AgNO 3 (aq) + NaCl(aq) AgCl(s) + NaNO 3 (aq) What happens when you put AgNO 3 and NaCl in water?
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Transcript of AgNO 3 (aq) + NaCl(aq) AgCl(s) + NaNO 3 (aq) What happens when you put AgNO 3 and NaCl in water?
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 ?
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.
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
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 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)link