The Complete Guide to Baking Soda

What Is Baking Soda?

Found in kitchens, bakeries and cleaning cupboards around the world, baking soda has earned a reputation as a remarkably versatile substance. It helps bread rise, neutralises odours, cleans household surfaces, softens water and has been used in traditional home remedies for generations.

Despite its many uses, baking soda is surprisingly simple.

Chemically, baking soda is sodium bicarbonate (NaHCO₃)—a naturally occurring alkaline mineral salt made from four common elements:

• Sodium (Na)
• Hydrogen (H)
• Carbon (C)
• Oxygen (O)

These elements combine to form tiny white crystals that are ground into the fine powder most of us recognise.

Because of this simplicity, it behaves in predictable ways. It dissolves easily in water, reacts with acids, helps neutralise odours and can gently lift dirt without being overly abrasive. These properties explain why the same ingredient can be used in baking, cooking, cleaning and many other everyday tasks.

What Is Baking Soda Made Of?

Every particle of baking soda contains the same simple chemical structure:

NaHCO₃

This chemical formula may appear intimidating at first, but it simply describes the arrangement of four familiar elements.

Sodium (Na)

Sodium is a naturally occurring mineral found throughout the Earth’s crust and oceans. It plays an essential role in living organisms, helping regulate fluid balance, nerve signalling and muscle contraction.

Most people recognise sodium as part of table salt (sodium chloride), but sodium also forms many other naturally occurring compounds, including sodium bicarbonate.

Hydrogen (H)

Hydrogen is the lightest and most abundant element in the universe.

It is found in:

• Water
• Plants
• Animals
• Air
• Almost every organic molecule on Earth

Within baking soda, hydrogen forms part of the bicarbonate ion.

Carbon (C)

Carbon is often called the element of life.

It forms the backbone of:

• Plants
• Animals
• Microorganisms
• Food
• Fuels

Carbon also occurs naturally in carbon dioxide gas, limestone, shells and countless minerals.

In baking soda, carbon is one reason it can release carbon dioxide gas when it reacts with acids.

Oxygen (O)

Oxygen is one of the most abundant elements on Earth.

It is present in:

• Air
• Water
• Rocks
• Living organisms

Combined with carbon and hydrogen, oxygen forms the bicarbonate portion of baking soda.

Why Is It Called “Sodium Bicarbonate”?

The scientific name simply describes what the compound contains.

Sodium refers to the positively charged sodium ion.

Bicarbonate refers to the bicarbonate ion (HCO₃⁻), a naturally occurring compound found throughout nature.

Together they form sodium bicarbonate.

What Does “Sodium” Mean?

The word sodium comes from the English word soda, while the chemical symbol Na comes from the Latin word natrium, referring to naturally occurring mineral deposits rich in sodium compounds.

Sodium itself is never found as a pure metal in nature because it reacts readily with water. Instead, it exists combined with other elements to form stable minerals and salts.

Examples include:

• Sodium chloride (table salt)
• Sodium bicarbonate (baking soda)
• Sodium carbonate (washing soda)

Sodium compounds have been used by humans for thousands of years in cooking, cleaning, food preservation and glassmaking.

What Does “Bicarbonate” Mean?

The bicarbonate ion (HCO₃⁻) is one of nature’s most important buffering compounds.

A buffer is a substance that helps resist sudden changes in acidity.

Bicarbonate naturally occurs in:

• Blood
• Saliva
• Seawater
• Groundwater
• Mineral springs

In the human body, bicarbonate helps maintain a stable pH, allowing cells, enzymes and organs to function normally.

In nature, it plays a similar balancing role in rivers, lakes and oceans.

When bicarbonate encounters an acid, it reacts by forming carbon dioxide gas and water. This simple reaction is responsible for the bubbling seen when baking soda is mixed with vinegar or lemon juice.

Why Is It Called “Baking Soda”?

Before modern chemistry existed, people discovered that certain mineral salts could help dough rise.

During the eighteenth and nineteenth centuries, sodium-rich compounds became known collectively as sodas.

