As we saw in section 4.3, nitric acid and hydrochloric acid are strong acids. write net ionic equations for the neutralization of the nitric acid.

First you write the "molecular" equation, then the ionic equation, and finally the net ionic equation.

You can read about these equations at

Here are the steps for your reaction.

1. Write the molecular equation

We write the equation as if all the reactants were molecules.

2HNO₃(aq) + Mg(OH)₂(s) → 2H₂O(l) + Mg(NO₃)₂(aq

2. Write the ionic equation

We write all the soluble strong electrolytes as ions. H₂O is a weak electrolyte, so we write it as a molecule. Mg(OH)₂ is insoluble, so we write it as a molecule as well.

2H⁺(aq) + 2NO₃⁻(aq) + Mg(OH)₂(s) → 2H₂O(l) + Mg²⁺(aq) + 2NO₃⁻(aq)

3. Write the net ionic equation

Here, we cancel all species that appear on both sides of the equation. We cancel the NO₃⁻ ions.

The net ionic equation is

2H⁺(aq) + Mg(OH)₂(s) → 2H₂O(l) + Mg²⁺(aq)

the answer is a. co2, this would be colder than the : )

explanation:

when the volume of gas is   changed from   717.73 ml   to 852 ml   the temperature will   change   from 315   c to 452   c

    calculation

this is calculated using the charles law formula

that is,   v1/t1 = v2/t2

          v1=?

        t1 = 315 c   into   kelvin = 315 +273 = 588 k

        v2 = 852   ml

        t2 = 425c + 273 =698 k

make v1   the subject of the formula ( by   multiplying both side by t1)

  v1=( v2 xt1) / t2

v1= (852 ml   x 588 k)/ 698 k= 717.73 ml