What happens when you put

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Reactions in Aqueous Solutions

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Reactions in Aqueous Solutions

Reactions in Aqueous Solutions

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Presentation transcript:

What happens when you put AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq) What happens when you put AgNO3 and NaCl in water?

What really happens when you put AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq) What really happens when you put AgNO3 and NaCl in water?

NaCl (aq) Na +1 (aq) + Cl -1 (aq) KEY POINT: really means: “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) 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:

Mg(NO3)2 (aq) Mg +2 (aq) + (NO3) -1 (aq) 2 KEY POINT: really means: “dissociated ions” or “ions in solution”

KEY POINT: AgCl (s) really means: Solid Silver (I) Chloride.

What happens when you put 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+ AgCl(s)

AgNO3 (aq) + NaCl(aq) AgCl(s) + NaNO3(aq) complete ionic equation

Na+ NO3- AgCl 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

net ionic equation

net ionic equation

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