What is the net ionic equation of sodium fluoride solution added to sulfuric acid solution?

Step1: Write the balanced equation for the reaction:

`~2NaF + ~H_2SO_4 -gt ~Na_2SO_4 + ~2HF`

Step 2: Determine the states of all of the substances.

We know, from the question, that NaF and `~H_2SO_4` are aqueous solutions.

The product hydrofluoric acid (HF) is also an aqueous solution.

To determine the status of the product `~Na_2SO_4` , check a list of solubility rules. You can find a list of solubility rules by googling...

Step 1: Write the balanced equation for the reaction:

`~2NaF + ~H_2SO_4 -gt ~Na_2SO_4 + ~2HF`

Step 2: Determine the states of all of the substances.

We know, from the question, that NaF and `~H_2SO_4` are aqueous solutions.

The product hydrofluoric acid (HF) is also an aqueous solution.

To determine the status of the product `~Na_2SO_4` , check a list of solubility rules. You can find a list of solubility rules by googling "solubility rules" or looking in your textbook.

According to the solubility rules, compounds that contain sulfates are soluble (unless they also contain Pb, Ca, Sr, or Ba).

So, `~Na_2SO_4` is soluble (i.e. forms an aqueous solution).

Therefore, all of the substances in the reaction are aqueous solutions:

`~2NaF_(aq)` + `~H_2SO_4_(aq)` -> `~Na_2SO_4_(aq)` + `~2HF_(aq)`

Step 3: Write the net ionic equation if a reaction has occurred.

In this case, since all of the substances are soluble, there is no real change from the reactant side of the equation to the product side of the equation. In both cases, the solution contains the following dissolved ions: `~Na^+` ,` ~F^-` , `~H^+` ,  `~SO_4^2^-` .

Therefore, there is no net ionic equation.