When sodium bicarbonate began replacing older leavening agents in cakes, biscuits and breads, it quickly became known as baking soda—quite literally, the soda used for baking.

The name has remained ever since.

Is Baking Soda Natural or Man-Made?

The answer is both and understanding why requires a look at where baking soda comes from.

Baking Soda Exists in Nature

Long before people learned how to manufacture it, sodium bicarbonate already existed in nature.

It occurs as a naturally occurring mineral called nahcolite, which forms over millions of years under very specific geological conditions.

Most natural deposits are found in ancient lake beds where water gradually evaporated, leaving behind layers of dissolved minerals. As these lakes dried and minerals became concentrated, sodium bicarbonate crystallised within the surrounding rock.

Today, large nahcolite deposits are found in several parts of the world, particularly in the United States, where some are thick enough to be commercially mined.

Natural sodium bicarbonate can also be found in:

• Mineral springs
• Alkaline lakes
• Underground brines
• Certain groundwater systems

Although these sources contain much smaller amounts than nahcolite deposits, they show that sodium bicarbonate is a naturally occurring part of Earth’s mineral cycle.

From Nature to the Kitchen

When natural nahcolite is mined, it is:

• Extracted from underground deposits.
• Crushed into smaller pieces.
• Purified to remove naturally occurring impurities.
• Ground into the familiar fine white powder.

After purification, it becomes the same food-grade baking soda found on supermarket shelves.

Why Isn’t All Baking Soda Mined?

Natural deposits are relatively uncommon and not every country has access to economically viable sources.

To meet worldwide demand, most baking soda is produced using a manufacturing method known as the Solvay Process.

Rather than mining sodium bicarbonate directly, this process creates it from abundant natural raw materials:

• Salt (sodium chloride)
• Limestone (calcium carbonate)
• Water
• Ammonia

These materials undergo a carefully controlled series of reactions that produce sodium bicarbonate crystals.

Although the process occurs in a factory, it does not create an artificial version of baking soda. It simply recreates, through chemistry, the same sodium bicarbonate found in nature.

Is Mined Baking Soda Better?

Chemically, no.

Whether sodium bicarbonate comes from a natural nahcolite deposit or is produced using the Solvay Process, the finished compound is still NaHCO₃.

Its chemical structure, behaviour and properties are identical.

The main differences lie in how it was obtained before purification not in the baking soda itself.

Does Manufacturing Leave Chemicals Behind?

Because people hear that ammonia is used during manufacturing, they sometimes worry that it remains in the final product.

In the Solvay Process, ammonia acts as a processing aid. It is recovered and reused during production rather than becoming an ingredient in the finished baking soda.

The final product is purified before packaging and food-grade baking soda must meet strict quality standards before it reaches consumers.

So, Is Baking Soda Natural?

Yes.

Baking soda is a naturally occurring mineral that can either be:

• Mined directly from natural nahcolite deposits, or
• Manufactured from common natural raw materials using the Solvay Process.

In both cases, the result is the same compound:

Sodium bicarbonate (NaHCO₃).

Understanding this helps explain why baking soda is neither a mysterious synthetic chemical nor an exotic natural remedy, it is simply one of nature’s most useful mineral salts, prepared in different ways to meet the needs of modern life.

How Is Baking Soda Made?

Inside the Solvay Process

At first glance, it sounds like a complicated industrial process filled with unfamiliar chemicals. In reality, it begins with four simple natural raw materials:

• Salt (sodium chloride)
• Limestone (calcium carbonate)
• Water
• Ammonia

These ingredients work together in a cycle that has been used for more than 160 years because it is efficient, economical and produces high-purity sodium bicarbonate.

The key thing to remember is this:

The Solvay Process does not create a different kind of baking soda, it produces exactly the same sodium bicarbonate (NaHCO₃) found in nature.

Step 1 — Salt Is Dissolved

The process begins with ordinary salt (sodium chloride).

Salt is dissolved in purified water to produce a concentrated salt solution called brine.

Brine provides the sodium needed to make sodium bicarbonate.

