What are the net ionic equations for: 1. Potassium Fluoride and Ammonium Chloride and 2. Sodium Hydrogen Sulfite and Potassium Cyanide?
To determine the net ionic equations for the given reactions, we need to identify the ions involved and determine the products formed. Let's break down each reaction step by step:
1. Potassium Fluoride (KF) and Ammonium Chloride (NH4Cl):
The chemical equation for this reaction is:
KF + NH4Cl → ?
Step 1: Write the dissociation equations for the compounds:
KF → K+ + F-
NH4Cl → NH4+ + Cl-
Step 2: Identify the exchange of ions:
K+ from KF combines with Cl- from NH4Cl to form KCl.
F- from KF combines with NH4+ from NH4Cl to form NH4F.
Step 3: Write the net ionic equation by removing the spectator ions:
The spectator ions are K+ and Cl-. They are present on both sides of the equation, so they can be ignored.
The net ionic equation for the reaction is:
F- + NH4+ → NH4F
2. Sodium Hydrogen Sulfite (NaHSO3) and Potassium Cyanide (KCN):
The chemical equation for this reaction is:
NaHSO3 + KCN → ?
Step 1: Write the dissociation equations for the compounds:
NaHSO3 → Na+ + HSO3-
KCN → K+ + CN-
Step 2: Identify the exchange of ions:
Na+ from NaHSO3 combines with CN- from KCN to form NaCN.
HSO3- from NaHSO3 combines with K+ from KCN to form KHSO3.
Step 3: Write the net ionic equation by removing the spectator ions:
The spectator ions are Na+ and HSO3-. They are present on both sides of the equation, so they can be ignored.
The net ionic equation for the reaction is:
CN- + K+ → KCN
By following these steps, we can determine the net ionic equations for these chemical reactions.