The dissolution of sodium chloride (NaCl) in water can be described by the following equation:
\[ \text{NaCl (s)} \rightleftharpoons \text{Na}^+ (aq) + \text{Cl}^- (aq) \]
In this equation, solid sodium chloride (NaCl) dissociates into sodium ions (Na⁺) and chloride ions (Cl⁻) in an aqueous solution (water).
Activity Completion:
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Describe the Process: When NaCl is added to water, it begins to dissolve. The positive end of water molecules (hydrogen) surrounds the chloride ions, while the negative end (oxygen) surrounds the sodium ions. This leads to the dissociation of NaCl into its constituent ions.
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Equilibrium State:
- The process is reversible, which means that while NaCl dissolves to form Na⁺ and Cl⁻, under certain conditions (like high concentration), these ions can recombine to form solid NaCl: \[ \text{Na}^+ (aq) + \text{Cl}^- (aq) \rightleftharpoons \text{NaCl (s)} \]
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Factors Affecting Dissolution:
- Temperature: Increased temperature generally increases the solubility of NaCl in water.
- Stirring: Stirring the solution can also help dissolve NaCl faster by distributing the ions more evenly.
- Surface Area: Using smaller crystal sizes of NaCl increases the surface area for interaction with water, facilitating faster dissolution.
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Impact on Conductivity:
- When NaCl dissolves, it increases the electrical conductivity of water due to the presence of free-moving ions (Na⁺ and Cl⁻).
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Real-life Applications:
- Understanding the dissolution of NaCl is crucial in areas such as food preservation, formulation of saline solutions in medicine, and industrial processes.
By observing and understanding these factors, one can fully grasp the significance of the dissolution of sodium chloride in various contexts.