Question

Question #f4231

Answer 1

`"AgNO"_text(3(aq]) + "HCl"_text((aq]) -> "AgCl"_text((s]) + "HNO"_text(3(aq])`

Explanation:

To write the complete ionic equation:

• Start with a balanced molecular equation.
• Break all soluble strong electrolytes (compounds with (aq) beside them) into their ions
• indicate the correct formula and charge of each ion
  indicate the correct number of each ion
  write (aq) after each ion
• Bring down all compounds with (s), (l), or (g) unchanged.

The molecular equation is

`"AgNO"_text(3(aq]) + "HCl"_text((aq]) -> "AgCl"_text((s]) + "HNO"_text(3(aq])`

How did I get this equation? Consider each reactant or product separately:

`"1 mole"` of `"AgNO"_3` contains `"1 mole"` of `"Ag"^+` and `"1 mole"` of `"NO"_3^-` ions.

`"Ag"_text((aq])^(+) + "NO"_text(3(aq])^(-) + "H"_text((aq])^(+) + "Cl"_text((aq])^(-) -> "AgCl"_text((s]) darr + "H"_text((aq])^(+) + "NO"_text(3(aq])^(-)`

The net ionic equation is

`"Ag"_text((aq])^(+) + "Cl"_text((aq])^(-) -> "AgCl"_text((s]) darr`