Why Does Salt Dissolve in Water but Not in Acetone?
The Simple Experiment That Opens Up a Big Part of Chemistry
Sometimes the most important ideas in chemistry do not begin with an expensive piece of equipment, a complicated calculation, or a page full of equations.
Sometimes they begin with a small spoonful of salt, two test tubes, a little water, and a little acetone.
Put salt into water and it dissolves.
Put salt into acetone and, rather disappointingly, it sits there.
That is it.
A very simple experiment.
And yet inside that simple observation is a huge amount of GCSE and A-Level chemistry: ionic bonding, intermolecular forces, polarity, solubility, energy changes, hydration, lattice enthalpy, and the difference between memorising chemistry and actually understanding it.
I often find that students have heard the phrase “like dissolves like”. They may even be able to repeat it in an exam. But when asked why salt dissolves in water and not in acetone, the understanding is often much less secure.
That is usually because they have never actually done the experiment.
They have never watched it happen.
They have never had that small moment of surprise where one liquid behaves completely differently from another.
And in chemistry, those small moments matter.
Chemistry Is Built on Fundamentals
One of the dangers in modern science education is that students can move very quickly through a syllabus without having time to properly understand the foundations.
They learn that sodium chloride is ionic.
They learn that water is polar.
They learn that some substances dissolve and others do not.
They learn definitions, diagrams, equations and exam phrases.
But chemistry is not just a collection of facts. It is a way of explaining why matter behaves as it does.
The fundamentals matter because they keep coming back.
If a student does not really understand why salt dissolves in water, then later topics become much harder. They may struggle with electrolysis, rates of reaction in solution, titrations, acids and alkalis, precipitation reactions, entropy, enthalpy changes, and even organic chemistry.
A weak foundation makes the whole building wobble.
A strong foundation allows everything else to make sense.
The Practical: Salt, Water and Acetone
The demonstration is beautifully simple.
You take two test tubes.
Into one, you place a small amount of water.
Into the other, you place a small amount of acetone.
Then you add a small quantity of sodium chloride to each and gently shake or stir.
In the water, the salt gradually disappears from view. It has dissolved.
In the acetone, the salt remains mostly as solid crystals.
To a student, the first reaction is often:
“But acetone dissolves things, doesn’t it?”
And that is a very good question.
Acetone is well known as a solvent. It is used in nail varnish remover. It can dissolve many organic substances. It has a strong smell and feels like a “powerful” chemical.
So why does it not dissolve ordinary table salt?
That question is the beginning of the chemistry.
Safety note: acetone is highly flammable and should only be used in very small quantities in a properly supervised laboratory setting, away from naked flames, with suitable eye protection and ventilation.
What Is Actually Happening When Salt Dissolves?
Salt, or sodium chloride, is made from sodium ions and chloride ions.
These ions are not floating about freely in the solid. They are arranged in a giant ionic lattice. Positive sodium ions and negative chloride ions are held together by strong electrostatic forces of attraction.
For salt to dissolve, that lattice has to be broken apart.
The sodium ions and chloride ions need to be separated from one another.
That takes energy.
But if the solvent particles can surround and stabilise those ions, then dissolving becomes possible.
This is where water is very special.
Why Water Works So Well
Water molecules are polar.
That means each water molecule has a slightly negative end and a slightly positive end. The oxygen end is slightly negative, while the hydrogen ends are slightly positive.
When sodium chloride is placed in water, the water molecules surround the ions.
The slightly negative oxygen end of water is attracted to the positive sodium ions.
The slightly positive hydrogen ends of water are attracted to the negative chloride ions.
The water molecules form shells around the ions and help pull them away from the crystal lattice. Once separated, the ions can move freely in solution.
This is why salt water can conduct electricity.
The ions are no longer locked in place. They are mobile.
This one tiny practical therefore links directly to electrolysis, conductivity, bonding, solutions and particle theory.
That is a lot of chemistry from one spoonful of salt.
Why Acetone Does Not Do the Same Job
Acetone is a useful solvent, but it does not stabilise sodium and chloride ions nearly as effectively as water does.
Although acetone is polar, it is not polar in the same way as water, and it does not form the same strong network of interactions with ions. It is much less effective at pulling the sodium and chloride ions apart and keeping them separated.
So the ionic lattice remains mostly intact.
The salt stays as a solid.
This is a useful lesson for students because it shows that “a solvent” does not mean “a liquid that dissolves everything”.
Different solvents dissolve different substances because particles interact in different ways.
