Write the net ionic equation for the following molecular equation. HNO3 is a strong electrolyte.

NaNO2(aq) + HNO3(aq)--> NaNO3(aq) + HNO2(aq)
HNO2 is a weak electrolyte.

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To write the net ionic equation, we need to first identify the strong electrolyte(s) and the weak electrolyte(s).

In this case, HNO3 is a strong electrolyte, while HNO2 is a weak electrolyte.

The next step is to write the balanced molecular equation:

NaNO2(aq) + HNO3(aq) → NaNO3(aq) + HNO2(aq)

To write the net ionic equation, we remove the spectator ions, which are the ions that do not participate in the chemical reaction. In this case, Na+ and NO3- are spectator ions.

The net ionic equation would be:

H+ (aq) + NO2- (aq) → HNO2 (aq)

To write the net ionic equation, we need to first write out the molecular equation:

NaNO2(aq) + HNO3(aq) --> NaNO3(aq) + HNO2(aq)

Next, we need to identify the strong electrolyte and weak electrolyte. It is given that HNO3 is a strong electrolyte, while HNO2 is a weak electrolyte.

A strong electrolyte dissociates completely into its ions when dissolved in water, while a weak electrolyte only partially dissociates into its ions.

Since HNO3 is a strong electrolyte, it dissociates completely into its ions:

HNO3(aq) -> H+(aq) + NO3-(aq)

NaNO2(aq) -> Na+(aq) + NO2-(aq)

However, we know that HNO2 is a weak electrolyte, so it only partially ionizes in water:

HNO2(aq) <-> H+(aq) + NO2-(aq)

Now, we can 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 reaction). The spectator ions here are Na+ and NO3-.

Net ionic equation: HNO3(aq) + HNO2(aq) -> H+(aq) + NO2-(aq)

This is the net ionic equation that represents the actual reaction taking place between NaNO2(aq) and HNO3(aq), where the strong electrolyte HNO3 reacts with the weak electrolyte HNO2 to produce H+ and NO2-.

NO2 + H^+ ==> HNO2