Why Do We Salt Roads in the Winter?

Henry Belcaster
Henry Belcaster
3 min read

Morning Salt Bae!

Not what I was expecting…

But great point, Durd!

Why do we salt roads in the winter?

Cause look at Durd:

Well, he’s in New York not California..

And it’s January.


At the risk of stating the obvious, when it’s below 32°F or 0°C outside, water freezes!

The roads are ice.

So in order to keep Durd from crashing, we gotta melt it!

But, how??

Okay…let’s try flame throwers for street lamps:

Hm. Nope.

What about ice-eating penguins?

Creates the same slippery problem…

And wtf, penguins don’t eat ice.

Okay let’s do…

~Table salt~

Ya! Sodium Chloride.

See, when salt is added to ice,

it starts to dissolve in water and break apart.

So you’re left sodium (Na+ ions) separated from chloride (Cl- ions).

Now, the positive sodium ions attract the oxygen atoms away from H2O water.

And the negative chloride ions attract water’s hydrogens:

Because of this, it’s harder to get the hydrogens and oxygens back together tightly enough to form solid H2O…ice!

The freezing point of the ice is lowered by salt.

So the streets stay…liquid!

Stay Warm,
Henry & Dylan 🌈

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