The addition of a crystal of sodium chlorate to a sodium chlorate solution containing no undissolved solute causes additional crystals of sodium chlorate to precipitate. The original solution was supersaturated or unsaturated
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The original solution was supersaturated.
In order to determine whether the original solution was supersaturated or unsaturated, we need to understand the concept of supersaturation.
Supersaturation occurs when a solution contains more dissolved solute than would normally be possible at its current temperature and pressure. This can happen when a solution is heated and then slowly cooled, allowing it to hold more solute than it would under normal conditions.
On the other hand, an unsaturated solution is one that has the capacity to dissolve more solute. It contains less solute than the maximum amount the solution could hold at its current temperature and pressure.
In the given scenario, when a crystal of sodium chlorate is added to a sodium chlorate solution containing no undissolved solute, and additional crystals of sodium chlorate precipitate, it indicates that the original solution was supersaturated.
The reason for this is that when a seed crystal, such as the one added, is introduced into a supersaturated solution, it provides a solid surface for the solute to crystallize onto. This triggers the precipitation of additional solute molecules, forming crystals.
In an unsaturated solution, there would be no precipitation because the solution has the capacity to dissolve more solute. Only when a solution is supersaturated does the precipitation occur.
Therefore, based on the observation that additional crystals of sodium chlorate precipitate when a crystal is added, we can conclude that the original solution was supersaturated.