# Net ionic equations (NaOH; HCl; H2O)

berry2
Hi,

I completed a Grade 12 experiment and now I am doing some calculations about it but I am confused.

Here is the question: "Write the net ionic equation for each reaction, and note the value of ΔH for each reaction. e.g. H+(aq) + OH-(aq) --> H2O(l)
ΔH = -45 kJ/mol HaOH

1. Heat of dissolution of NaOH; 200 mL of labelled water + 5.5 g of crystal NaOH

2. Heat of reaction between aqueous NaOH and aqueous HCl; 100 mL of 1.0 mol/L HCl + 100 mL of 1.0 mol/L NaOH

3. Heat of reaction between solid NaOH and aqueous HCl; 200 mL of 1.0 mol/L HCl + 5.5g of crystal NaOH

These were the instructions also given: "Since all the solutions are dilute, then the density of each solution can be assumed to be 1.00 g/mL. So, 100 mL has a mass of 100 g."

So for the first reaction, would the net ionic equation be something like this:
1. 200 g H2O(l) + 5.5 g NaOH(s) --> I don't know what the product would be?
2. 100 g HCl(aq) + 100 g NaOH(aq) --> NaCl + H2O?
3. 200 g of HCl(aq) + 5.5 g NaOH(s) --> NaCl + H2O?

Any help would really be appreciated! Thanks