Question #f4231

1 Answer
Manish Bhardwaj · Stefan V.
Oct 9, 2014

#"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#

Related questions
See all questions in Balancing Chemical Equations
Impact of this question
78259 views around the world
You can reuse this answer
Creative Commons License