No, calcium chloride does not react with sodium nitrate.
Based on chemical principles and the provided reference, calcium chloride (CaCl₂) does not react with sodium nitrate (NaNO₃). When these two ionic compounds are mixed in an aqueous solution, no precipitate, gas, or water is formed, which are the typical indicators of a chemical reaction in a double displacement (metathesis) context.
The potential products of a double displacement reaction between calcium chloride and sodium nitrate would be calcium nitrate (Ca(NO₃)₂) and sodium chloride (NaCl). Both of these potential products are highly soluble in water.
- Calcium Nitrate (Ca(NO₃)₂): Nitrates are almost universally soluble.
- Sodium Chloride (NaCl): Alkali metal salts (like sodium salts) and chlorides are generally soluble (with exceptions like AgCl, PbCl₂, Hg₂Cl₂).
Because all potential products remain dissolved in the solution, there is no driving force for a reaction to occur. All ions – calcium ions (Ca²⁺), chloride ions (Cl⁻), sodium ions (Na⁺), and nitrate ions (NO₃⁻) – simply remain as solvated ions in the solution, unchanged.
Why No Reaction Occurs
The provided reference directly confirms this lack of reaction:
"So there's no reaction. And no net ionic equation for nano3 plus ca cl2."
This statement from the video underscores that since no new insoluble compound (precipitate), gas, or water is formed, the ions present before mixing are the same as those present after mixing, making it a "no reaction" scenario. Consequently, there is no net ionic equation to represent any chemical change.
Summary of Interaction
To further illustrate the lack of reaction, consider the components:
| Component | Chemical Formula | State in Solution |
|---|---|---|
| Calcium Chloride | CaCl₂ | Ca²⁺(aq) + 2Cl⁻(aq) |
| Sodium Nitrate | NaNO₃ | Na⁺(aq) + NO₃⁻(aq) |
When mixed, if a reaction were to occur, the ions would swap partners:
| Expected Potential Product | Solubility | Outcome |
|---|---|---|
| Calcium Nitrate | Soluble | Remains as Ca²⁺(aq) + 2NO₃⁻(aq) |
| Sodium Chloride | Soluble | Remains as Na⁺(aq) + Cl⁻(aq) |
Since all ions remain in solution, they are all considered spectator ions, and therefore, no overall chemical reaction takes place.
