Potassium phosphate (K₃PO₄) dissolves readily in water.
Potassium phosphate dissolves in water, forming an aqueous solution. When represented in a chemical equation, this dissolution is indicated by the notation (aq) following the chemical formula K₃PO₄.
Understanding the Dissolution
Potassium phosphate is an ionic compound. When ionic compounds like potassium phosphate are added to water, the polar water molecules surround and attract the individual ions (potassium cations, K⁺, and phosphate anions, PO₄³⁻), pulling them away from the crystal lattice. This process is known as solvation or hydration when water is the solvent.
According to the reference provided, writing K₃PO₄(aq) in a chemical equation explicitly states that the potassium phosphate is dissolved in water.
- Chemical Notation: The notation (aq) stands for "aqueous," meaning "dissolved in water."
- Reference Insight: As stated in the reference, "because we wrote aq on this side of the equation. We're saying it's dissolved in water." This confirms that the (aq) symbol is the standard way to indicate that a substance like potassium phosphate is in an aqueous solution. The reference also notes that you don't need to explicitly write water again on the same side of the equation when using (aq), as the symbol inherently implies the presence of water as the solvent.
Practical Considerations (Implied by Solubility)
While the reference focuses on the chemical representation, the fact that K₃PO₄ is highly soluble means:
- Adding to Water: When potassium phosphate solid is added to water, it will disperse and dissolve over time, often sped up by stirring.
- Solution Formation: The result is a homogeneous mixture where the potassium and phosphate ions are distributed throughout the water.
In summary, potassium phosphate dissolves in water because it is a soluble ionic compound. This state is represented chemically as K₃PO₄(aq).
