10 Everyday Examples of Soluble and Insoluble Substances

You’ve likely stirred sugar into your tea or watched oil float on water. These everyday observations are governed by a fundamental concept in chemistry known as solubility. By understanding solubility, you will gain insight into why certain substances dissolve in liquids while others don’t.

In this article, we will go through the basics of solubility and introduce you to 10 common substances, detailing whether they’re soluble or insoluble in water.

What is Solubility?

Solubility is a term that describes the maximum amount of a substance (solute) that can dissolve in a liquid (solvent) to form a homogeneous solution. For instance, when you add too much sugar to your tea, and it starts to accumulate at the bottom, you’ve reached the sugar’s solubility limit in that tea at that particular temperature.

At its core, solubility is about how much of a substance (the solute) can dissolve in a liquid (the solvent) until no more can be absorbed, resulting in a uniform solution. Think of it as the threshold at which a solute can no longer be incorporated into a solvent.

The Relationship Between Solute and Solvent

You’ve likely experienced this relationship firsthand. When making a cup of coffee, for instance, there’s only so much sugar you can add before it starts settling at the bottom. In this scenario, sugar is your solute, and coffee is your solvent. The sugar that remains undissolved has exceeded its solubility limit in the coffee at that specific temperature.

But why do some substances dissolve while others don’t? It boils down to the molecular interactions between the solute and the solvent.

In the context of chemistry, there’s a saying: “like dissolves like.” This means that polar solutes (those with charged molecules) tend to dissolve in polar solvents like water, while non-polar solutes (those without charged molecules) are more compatible with non-polar solvents like oil. This is why oil and water don’t mix, their molecular structures are inherently different.

Factors Affecting the Solubility of a Substance

Solubility isn’t just a random occurrence; it’s governed by specific factors that determine whether a substance will dissolve or remain separate.

As you explore the field of solubility, it’s essential to recognize the primary influencers: temperature, pressure, and molecular interactions. Let’s dive into each one and see how they shape the solubility of the substances you encounter daily.

Temperature: The Heat’s Impact on Solubility

You might have noticed that sugar dissolves faster in hot tea than in iced tea. This isn’t a mere coincidence; temperature plays a crucial role in solubility.

For many solids, as the temperature increases, so does their solubility in water. This is because higher temperatures provide more kinetic energy to the molecules, allowing them to break down and integrate into the solvent more efficiently.

However, it’s worth noting that this isn’t a universal rule. For some gases, their solubility decreases as temperature rises. That’s why a cold can of soda is fizzier than a warm one: colder temperatures can hold more dissolved carbon dioxide.

Pressure: The Push and Pull on Solubility

While pressure plays a less pronounced role for solids and liquids, it’s a significant factor for gases. Increasing the pressure on a gas over a liquid can increase its solubility. This principle is evident when you open a carbonated drink. The hissing sound you hear is the release of carbon dioxide gas, which is dissolved under high pressure. When the pressure is reduced upon opening, the gas escapes.

Molecular Interactions: The Invisible Bonds

At the microscopic level, everything is about interactions. The nature of the solute and solvent molecules determines their compatibility. As mentioned earlier, “like dissolves like.” Polar solutes, with their charged ends, tend to dissolve in polar solvents like water.

Conversely, non-polar solutes, which lack these charges, prefer non-polar solvents like oil. This molecular matchmaking is why oil doesn’t mix with water but dissolves seamlessly in vinegar, forming a vinaigrette.

The “Like Dissolves Like” Phenomenon: A Deep Dive into Solubility

Now, let us take some time to learn more about the “Like Dissolves Like” phenomenon and understand its significance in the context of 10 soluble and insoluble substances.

Distinguishing Between Polar and Non-Polar Substances

In the world of molecules, not all are created equal. Some molecules have regions with slight positive and negative charges, making them polar. Others lack these charges and are non-polar.

For instance, consider water. Its molecule has a bent shape, with the oxygen atom having a slight negative charge and the hydrogen atoms having slight positive charges. This makes water a polar molecule. On the other hand, oil is made up of long chains of carbon and hydrogen atoms without any significant charge differences, classifying it as non-polar.

When you try to mix oil and water, they separate. Why? Because the polar water molecules are more attracted to each other than to the non-polar oil molecules, and vice versa.

The Role of Molecular Bonds in Determining Solubility

The solubility of a substance is greatly influenced by the type of molecular bonds it possesses and the bonds of the solvent in which it’s being dissolved. When a substance dissolves, its molecules or ions are surrounded by solvent molecules, a process called solvation.

