agno 3 ( aq ) + nacl ( aq ) agcl ( s ) + nano 3 ( aq )
DESCRIPTION
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: - PowerPoint PPT PresentationTRANSCRIPT
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”
KEY POINT:
AgNO3 (aq)
really means:
Ag +1 (aq) + NO3 -1 (aq)
“dissociated ions”or “ions in solution”
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)
)(2 lOH
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:
AgCl (s)
really means:
AgCl (s)
Solid Silver (I) Chloride.
KEY POINT:
NaNO3 (aq)
really means:
Na +1 (aq) + NO3 -1 (aq)
“dissociated ions”or “ions in solution”
AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq)
What happens
when you put
AgNO3 and NaCl
in water?
AgNO3 NaCl
Ag+
NO3-
Na+
Cl-
Ag+
NO3-
Na+
Cl-
AgCl
NO3-
Na+
AgCl
NO3-
Na+
AgCl(s)precipitate
NO3-
Na+
NO3-Na+
NO3-
Na+NO3-Na+Na+ NO3
-
Na+
NO3- Na+
NO3-
Na+
NO3-
Na+
AgCl(s)
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
NO3- Na+
AgCl
Reaction
AgCl
NO3-Na+
No Reaction
AgCl
NO3- Na+
These ions do not participatein the reaction. They are called
SPECTATOR IONS
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:
Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)
AgCl (s) + NO3- (aq) + Na+ (aq)
NO3- and Na+ are not participating in the reaction
Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)
AgCl (s) + NO3- (aq) + Na+ (aq)
net ionic equation
Ag+ (aq) + Cl- (aq) AgCl (s)
Ag+ (aq) + NO3- (aq) + Na+ (aq) + Cl- (aq)
AgCl (s) + NO3- (aq) + Na+ (aq)
net ionic equation
Ag+ (aq) + Cl- (aq) AgCl (s)
– 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
• Consider the possibility that a precipitate may form.
• Must use the solubility rules 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)