Step 2 — Limestone Is Heated

Limestone is a naturally occurring rock made mostly of calcium carbonate (CaCO₃).

When heated in a kiln, limestone breaks apart into:

• Carbon dioxide (CO₂)
• Calcium oxide (quicklime)

The carbon dioxide produced here will later become part of the baking soda molecule.

Step 3 — Ammonia Is Added

Ammonia gas is added to the salt solution.

Many people become concerned when they hear this step, but ammonia is not added as an ingredient for consumers. Instead, it acts as a processing aid, helping the reaction occur efficiently.

Step 4 — Carbon Dioxide Is Introduced

Carbon dioxide from the heated limestone is bubbled through the ammoniated brine.

This causes sodium bicarbonate to form.

Unlike many other salts, sodium bicarbonate is only slightly soluble in cold water.

As it forms, it naturally crystallises out of the solution as tiny white crystals.

These crystals are collected by filtration.

Step 5 — Purification

The sodium bicarbonate crystals are:

• Washed
• Purified
• Dried
• Ground into a fine powder

This becomes the baking soda used in food, cooking and household products.

What Happens to the Ammonia?

During the Solvay Process, the ammonia is recovered and recycled back into the system to be used again.

Very little is wasted, which is one reason the Solvay Process has remained the world’s dominant manufacturing method for over a century.

A Brief History of Baking Soda

How People Baked Before Modern Baking Soda

Long before chemistry identified sodium bicarbonate or factories learned to produce it, people had already developed ingenious ways to make bread, cakes and other baked foods rise. These methods relied on fermentation, naturally occurring minerals, plant ashes and even air trapped inside beaten eggs.

The story of baking soda is therefore also the story of humanity’s search for lighter, softer bread.

Before Baking Soda

For thousands of years, the only way to make bread rise was through fermentation.

Wild yeasts living naturally in the environment settled on flour mixed with water, producing carbon dioxide as they consumed sugars. Tiny bubbles became trapped inside the dough, causing it to expand.

This process gave rise to what we now call sourdough.

Every region developed its own sourdough cultures, each containing different yeasts and bacteria that produced distinctive flavours and textures.

Even today, sourdough remains one of the oldest continuously used baking methods in the world.

Ancient Egypt

Around 4,000–5,000 years ago, the ancient Egyptians became masters of leavened bread.

It is believed that a batch of dough was accidentally left standing long enough for wild yeasts to begin fermenting it. Rather than throwing it away, the dough was baked and produced a lighter loaf than the flatbreads people were accustomed to.

The discovery changed baking forever.

Egyptian bakers soon learned to keep a portion of fermented dough and add it to new batches, creating an early form of sourdough starter.

The Greeks and Romans

The Greeks and Romans refined bread-making even further.

In addition to sourdough, they sometimes used:

• Grape must
• Wine foam
• Beer barm (foam from brewing)
• Fermented grain mixtures

These ingredients introduced active yeasts that encouraged dough to rise.

Bread gradually became softer, lighter and more varied across the Mediterranean world.

Potash and Pearlash

By the 1700s, bakers had discovered another useful ingredient.

When hardwood was burned, the ashes contained potassium-rich alkaline salts. These salts could be extracted with water and evaporated to produce potash (mainly potassium carbonate).

Potash reacted with acidic ingredients in dough to release carbon dioxide, helping baked goods become lighter.

Later, potash was purified further into pearlash, one of the first commercially produced chemical leavening agents.

Pearlash became especially popular in North America before modern baking soda was available.

Whipped Eggs

Not every baked food relied on fermentation or alkaline salts.

Many cakes rose simply because cooks vigorously whisked eggs.

Beating egg whites trapped countless tiny air bubbles inside a network of proteins. During baking these bubbles expanded, giving sponge cakes their light texture.

This method is still used today in foods such as:

• Sponge cakes
• Angel food cake
• Soufflés
• Meringues

The Discovery of Baking Soda

During the eighteenth and nineteenth centuries, chemists began studying alkaline minerals more closely.

As sodium bicarbonate became easier to produce, bakers quickly recognised its advantages.