For a substance to dissolve, the attractions between its molecules or ions need to be overcome. If the solvent can offer stronger or comparable attractions, the substance will dissolve.

This is where the “Like Dissolves Like” principle comes into play. Polar solvents, like water, can dissolve ionic compounds (like salt) and other polar substances due to the strong attraction between the charged particles. Non-polar solvents, like oil, are better at dissolving non-polar substances.

For example, when you add salt (an ionic compound) to water, the positive and negative ions in salt are attracted to the water’s polar molecules, leading to dissolution. But if you try to dissolve salt in oil, it won’t work because the ionic bonds in salt are stronger than any potential attractions with the non-polar oil molecules.

In the upcoming section, we’ll finally learn about ten everyday substances and discover whether they readily dissolve in water or prefer to remain undissolved.

10 Everyday Examples of Soluble Substances

Now, let’s take a look at some common soluble substances and the science behind their solubility.


As we’ve discussed before, you’ve probably noticed countless times how sugar disappears when stirred into a hot drink. This is because sugar, or sucrose, is a polar molecule.

Water, being a polar solvent, interacts with the polar regions of the sugar molecules, causing them to break apart and dissolve. This process is driven by the formation of hydrogen bonds between water and sugar molecules. So, the next time you sweeten your tea, remember that there’s a bit of chemistry happening right in your cup.


Salt, or sodium chloride, is another substance that readily dissolves in water. When you add salt to water, the positive sodium ions and negative chloride ions are attracted to the polar water molecules. This interaction pulls the ions away from the salt crystal, allowing them to disperse throughout the water. This is why salt is so effective in flavoring foods; its ions spread out and interact with taste receptors on your tongue.



Honey might be thick and sticky, but it’s also water-soluble. The primary components of honey are sugars like fructose and glucose, which, as we’ve seen with table sugar, are polar and dissolve in water.

The water content in honey also plays a role in its solubility. When you mix honey with water, the sugars in honey interact with the water molecules, leading to a smooth mixture. This property is why honey can be easily mixed into beverages or used in recipes that require a liquid sweetener.


Glucose is a simple sugar that provides energy for our cells. Like other sugars, glucose is polar and dissolves well in water. When glucose enters our bloodstream, it’s carried by the water-based blood to cells throughout our body. The solubility of glucose in water is crucial for our metabolism, as it ensures that energy is readily available for our cells.

Copper Sulphate Crystals

copper sulphate crystals
copper sulphate crystals

Copper sulfate, with its vibrant blue crystals, is often used in school experiments to demonstrate solubility. When copper sulfate is added to water, it dissociates into copper ions and sulfate ions. These ions are then surrounded by water molecules, leading to a clear blue solution. Beyond the classroom, copper sulfate is used in agriculture and industry, and its solubility in water is key to many of its applications.

Baking Soda

Baking soda, or sodium bicarbonate, is a staple in many kitchens. When dissolved in water, it releases sodium ions and bicarbonate ions. This solubility plays a crucial role in baking, as the bicarbonate ions react with acids to produce carbon dioxide gas, making baked goods rise. The solubility of baking soda increases with temperature, which is why it dissolves better in hot water than in cold.


Coffee is a complex mixture of compounds, many of which are soluble in water. The primary soluble components are the flavor and aroma compounds, along with caffeine. The solubility of these compounds is influenced by factors like roast level, grind size, and brewing temperature. Darker roasts, for example, tend to be more soluble than lighter roasts. This solubility is what gives coffee its rich flavor and aroma when brewed.

Potassium Nitrate

potassium nitrate
potassium nitrate

Potassium nitrate, often used as a fertilizer in gardens or labs for various experiments, is highly soluble in water. Its solubility increases significantly with temperature, which is why it’s sometimes used in solubility demonstrations in classrooms. When dissolved, it dissociates into potassium and nitrate ions, making it useful in various applications, from agriculture to food preservation.

Lemon Juice

Lemon juice is rich in citric acid, a compound that’s readily soluble in water. This solubility is responsible for the sharp, tangy taste you experience when sipping a lemonade. The acidic nature of lemon juice, due to its citric acid content, also makes it a popular natural cleaning agent, as it can dissolve mineral deposits and stains.


