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AgNO 3 ( aq ) + NaCl( aq ) AgCl( s ) + NaNO 3 ( aq ) - PowerPoint PPT Presentation


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AgNO 3 ( aq ) + NaCl( aq ) AgCl( s ) + NaNO 3 ( aq ). What happens when you put AgNO 3 and NaCl in water?. AgNO 3 ( aq ) + NaCl( aq ) AgCl( s ) + NaNO 3 ( aq ). What really happens when you put AgNO 3 and NaCl in water?. KEY POINT: NaCl ( aq )

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AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq)

What happens when you put

AgNO3 and NaCl in water?


AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq)

What really happens when you put

AgNO3 and NaCl in water?


KEY POINT:

NaCl (aq)

really means:

Na +1(aq) + Cl -1(aq)

“dissociated ions”

or

“ions in solution”


What is dissolving
What is Dissolving ?

When an ionic compound (eg salt) dissolves in water, the compound disassociates. (breaks apart into cations and anions)

Ex: Ca(NO3)2(s)Ca2+(aq) + 2NO3-(aq)

When a covalent compound (eg sugar) dissolves in water, the molecules simply disperse; they do not disassociate. Molecules of the covalent compounds simply disperse due to attraction with polar water molecules.


An Ionic Compound Dissolves:

A Covalent Compound Dissolves:


KEY POINT:

Mg(NO3)2(aq)

really means:

Mg +2(aq) + (NO3) -1(aq)

2

“dissociated ions”

or

“ions in solution”


KEY POINT:

AgCl (s)

really means:

AgCl (s)

Solid Silver (I) Chloride.


AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq)

What happens when you put

AgNO3 and NaCl in water?


AgNO3

NaCl


NO3-

Na+

Ag+

Cl-


Na+

NO3-

Ag+

Cl-


Na+

NO3-

AgCl


Na+

NO3-

AgCl(s)

precipitate

AgCl


NO3-

Na+

NO3-

NO3-

Na+

Na+

Na+

NO3-

NO3-

Na+

Na+

Na+

NO3-

NO3-

Na+

NO3-

Na+

AgCl(s)


AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq)

complete ionic equation


AgCl

Na+

NO3-

Reaction


No Reaction

Na+

NO3-

AgCl


These ions do not participate

in the reaction. They are called

SPECTATOR IONS

Na+

NO3-

AgCl


The net ionic equation is constructed from the complete ionic equation:


NO3- and Na+ are not participating in the reaction




  • Complete molecular equation-

    • describes double replacement reaction

  • Complete ionic equation-

    • more accurately shows the reacting species as ions and the products either as ions or a precipitate

  • Net ionic equation-

    • focuses only on the ions REACTING

  • Spectator ions are those ions that do NOT participate in the reaction


Predicting the formation of a precipitate
PREDICTING THE FORMATION OF A PRECIPITATE

  • Consider the possibility that a precipitate may form.

  • Must use the solubility table on page 227 to decide.

  • Possible outcomes

    • No visible reaction (nvr)

    • Formation of one ppt.

    • Formation of two ppt. (rare occurrence)


Basic Chemical equation AgNO3(aq) + KCl(aq)AgCl(s) + KNO3(aq)

Complete ionic equation shows ions in solution Ag+ (aq)+NO3(aq) + K+ (aq)+Cl-(aq)AgCl(s) + K+ (aq) + NO3-(aq)

Net ionic equation shows ions in rxn Ag+ (aq)+Cl-(aq)AgCl(s)

(leave out spectator ions)

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