Ask the Chatbot Games & Quizzes ProCon History & Society Science & Tech Biographies Animals & Nature Geography & Travel Arts & Culture Money Videos
Science & Tech
verifiedCite
While every effort has been made to follow citation style rules, there may be some discrepancies. Please refer to the appropriate style manual or other sources if you have any questions.
Select Citation Style

Why Does Salt Melt Ice?

verifiedCite
While every effort has been made to follow citation style rules, there may be some discrepancies. Please refer to the appropriate style manual or other sources if you have any questions.
Select Citation Style
Written by
Cydney Grannan
Cydney Grannan was an Editorial Intern at Encyclopædia Britannica. She received her B.A. in English from the University of Chicago in 2016.
Cydney Grannan
Fact-checked by
The Editors of Encyclopaedia Britannica
Encyclopaedia Britannica's editors oversee subject areas in which they have extensive knowledge, whether from years of experience gained by working on that content or via study for an advanced degree. They write new content and verify and edit content received from contributors.
The Editors of Encyclopaedia Britannica
winter ice melting salt on the ground, pattern as background
© nd700/Fotolia

More than 20 million tons of salt are used every year to melt snow and ice in cold northern regions. But how does salt do it?

First, it’s important to understand a bit about H2O in the winter. Thirty-two degrees Fahrenheit (0 degrees Celsius) is its freezing point—that is, when water reaches 32 °F, it turns into ice. At this temperature, your icy road generally has a thin layer of water on top of the ice, and the ice molecules and water molecules are interacting. This water is constantly melting some of the ice, while the ice beneath it is freezing some of the water. At this temperature, the exchange rate is pretty constant, meaning the amount of water and the amount of ice stay the same. If it gets colder, more water becomes ice. If it gets warmer, more ice becomes water. When the ionic compound salt is added to the equation, it lowers the freezing point of the water, which means the ice on the ground can’t freeze that layer of water at 32 °F anymore. The water, however, can still melt the ice at that temperature, which results in less ice on the roads.

But you may be asking how salt lowers the freezing point of water. This concept is called “freezing point depression.” Essentially, the salt makes it harder for the water molecules to bond together in their rigid structure. In water, salt is a solute, and it will break into its elements. So, if you’re using table salt, also known as sodium chloride (NaCl), to melt ice, the salt will dissolve into separate sodium ions and chloride ions. Often, however, cities use calcium chloride (CaCl2), another type of salt, on their icy streets. Calcium chloride is more effective at melting ice because it can break down into three ions instead of two: one calcium ion and two chloride ions. More ions mean more ions getting in the way of those rigid ice bonds.

Unfortunately, chloride is superbad for the environment. It can kill aquatic animals, and that can thereby affect other animal populations in their food web. Chloride also dehydrates and kills plants and can alter soil composition, making it harder for vegetation to grow. While some other compounds that can melt ice and snow don’t include chloride, they are much more expensive than sodium chloride or calcium chloride.