Unlike sourdough or yeast, baking soda worked almost immediately when mixed with an acidic ingredient.

Recipes became:

• Faster
• More predictable
• More consistent

Home baking changed dramatically.

Instead of waiting hours for dough to ferment, cakes and biscuits could be mixed and baked within minutes.

Why Is Baking Soda Alkaline?

Understanding pH, Acids and Alkalis

One of baking soda’s most useful properties is that it is alkaline.

This single characteristic explains why it helps cakes rise, why it reacts so dramatically with vinegar, why it can neutralise many odours, and why it has become such a versatile ingredient in both cooking and household cleaning.

To understand baking soda, we first need to understand pH.

What Is pH?

The letters pH stand for “potential of hydrogen.”

The pH scale measures how acidic or alkaline a substance is.

It ranges from 0 to 14.

• 0–6.9 → Acidic
• 7 → Neutral
• 7.1–14 → Alkaline (basic)

The further a substance is from 7, the stronger its acidity or alkalinity.

Some familiar examples include:

Baking soda sits just above neutral, making it a mild alkali rather than a strongly caustic one.

What Makes Something Acidic?

Acids release hydrogen ions (H⁺) when dissolved in water.

These hydrogen ions give acids their characteristic properties.

Many familiar foods are naturally acidic, including:

• Vinegar
• Lemon juice
• Limes
• Grapefruit
• Tomatoes
• Apples
• Yoghurt
• Buttermilk

Acids often taste sour because of these naturally occurring organic acids.

Examples include:

• Acetic acid in vinegar
• Citric acid in citrus fruits
• Malic acid in apples
• Lactic acid in yoghurt
• Tartaric acid in grapes

What Makes Something Alkaline?

Alkaline substances have the opposite effect.

Instead of contributing hydrogen ions, they help neutralise them.

This is why alkalis can reduce acidity when mixed with acids.

Examples of mildly alkaline foods include:

• Egg whites
• Some mineral waters
• Baking soda

Stronger alkalis include washing soda, ammonia and sodium hydroxide, which have very different uses and require much greater care.

Baking soda is much gentler because it is only mildly alkaline.

Why Is Baking Soda Alkaline?

The answer lies in the bicarbonate ion (HCO₃⁻).

When baking soda dissolves in water, the bicarbonate ion interacts with water molecules in a way that removes some free hydrogen ions from the solution.

With fewer hydrogen ions present, the solution becomes slightly alkaline.

This gives baking soda a pH of approximately 8.3.

Unlike stronger alkalis, baking soda acts as a buffer, meaning it helps moderate changes in acidity rather than forcing the pH to extreme levels.

This buffering ability is one reason bicarbonate is found naturally throughout the human body and in many natural waters.

Why Does This Matter in Baking?

Many baking ingredients are naturally acidic.

When baking soda is mixed with these ingredients, it begins to neutralise some of their acidity.

At the same time, carbon dioxide gas is released.

Those tiny bubbles expand during baking, creating a lighter texture in cakes, muffins, pancakes and quick breads.

Without enough acid, baking soda cannot release all of its carbon dioxide.

This is why recipes carefully balance acidic and alkaline ingredients.

Better Browning

Because baking soda creates a slightly more alkaline environment, it encourages the Maillard reaction—the complex series of reactions responsible for the rich golden-brown colour and toasted flavours that develop during baking.

This is why baked goods made with baking soda often brown more readily.

Softer Texture

The carbon dioxide bubbles produced during baking create countless tiny air pockets.

These pockets give foods a lighter, softer crumb.

Without enough gas production, cakes and muffins become compact and dense.

Improved Spread in Cookies

In cookie dough, baking soda encourages spreading during baking.

As the dough softens, the carbon dioxide helps create a thinner, crisp-edged cookie with a tender centre.

Recipes that use baking powder instead often produce thicker cookies with a more cake-like texture.

Balancing Acidity

Some ingredients have a naturally tangy or sharp flavour.

Baking soda helps balance part of this acidity while still allowing the ingredient’s characteristic flavour to remain.

