Question

Cobalt(II) chloride hexahydrate, dissolves readily in water to give a red solution. If we use this solution as an "ink," we can write secret messages on paper. The writing is not visible when the water evaporates from the paper. When the paper is heated, however, the message can be read. Explain the chemistry behind this observation. (IMAGE CAN'T COPY)

Short answer

The color change is due to the reversible hydration and dehydration of cobalt(II) chloride, altering its color upon heating.

Step-by-step solution

Understanding Cobalt(II) Chloride Hexahydrate

Cobalt(II) chloride hexahydrate, with the formula \( CoCl_2 \, \cdot \, 6H_2O \), is a complex of cobalt chloride and water. In its hydrated form, this compound typically appears as a pink solid due to its molecular structure incorporating water molecules.

Dissolution in Water

When dissolved in water, cobalt(II) chloride hexahydrate forms a red solution. The water molecules coordinate with the cobalt ion, creating a complex that intensifies the red color, making it useful as an 'ink' for writing.

Evaporation of Water

As the water evaporates from the paper, the cobalt(II) chloride remains but becomes nearly invisible because it is in its anhydrous form or less hydrated form that is less distinct visually.

Heating and Message Revelation

When the paper is heated, the anhydrous cobalt chloride or less hydrated forms absorb water from the moisture in the air. They convert back to a partially hydrated or hydrated form, which is visually distinct, allowing the red color to reappear and the message to become visible again.

Chemical Explanation

The color change upon heating is due to the reversible reaction of cobalt(II) chloride with water:\[CoCl_2 (s) + 6H_2O (l) \rightleftharpoons Co(H_2O)_6^{2+} (aq) + 2Cl^{-} (aq)\]Heating drives the reaction to the left, reverting to a form where moisture collection changes the visible color due to coordination complex changes.

Key concepts

Cobalt(II) Chloride Hexahydrate

Cobalt(II) chloride hexahydrate is an interesting compound with the chemical formula \( CoCl_2 \cdot 6H_2O \). This molecule consists of cobalt chloride bonded with six water molecules, which is what we refer to as its 'hydrated' form.

• The hydrated form typically appears pink due to the presence of water molecules that influence its color.
• These water molecules play a crucial role in the structure and color of cobalt(II) chloride hexahydrate.

Understanding this compound's hydrated nature is vital when discussing its applications, such as in secret inks or desiccants. When heated or introduced to moisture, its hydration state changes, which leads to color changes. This ability makes it useful for practical applications like the one described in the exercise, where it can reveal hidden messages.

Coordination Complex

A coordination complex involves a central metal atom bonded to surrounding molecules or ions, known as ligands. Cobalt(II) chloride hexahydrate forms such a complex in solution.

• The cobalt ion, \( Co^{2+} \), is the central metal ion.
• Water molecules act as ligands, coordinating with the metal ion.

When cobalt(II) chloride hexahydrate dissolves in water, the water molecules coordinate around the cobalt ion, forming a complex. This complex is responsible for the distinct red color observed in the solution. Understanding coordination complexes helps explain how metal ions such as cobalt can influence the color and behavior of solutions.

Reversible Reactions

Reversible reactions are chemical reactions where the products can re-form the reactants. This is an essential concept in the discussed exercise. The reversible reaction of cobalt(II) chloride with water is:\[CoCl_2 (s) + 6H_2O (l) \rightleftharpoons Co(H_2O)_6^{2+} (aq) + 2Cl^{-} (aq)\]

• In one direction, water is added to the cobalt chloride, which dissolves and results in the red-colored hydrated form.
• When water is removed (as during evaporation), the reaction can reverse.

This reversible nature explains why heating the paper reveals the hidden message. Upon heating, the cobalt chloride absorbs moisture from the air, triggering the reverse reaction and causing the color to reappear.

Hydration and Dehydration

Hydration and dehydration involve the addition or removal of water molecules, and they significantly influence chemical and physical properties. For cobalt(II) chloride, these processes are directly linked to color changes observed in the exercise.

Hydration Process

• In hydrated form, cobalt(II) chloride is pink due to the coordinated water molecules.
• During hydration, adding water results in the formation of a red solution when dissolved.

Dehydration Process

• When water is removed through evaporation, cobalt(II) chloride becomes less hydrated or anhydrous, appearing nearly invisible.
• Dehydration can be reversed by reintroducing water, as seen when heating reveals the red message. The paper, when heated, helps the compound collect moisture from the air, becoming hydrated once more.

This cycling between hydration and dehydration forms the foundation of how cobalt(II) chloride hexahydrate functions in secret ink and similar applications.