{"id":66146,"date":"2026-08-04T04:57:02","date_gmt":"2026-08-03T19:57:02","guid":{"rendered":"https:\/\/phys-edu.net\/wp\/?p=66146"},"modified":"2026-08-04T04:57:02","modified_gmt":"2026-08-03T19:57:02","slug":"the-laminated-sheet-that-reveals-acids-and-bases-an-easy-low-chemical-ultra-microplate-experiment","status":"publish","type":"post","link":"https:\/\/phys-edu.net\/wp\/?p=66146&lang=en","title":{"rendered":"The Laminated Sheet That Reveals Acids and Bases! An Easy, Low-Chemical “Ultra-Microplate” Experiment"},"content":{"rendered":"

I’m Ken Kuwako, the Science Trainer. Every day is an experiment!<\/strong><\/span><\/p>\n

Drop a little hydrochloric acid onto magnesium, and suddenly it starts to “swim”! Even better, this simple experiment lets you explore the fascinating properties of acids and alkalis all at once.<\/p>\n

Today I’d like to share an observation experiment I used with my ninth-grade science students to investigate the properties of acids and alkalis. The setup couldn’t be simpler\u2014just place a single drop of each solution from small squeeze bottles onto a laminated sheet. Using BTB solution, phenolphthalein, litmus paper, and strips of magnesium ribbon, the classroom quickly filled with excited questions of “Why did that happen?”<\/p>\n

Only Tiny Amounts of Chemicals, Yet Big Results\u2014A Brilliant Laminated Experiment Sheet<\/h3>\n

Each group receives a laminated experiment sheet, and students simply add drops of solution from small bottles. It’s easy to prepare, produces very little chemical waste, and cleanup takes only a few minutes. It’s an experiment that checks every box.<\/p>\n

You could even think of it as an ultra-microplate experiment<\/b>\u2014an even smaller version of a traditional microplate activity.<\/p>\n

Here’s what the experiment sheet looks like (feel free to download and use it).<\/p>\n

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Acid and Alkali Experiment Sheet (Laminating PDF)<\/a>\u3000\u3000Word Download<\/a><\/p>\n

Simply print the sheet and laminate it, and you’re ready to go.<\/p>\n

The original idea came from a handmade version created by one of our science assistants several years ago. I’ve since refined the design, and this is the version we currently use.<\/p>\n

First, arrange the indicators like this.<\/p>\n

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Why Does the Magnesium Ribbon “Swim”?<\/h3>\n

Next, add hydrochloric acid, sulfuric acid, and the other solutions in vertical rows.<\/p>\n

Students are always amazed by the color changes and chemical reactions. But the biggest surprise comes when the magnesium ribbon starts moving through the liquid as if it were alive.<\/p>\n

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This movement is actually caused by the chemical reaction itself.<\/p>\n

When magnesium reacts with hydrochloric acid, hydrogen gas is produced. Tiny bubbles rapidly form all over the surface of the ribbon. As these bubbles grow and detach, they repeatedly lift and release the ribbon, making it bob, float, and sink. The result is a surprisingly lifelike “swimming” motion.<\/p>\n

Behind every visible movement is an invisible stream of gas being produced.<\/b><\/p>\n

It’s a wonderful example of how chemistry can make the invisible visible.<\/p>\n

At this point in the experiment, we’ve tested everything up to the saltwater sample. Here’s one important tip:<\/p>\n

Always add the ammonia solution last.<\/strong><\/p>\n

Something very interesting is about to happen.<\/p>\n

Why Did a Solution Change Color Without Being Touched?<\/h3>\n

Here’s what the completed experiment looks like.<\/p>\n

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The most surprising part of the experiment came when we added the ammonia solution.<\/p>\n

After placing a drop of ammonia, the nearby saltwater sample\u2014which we hadn’t touched at all\u2014also changed color!<\/p>\n

The students couldn’t believe their eyes.<\/p>\n

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So what happened?<\/p>\n

Ammonia is highly volatile, meaning it easily escapes into the air as a gas\u2014even at room temperature. The ammonia molecules drifted through the air and dissolved into the neighboring drop of saltwater, making it alkaline enough to change the indicator’s color.<\/p>\n

In other words, the liquids never touched each other, but the gas connected them.<\/p>\n

This is exactly the same reason perfume spreads throughout a room or why the smell of freshly baked bread travels through the air. On this tiny experiment sheet, students were actually witnessing the physical process of gas diffusion<\/b> in real time.<\/p>\n

Moments like this are what make science so exciting. Unexpected results spark curiosity, and curiosity leads to discovery.<\/p>\n

Why not try this acid-and-alkali experiment yourself? You might uncover a scientific surprise of your own!<\/p>\n

Preparing the Reagents<\/h3>\n

\u2022 3% Hydrochloric Acid \u2192 It’s convenient to keep a 10% stock solution and dilute it as needed. For dilution instructions, see the guide below.<\/p>\n

\u5869\u9178\u30fb\u786b\u9178\u30fb\u30a2\u30f3\u30e2\u30cb\u30a2\u30fb\u5869\u5316\u9285\u306e\u5e0c\u91c8\u306e\u65b9\u6cd5\uff08\u5e0c\u91c8\u306e\u57fa\u672c\u3092\u62bc\u3055\u3048\u3088\u3046\uff01\uff5e\u85ac\u54c1\u306e\u6b63\u3057\u3044\u4f7f\u3044\u65b9\u3068\u6388\u696d\u6e96\u5099\uff5e\uff09<\/a><\/p><\/blockquote>\n