Question #f4231

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Question #f4231

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Answer 1 · 2014-10-09T02:21:50

${AgNO}_{3(aq]} + {HCl}_{(aq]} \to {AgCl}_{(s]} + {HNO}_{3(aq]}$ $"AgNO"_text(3(aq]) + "HCl"_text((aq]) -> "AgCl"_text((s]) + "HNO"_text(3(aq])$

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

${AgNO}_{3(aq]} + {HCl}_{(aq]} \to {AgCl}_{(s]} + {HNO}_{3(aq]}$ $"AgNO"_text(3(aq]) + "HCl"_text((aq]) -> "AgCl"_text((s]) + "HNO"_text(3(aq])$

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

$1 mole$ $"1 mole"$ of ${AgNO}_{3}$ $"AgNO"_3$ contains $1 mole$ $"1 mole"$ of ${Ag}^{+}$ $"Ag"^+$ and $1 mole$ $"1 mole"$ of ${NO}_{3}^{-}$ $"NO"_3^-$ ions.

${Ag}_{(aq]}^{+} + {NO}_{3(aq]}^{-} + H_{(aq]}^{+} + {Cl}_{(aq]}^{-} \to {AgCl}_{(s]} ⏐ ⏐ ↓ + H_{(aq]}^{+} + {NO}_{3(aq]}^{-}$ $"Ag"_text((aq])^(+) + "NO"_text(3(aq])^(-) + "H"_text((aq])^(+) + "Cl"_text((aq])^(-) -> "AgCl"_text((s]) darr + "H"_text((aq])^(+) + "NO"_text(3(aq])^(-)$

The net ionic equation is

${Ag}_{(aq]}^{+} + {Cl}_{(aq]}^{-} \to {AgCl}_{(s]} ⏐ ⏐ ↓$ $"Ag"_text((aq])^(+) + "Cl"_text((aq])^(-) -> "AgCl"_text((s]) darr$

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Question #f4231

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