RINSING OFF SOAP WITH SOFT WATER - Why Is It Harder to Rinse Off Soap With Soft Water? - Rinsing in soft water may leave you feeling a little slippery and soapy, even after a thorough rinsing. Why? The answer lies in understanding the chemistry of soft water and soap. Hard water contains calcium and magnesium ions. Water softeners remove those ions by exchanging them for sodium or potassium ions. Two factors contribute to that slippery-when-wet feeling you get after soaping up with soft water. First, soap lathers better in soft water than in hard water, so it's easy to use too much. The more dissolved soap there is, the more water you need to rinse it away. Second, the ions in softened water lessen its ability to stick to the soap molecules, making it more difficult to rinse the cleanser off your body. The reaction between a triglyceride molecule (fat) and sodium hydroxide (lye) to make soap yields a molecule of glycerol with three ionically bonded molecules of sodium stearate (the soap part of soap). This sodium salt will give up the sodium ion to water, while the stearate ion will precipitate out of solution if it comes into contact with an ion that binds it more strongly than sodium (such as the magnesium or calcium in hard water). The magnesium stearate or calcium stearate is a waxy solid that you know as soap scum. It can form a ring in your tub, but it rinses off your body. Soap would rather stick to you than get rinsed away in soft water.

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Rinsing Off Soap With Soft Water

Why Is It Harder to Rinse Off Soap With Soft Water?

By Anne Marie Helmenstine, Ph.D.

Do you have hard water?

If you do, you may have a water softener to help protect your plumbing from scale buildup, prevent soap scum, and lessen the amount of soap and detergent needed for cleaning.

You've probably heard that cleaners work better in soft water than in hard water, but does that mean you will feel cleaner if you bathe in soft water?

Actually, no.

Rinsing in soft water may leave you feeling a little slippery and soapy, even after a thorough rinsing.

Why? The answer lies in understanding the chemistry of soft water and soap.

The Hard Facts of Hard Water

Hard water contains calcium and magnesium ions. Water softeners remove those ions by exchanging them for sodium or potassium ions.

Two factors contribute to that slippery-when-wet feeling you get after soaping up with soft water.

First, soap lathers better in soft water than in hard water, so it's easy to use too much.

The more dissolved soap there is, the more water you need to rinse it away.

Second, the ions in softened water lessen its ability to stick to the soap molecules, making it more difficult to rinse the cleanser off your body.

Chemical Reaction

The reaction between a triglyceride molecule (fat) and sodium hydroxide (lye) to make soap yields a molecule of glycerol with three ionically bonded molecules of sodium stearate (the soap part of soap). 

This sodium salt will give up the sodium ion to water, while the stearate ion will precipitate out of solution if it comes into contact with an ion that binds it more strongly than sodium (such as the magnesium or calcium in hard water).

The magnesium stearate or calcium stearate is a waxy solid that you know as soap scum.

It can form a ring in your tub, but it rinses off your body.

The sodium or potassium in soft water makes it much more unfavorable for the sodium stearate to give up its sodium ion so that it can form an insoluble compound and get rinsed away.

Instead, the stearate clings to the slightly charged surface of your skin.

Essentially, soap would rather stick to you than get rinsed away in soft water.

Addressing the Problem

There are a few ways you can address the problem:

You can use less soap, try a synthetic liquid body wash (synthetic detergent or syndet), or rinse with naturally soft water or rainwater, which probably won't contain elevated levels of sodium or potassium.

Anne Marie Helmenstine, Ph.D.

Chemistry Expert

Education

Ph.D., Biomedical Sciences, University of Tennessee at Knoxville

B.A., Physics and Mathematics, Hastings College

Introduction

Ph.D. in biomedical sciences from the University of Tennessee at Knoxville - Oak Ridge National Laboratory.

Science educator with experience teaching chemistry, biology, astronomy, and physics at the high school, college, and graduate levels.

ThoughtCo and About Education chemistry expert since 2001.

Widely-published graphic artist, responsible for printable periodic tables and other illustrations used in science.

Experience

Anne Helmenstine, Ph.D. has covered chemistry for ThoughtCo and About Education since 2001, and other sciences since 2013. She taught chemistry, biology, astronomy, and physics at the high school, college, and graduate levels. She has worked as a research scientist and also abstracting and indexing diverse scientific literature for the Department of Energy.

In addition to her work as a science writer, Dr. Helmenstine currently serves as a scientific consultant, specializing in problems requiring an interdisciplinary approach. Previously, she worked as a research scientist and college professor. 

Education

Dr. Helmenstine holds a Ph.D. in biomedical sciences from the University of Tennessee at Knoxville and a B.A. in physics and mathematics with a minor in chemistry from Hastings College. In her doctoral work, Dr. Helmenstine developed ultra-sensitive chemical detection and medical diagnostic tests.

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