Write the net ionic equation for the following molecular equation. HBr is a strong electrolyte. HClO is a weak electrolyte.
KClO(aq) + HBr(aq) KBr(aq) + HClO(aq)
ClO^-(aq) + H^+(aq) --> HClO(aq)
To write the net ionic equation, we need to break down the compounds into their ions and exclude the spectator ions.
The given molecular equation is:
KClO(aq) + HBr(aq) → KBr(aq) + HClO(aq)
Step 1: Write the balanced molecular equation:
KClO(aq) + HBr(aq) → KBr(aq) + HClO(aq)
Step 2: Identify the strong electrolyte. In this case, HBr is a strong electrolyte. It will dissociate completely into ions in solution:
HBr(aq) → H+(aq) + Br-(aq)
Step 3: Identify the weak electrolyte. In this case, HClO is a weak electrolyte. It will partially dissociate into ions:
HClO(aq) ⇌ H+(aq) + ClO-(aq)
Step 4: Write the net ionic equation by eliminating the spectator ions (ions that appear on both sides of the equation):
HBr(aq) + ClO-(aq) → HClO(aq) + Br-(aq)
So, the net ionic equation for the given molecular equation is:
HBr(aq) + ClO-(aq) → HClO(aq) + Br-(aq)
To write the net ionic equation, we first start with the balanced molecular equation:
KClO(aq) + HBr(aq) → KBr(aq) + HClO(aq)
Next, we need to identify the compounds that are strong electrolytes and dissociate completely in solution. In this case, HBr is a strong electrolyte, which means it dissociates into ions in solution.
HBr(aq) → H+(aq) + Br-(aq)
On the other hand, HClO is a weak electrolyte, so it does not fully dissociate in solution. Therefore, it remains as a molecular compound.
Now, let's write the net ionic equation by eliminating the spectator ions (ions that appear on both sides of the equation and do not participate in the net reaction). In this case, potassium ions (K+) and bromide ions (Br-) are spectator ions. That leaves us with the following net ionic equation:
HBr(aq) + ClO-(aq) → HClO(aq)
So, the net ionic equation for the given molecular equation is:
HBr(aq) + ClO-(aq) → HClO(aq)