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Reactions in Aqueous Solutions

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What happens when you put

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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?

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.

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 bu using solubility table 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)