Question

When aqueous solutions of sodium cyanide and nitric acid are mixed, an aqueous solution of sodium nitrate and hydrocyanic acid results. Write the net ionic equation for the reaction.

Answer 1

Answer:

There is no net ionic equation

Explanation:

Step 1: Data given

sodium cyanide = NaCN

nitric acid = HNO3

sodium nitrate = NaNO3

hydrocyanic acid = HCN

Step 2: The unbalanced equation

NaCN(aq) + HNO3(aq) → NaNO3(aq) + HCN(aq)

The equation is already balanced.

Step 3: the net ionic equation

The net ionic equation, for which spectator ions are omitted - remember that spectator ions are those ions located on both sides of the equation - will , after canceling those spectator ions in both side, look like this:

Na+ + CN- + H+ NO3-   → Na+ + NO3- + H+ + CN-

There is no net ionic equation

If you don't have a net ionic equation to balance, that means you have what is usually called a molecular equation (or a complete molecular equation)

Answer 2

Answer:

There is no net ionic equation

Explanation:

We identify the reactants and the products for the reaction

NaCN, HNO₃, NaNO₃, HCN

In this case, they are all soluble in water (aq)

We write the reaction, by the ionic form

Na⁺(aq) + CN⁻ (aq) + H⁺ (aq) + NO₃⁻(aq)  → Na⁺(aq) + NO₃⁻(aq)  + H⁺(aq) + CN⁻(aq)

All of the ions are spectators, they all react so there is no net ionic equation