This balance contributes to a smoother overall taste.

Baking Soda vs Baking Powder

Although they are often confused, they are not the same.

Baking Soda

• Pure sodium bicarbonate.
• Needs an acidic ingredient.
• Creates a rapid reaction.
• Produces excellent browning.

Baking Powder

• Contains baking soda plus one or more powdered acids and starch.
• Works when mixed with liquid and, in many cases, again when heated.
• Useful in recipes without naturally acidic ingredients.

Some recipes use both.

Baking soda reacts with the natural acids already present, while baking powder provides additional lift during baking.

Household Uses of Baking Soda

Unlike soap or detergents, baking soda does not work in just one way. Instead, several of its natural properties work together.

Mild Abrasive

Each particle of baking soda is a tiny crystal.

These crystals are hard enough to help lift dirt, grease and dried-on food, yet gentle enough not to scratch many hard surfaces.

This makes baking soda useful for cleaning:

• Stainless steel sinks
• Ceramic cooktops
• Porcelain
• Tiles
• Glass bakeware
• Kitchen benches
• Grouts

Helps Neutralise Odours

Many unpleasant smells are caused by acidic or alkaline compounds.

Because baking soda is mildly alkaline, it can help neutralise some acidic odours rather than simply masking them with fragrance.

This is why it is commonly placed in:

• Refrigerators
• Shoe cupboards
• Rubbish bins
• Pet areas
• Closets

Unlike air fresheners that cover smells with perfume, baking soda helps reduce certain odours at their source.

Softens Water

Hard water contains dissolved minerals, mainly calcium and magnesium.

These minerals can reduce the effectiveness of soaps and detergents.

Adding a small amount of baking soda to some cleaning tasks may help soften water, allowing soaps to work more effectively.

Laundry Uses

Baking soda has long been used in laundry because it can help improve washing performance.

Traditional uses include:

• Helping reduce odours in clothing.
• Freshening towels.
• Assisting with the cleaning of sportswear.
• Helping soften wash water in some areas.

Many people also use baking soda to freshen washing machines by running an empty cycle with warm water and baking soda.

Cleaning Fruits and Vegetables

Many households soak fruits and vegetables in a solution of water and baking soda before rinsing.

This may help remove:

• Dirt
• Dust
• Wax residues
• Some surface residues from handling and transport

After soaking, produce should always be rinsed thoroughly under clean running water.

Softening Legumes

In many cultures, a small amount of baking soda has traditionally been added to soaking water or cooking water for:

• Chickpeas
• Dried beans
• Lentils

The alkaline water helps soften the outer skins, often reducing cooking time.

Tenderising Foods

Some traditional recipes include a small amount of baking soda when preparing meat or certain vegetables.

Its mild alkalinity can help change the texture of proteins, making them feel more tender.

This technique is still used in some Asian cuisines, particularly in stir-fries.

homemade personal care recipes.

Tooth Powders

Before commercial toothpaste became widely available, simple tooth powders often included baking soda because of its mild abrasive texture.

It was commonly combined with ingredients such as:

• Salt
• Herbs
• Peppermint
• Clove

Bathing

Some people traditionally added baking soda to bath water, believing it helped soften the water and leave the skin feeling refreshed.

Around the Garden

Gardeners have traditionally found many household uses for baking soda.

Examples include:

• Cleaning clay pots.
• Freshening compost bins.
• Cleaning gardening tools.
• Helping remove dirt from harvested vegetables.

Traditional Household Remedies

Throughout history, baking soda has appeared in countless household remedy books and family traditions.

It has traditionally been used in preparations for:

• Occasional indigestion.
• Gargles.
• Mouth rinses.
• Skin pastes.
• Household cleaning mixtures.
• Laundry.

These practices have been passed down through generations in many parts of the world.

A Pantry Essential

Few household ingredients have earned a place in so many different areas of daily life.

From baking bread and cooking beans to cleaning kitchens, caring for laundry and preparing homemade personal care products, baking soda has remained one of the most versatile items in the pantry.