That is a much more powerful idea than simply learning a solubility rule.
The GCSE Chemistry Behind the Experiment
At GCSE level, this practical helps students understand several key ideas.
It shows that dissolving is not the same as melting. The salt does not become liquid sodium chloride. It separates into particles that spread through the water.
It shows that ionic compounds can dissolve in water because the ions can become separated and surrounded by water molecules.
It links to conductivity because solid salt does not conduct electricity, but salt solution does.
It helps explain why some substances are soluble and others are not.
It also challenges the common misconception that if a liquid looks clear and chemical-like, it must be able to dissolve anything.
For GCSE students, seeing this experiment makes the particle model much more real.
They are no longer just drawing circles in boxes. They are seeing the behaviour of particles through an actual chemical observation.
The A-Level Chemistry Behind the Same Experiment
At A-Level, the same simple practical becomes even richer.
Now we can discuss lattice enthalpy and hydration enthalpy.
To dissolve sodium chloride, energy is needed to overcome the attractions in the ionic lattice. But energy is released when water molecules surround the ions and form ion-dipole interactions.
Whether a substance dissolves depends on the balance between these energy changes, as well as the change in disorder or entropy.
Students can also consider solvent polarity, dielectric constant, hydrogen bonding, polar protic and polar aprotic solvents, and the ability of a solvent to stabilise separated ions.
This is why I like this experiment so much.
It is simple enough for GCSE, but deep enough for A-Level.
The same observation grows with the student.
That is what good practical chemistry should do.
“Like Dissolves Like” Is Useful, but Not Enough
Students are often taught the phrase:
“Like dissolves like.”
There is truth in it.
Polar substances tend to dissolve in polar solvents. Non-polar substances tend to dissolve in non-polar solvents.
But the phrase can become too vague if it is not explained properly.
Salt is ionic. Water is highly polar and very good at stabilising ions. Acetone may be polar, but it is not nearly as good at separating and stabilising sodium and chloride ions.
So the real question is not simply:
“Is the solvent polar?”
The better question is:
“Can the solvent particles interact strongly enough with the solute particles to overcome the forces holding the solute together?”
That is a much better chemical question.
It moves the student from memorising a slogan to thinking like a chemist.
Why Students Need to See These Experiments
One of the reasons I believe so strongly in practical science is that students remember what they have seen and done.
A student may forget a textbook paragraph about solubility.
They are much less likely to forget putting salt into two different liquids and discovering that one dissolves it and the other does not.
That moment creates a hook.
Once the hook is there, the theory has somewhere to attach.
This is why having access to a proper laboratory makes such a difference in tuition. We can take the key ideas from the specification and turn them into something visible.
Instead of just saying “water is polar”, we can show why polarity matters.
Instead of just saying “ionic substances dissolve in water”, we can compare water with another solvent and ask why the result is different.
Instead of just teaching exam answers, we can build understanding.
And once students understand, exam answers become much easier.
A Practical Example in a Lesson
A useful lesson might begin with the question:
“Which liquid will dissolve salt better: water or acetone?”
Most students will correctly guess water. But then I might ask:
“Why?”
That is where the real learning begins.
Some students will say:
“Because water is wet.”
Some will say:
“Because acetone is stronger.”
Some will say:
“Because salt just dissolves in water.”
These are all starting points.
Then we can look at the structure of sodium chloride, draw the ionic lattice, examine a water molecule, and show how the partial charges attract the ions.
We can then compare this with acetone and discuss why not all solvents work in the same way.
From there, we can extend the idea.
Why does sugar dissolve in water?
Why does oil not dissolve in water?
Why do some organic substances dissolve in acetone?
Why do ionic compounds often conduct electricity when molten or dissolved?
One tiny experiment has now opened the door to a large part of chemistry.
Getting the Fundamentals Right
In my experience, many students do not struggle with chemistry because they are not intelligent enough.
They struggle because the basic ideas have not quite clicked.
They have learned words without pictures.
They have memorised rules without seeing examples.
They have practised exam questions without fully understanding the particles and forces behind them.
Chemistry is a subject where the invisible world matters. Atoms, ions, molecules, electrons and intermolecular forces cannot usually be seen directly. That makes practical work even more important, not less.
A simple observation can make an invisible idea visible.
Salt dissolving in water is not just salt disappearing.
It is ions being pulled apart, surrounded and stabilised.
Salt not dissolving in acetone is not a failed experiment.
It is evidence.
It tells us something about the forces between particles.
That is chemistry.


