Write the ions present in a solution of Na
3
PO
4
.
Express your answers as chemical formulas separated by a comma. Offset subscripts and charges on each ion.
The Correct Answer and Explanation is :
In a solution of sodium phosphate, ( \text{Na}_3\text{PO}_4 ), the ions present are:
Na(^{+}), PO(_4^{3-})
Explanation
When sodium phosphate (( \text{Na}_3\text{PO}_4 )) dissolves in water, it dissociates into ions. Dissociation is a process where ionic compounds separate into their respective cations (positive ions) and anions (negative ions) when they dissolve in a solvent like water. This happens because water molecules are polar, meaning they have a partial positive charge on one end and a partial negative charge on the other. The negative ends of water molecules attract the positive ions, and the positive ends attract the negative ions, helping to pull the compound apart.
In the case of sodium phosphate:
- Sodium ions (Na(^+)):
Sodium phosphate has three sodium ions (( \text{Na}^+ )) for every phosphate ion. Each sodium ion carries a ( +1 ) charge. As the compound dissolves, these sodium ions separate and become free-floating in the solution. So, you get three ( \text{Na}^+ ) ions per formula unit of sodium phosphate. - Phosphate ion (PO(_4^{3-})):
The phosphate ion has a ( 3- ) charge. When sodium phosphate dissociates, the phosphate ion remains as one unit with this charge.
The balanced equation representing the dissociation is:
[
\text{Na}_3\text{PO}_4 \rightarrow 3\text{Na}^+ + \text{PO}_4^{3-}
]
Each sodium ion and the phosphate ion are surrounded by water molecules, stabilizing them in solution. This dissociation is crucial in various applications, including biochemical reactions where phosphate ions are needed as reactants or in pH buffering.