What is the complete ionic equation for H3PO4(aq)+3KOH(aq)—>3H2O(l)+K3PO4(aq)
H3PO4(aq) + 3KOH(aq)—>3H2O(l) + K3PO4(aq)
3H^+(aq) + [PO4]^3-(aq) + 3K^+(aq) + 3OH^-(aq)—>3H2O(l) + 3K^+(aq) + [(PO4]^3-(aq)
To determine the complete ionic equation for the reaction between H3PO4(aq) and 3KOH(aq), we need to first write the balanced chemical equation:
H3PO4(aq) + 3KOH(aq) → 3H2O(l) + K3PO4(aq)
Next, we dissociate the strong electrolytes (compounds that fully dissociate in water) into their respective ions:
H3PO4(aq) → 3H+(aq) + PO4^3-(aq)
3KOH(aq) → 3K+(aq) + 3OH-(aq)
3H2O(l) → 3H2O(l)
K3PO4(aq) → 3K+(aq) + PO4^3-(aq)
Finally, we can write the complete ionic equation by replacing the soluble strong electrolytes with their respective ions:
3H+(aq) + PO4^3-(aq) + 3K+(aq) + 3OH-(aq) → 3H2O(l) + 3K+(aq) + PO4^3-(aq)
So, the complete ionic equation for the reaction is:
3H+(aq) + 3OH-(aq) → 3H2O(l)
To write the complete ionic equation for the reaction between H3PO4(aq) and 3KOH(aq) to produce 3H2O(l) and K3PO4(aq), you need to break down all the compounds into their individual ions.
First, let's write the balanced molecular equation:
H3PO4(aq) + 3KOH(aq) → 3H2O(l) + K3PO4(aq)
Now, let's break down the compounds into their respective ions:
H3PO4(aq): H+(aq) + H2PO4^-(aq)
3KOH(aq): 3K+(aq) + 3OH^-(aq)
3H2O(l): 3H2O(l)
K3PO4(aq): 3K+(aq) + PO4^3-(aq)
Next, we can write the complete ionic equation by including all the ions:
H+(aq) + H2PO4^-(aq) + 3K+(aq) + 3OH^-(aq) → 3H2O(l) + 3K+(aq) + PO4^3-(aq)
Finally, we can cancel out any spectator ions that appear on both sides of the equation. In this case, the K+ ions are spectator ions since they appear on both sides:
H+(aq) + H2PO4^-(aq) + 3OH^-(aq) → 3H2O(l) + PO4^3-(aq)
Therefore, the complete ionic equation is:
H+(aq) + H2PO4^-(aq) + 3OH^-(aq) → 3H2O(l) + PO4^3-(aq)