gas, which can be collected and used for various experiments. This method is safe, inexpensive, and commonly used in educational settings to demonstrate gas production and acid-base reactions.
