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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 )

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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 ) - PowerPoint PPT Presentation

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Page 1: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

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

What happens when you put

AgNO3 and NaCl in water?

Page 2: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

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

What really happens when you put

AgNO3 and NaCl in water?

Page 3: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

KEY POINT:

NaCl (aq)

really means:

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

“dissociated ions”or “ions in solution”

Page 4: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

What is Dissolving ?

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

Ex: Ca(NOEx: Ca(NO33))22(s)(s) Ca Ca2+2+(aq)(aq) + 2NO + 2NO33--(aq)(aq)

)(2 lOH

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

Page 5: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

An Ionic Compound Dissolves:

A Covalent Compound Dissolves:

Page 6: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

KEY POINT:

Mg(NO3)2 (aq)

really means:

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

“dissociated ions”or “ions in solution”

Page 7: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

KEY POINT:

AgCl (s)

really means:

AgCl (s)

Solid Silver (I) Chloride.

Page 8: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

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

What happens when you put

AgNO3 and NaCl in water?

Page 9: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

AgNO3 NaCl

Page 10: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

Ag+

NO3-

Na+

Cl-

Page 11: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

Ag+

NO3-

Na+

Cl-

Page 12: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

AgCl

NO3-

Na+

Page 13: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

AgCl

NO3-

Na+

AgCl(s)precipitate

Page 14: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

NO3-

Na+

NO3-Na+

NO3-

Na+NO3-Na+Na+ NO3

-

Na+

NO3- Na+

NO3-

Na+

NO3-

Na+

AgCl(s)

Page 15: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)

AgCl (s) + NO3- (aq) + Na+ (aq)

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

complete ionic equation

Page 16: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

NO3- Na+

AgCl

Reaction

Page 17: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

AgCl

NO3- Na+

No Reaction

Page 18: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

AgCl

NO3- Na+

These ions do not participatein the reaction. They are called

SPECTATOR IONS

Page 19: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)

AgCl (s) + NO3- (aq) + Na+ (aq)

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

Page 20: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)

AgCl (s) + NO3- (aq) + Na+ (aq)

NO3- and Na+ are not participating in the reaction

Page 21: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)

AgCl (s) + NO3- (aq) + Na+ (aq)

net ionic equation

Ag+ (aq) + Cl- (aq) AgCl (s)

Page 22: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)

AgCl (s) + NO3- (aq) + Na+ (aq)

net ionic equation

Ag+ (aq) + Cl- (aq) AgCl (s)

Page 23: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

– 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

Page 24: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

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)

Page 25: AgNO 3  ( aq )   +   NaCl( aq )           AgCl( s )   +   NaNO 3 ( aq )

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)link