99.95% Pure Magnesium Ribbon: Lab Uses, Properties, Safety & Specifications

What Is Lab-Grade Magnesium Ribbon?

Magnesium ribbon is a thin, flexible strip of pure magnesium metal (Mg) with a bright silver surface. At 99.95% purity, lab-grade magnesium ribbon is free of impurities that would interfere with chemical reactions, making it the standard material for quantitative chemistry experiments, thermite demonstrations, and metal reactivity studies in high school, university, and professional research settings.

SciMed's Magnesium Ribbon — 99.95% Pure, 25g / 70ft Roll provides a generous supply ideal for classroom and lab use, with consistent ribbon width and thickness for reproducible results.

Chemical Properties

  • Symbol: Mg | Atomic Number: 12 | Atomic Mass: 24.31 g/mol
  • Melting Point: 650°C (1,202°F)
  • Boiling Point: 1,091°C (1,996°F)
  • Density: 1.74 g/cm³
  • Reactivity: Reacts with water (slowly), acids (vigorously), oxygen (burns with intense white flame)

Standard Laboratory Experiments Using Magnesium Ribbon

1. Combustion in Air (Classic Demonstration)

Magnesium burns in air with a brilliant white flame (3,100°C), producing magnesium oxide (MgO) and small amounts of magnesium nitride (Mg₃N₂). This reaction demonstrates the reactivity series, oxidation reactions, and energy changes. Safety note: Never look directly at burning magnesium without UV-protective goggles — the emitted UV light can cause eye damage.

Reaction: 2Mg + O₂ → 2MgO

2. Reaction with Hydrochloric Acid

Magnesium reacts vigorously with dilute HCl, producing hydrogen gas — used to demonstrate metal-acid reactivity, measure reaction rates, and collect gas for property tests (flammability, density).

Reaction: Mg + 2HCl → MgCl₂ + H₂↑

3. Reaction with Water and Steam

Magnesium reacts slowly with cold water but vigorously with steam, producing magnesium hydroxide and hydrogen. Used to demonstrate reactivity series position and displacement reactions.

4. Determination of Molar Mass (Stoichiometry)

By measuring the volume of hydrogen gas produced when a known mass of magnesium reacts with excess HCl (at measured temperature and pressure), students calculate the molar mass of magnesium using the ideal gas law — a classic quantitative experiment reinforcing mole concept.

5. Reduction of Metal Oxides (Thermite Variation)

Magnesium's high reactivity (above carbon in the reactivity series) allows it to reduce oxides of less reactive metals: Mg + CuO → MgO + Cu. Used in displacement reaction demonstrations.

Safety Handling and Storage

  • Store in a cool, dry location away from water, acids, and oxidizing agents
  • Keep in sealed container — surface oxidation reduces reactivity over time
  • Magnesium fires cannot be extinguished with water or CO₂ (reactions worsen). Use Class D dry powder extinguisher or dry sand
  • Wear UV-protective goggles when performing combustion demonstrations
  • Dispose according to local chemical waste regulations — do not dispose down drains

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