Alcohol, specifically ethanol, is miscible with water, meaning the two can be mixed in any proportion without separating. This solubility arises from ethanol’s molecular structure, which has a polar hydroxyl group and a non-polar hydrocarbon chain. This dual nature allows it to dissolve in both polar solvents like water and non-polar solvents. It’s this characteristic that makes alcoholic beverages varied and versatile, from potent spirits to milder drinks.

10 Everyday Examples of Insoluble Substances

While many substances dissolve seamlessly in water, others resist this union. These insoluble substances have unique characteristics that prevent them from blending with water. Let’s explore some common examples and understand the science behind their inability to dissolve.

Mustard Oil

Mustard oil is renowned for its pungent aroma and is a favorite in various culinary traditions. But pour some into water, and you’ll notice it forms a separate layer.

Mustard oil is primarily composed of fats and lacks the polar groups that water molecules have. This difference in molecular structure means that the oil molecules are more attracted to each other than to water molecules, leading them to stay separate.


saw dust
saw dust

If you’ve ever done woodworking or simply observed a carpenter at work, you’re familiar with sawdust. Sprinkle some on water, and you’ll see it float.

Sawdust is composed of tiny wood particles. Wood is primarily made of cellulose, a complex carbohydrate that doesn’t dissolve in water. Additionally, the air trapped in the sawdust makes it buoyant, causing it to float.


Sand, whether from serene beaches or vast deserts, is omnipresent. Yet, no matter how much you stir, it won’t dissolve in your beach bucket filled with water.

The reason why sand is an insoluble substance is because it is primarily composed of silicon dioxide. The strong covalent bonds between the silicon and oxygen atoms in sand are much stronger than any potential bonds with water molecules, making it insoluble.

Chalk Powder

Chalk, often associated with school blackboards, leaves behind a powdery residue. If you’ve ever tried to mix this powder with water, you’ve seen it doesn’t dissolve.

That’s because chalk is made of calcium carbonate. While it can react with acids, it doesn’t dissolve in pure water due to its stable crystalline structure.

Petals of Flowers

Flower petals, with their vibrant colors and delicate textures, are a treat for the eyes. But submerge them in water, and they retain their integrity.

The cellular structure of flower petals is designed to be sturdy and protect the reproductive parts of the flower. This structure, combined with the waxy surface of many petals, prevents them from dissolving in water.


You’ve likely observed how water droplets bead up on a freshly waxed car or candle surface. The reason is because wax is a hydrophobic (water-repelling) substance. It is primarily composed of long-chain hydrocarbons. These chains lack the polar groups that water molecules possess, leading to minimal interaction between the two. As a result, water tends to bead up on waxy surfaces rather than spread out or dissolve the wax.

Plastic Beads

Plastic beads, often found in craft projects or certain cosmetics, are notorious for their persistence in the environment.

Plastics, including the ones used to make these beads, are primarily composed of polymers – large molecules made up of repeating subunits. These polymers are non-polar and lack the ability to form bonds with water molecules, making them insoluble in water.

Peanut Oil

Peanut oil is a favorite in many kitchens, especially for frying. Pour it into water, and it forms a distinct layer.

Like other oils, peanut oil is made up of triglycerides, which are non-polar molecules. Due to the absence of polar groups, peanut oil molecules are more attracted to each other than to water molecules, leading them to remain separate when mixed with water.


Rubber, whether in the form of a child’s toy or a car tire, doesn’t dissolve in water, regardless of how long it’s submerged. The reason behind its insolubility with water is that rubber is a polymer made from repeating units of isoprene. Its molecular structure is non-polar and lacks sites that can bond with water molecules, making it insoluble in water.


Charcoal, often used in grilling or water purification, has an impressive ability to absorb impurities without dissolving in water.

Charcoal is primarily carbon with a porous structure. While it can adsorb (bind to its surface) many substances, it doesn’t dissolve in water due to its non-polar nature.

Final Thoughts

Throughout this article, we’ve encountered a diverse array of substances, each with its unique relationship with water. From readily soluble substances like salt and sugar to steadfast insoluble substances like wax and rubber, each material offers a lesson in the principles of chemistry.

Thank you for reading our article, and as you go about your day, take a moment to observe the interactions around you. When you brew your morning coffee or cook dinner, solubility is at play. When you water your plants or wash your car, the principles of solubility are silently shaping those experiences.

Challenge yourself to identify soluble and insoluble substances in your surroundings. Why does your tea dissolve sugar but not oil? Why does rain bead up on certain surfaces but not others? By asking these questions and seeking answers, you’ll cultivate a deeper appreciation for the science that governs the everyday.

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