solubility rules
DESCRIPTION
Solubility Rules. Explain examples of solubility and precipitation at both the particle and symbolic levels. Use a table of solubility rules to predict the formation of a precipitate. Additional KEY Terms ppt spectator ion. Solubility: - PowerPoint PPT PresentationTRANSCRIPT
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• Explain examples of solubility and precipitation at both the particle and symbolic levels.
• Use a table of solubility rules to predict the
formation of a precipitate.
Additional KEY Termsppt spectator ion
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The terms soluble and insoluble are relative terms.
soluble soluble insoluble
solute
Solubility:The amount of solute needed to make a saturated
solution, under given conditions.
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Precipitation (ppt) reaction:Formation of an ionic compound that is not soluble in the current solvent.
Usually SR or chemical reactions
Spectator ions - do not participate, remain moving freely in solution.
DR DR
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There are many different ways to present RULES for what will dissolve and what will NOT (ppt)
Basic Solubility Rules (View 1)
1. All ionic compounds containing Group 1 elements, H+ and ammonium ion are soluble.
2. All ionic compounds with Group VII elements (other than F) and metals are soluble, except those of Ag+, Hg+1, and Pb+2.
3. All acetates and nitrates are soluble.4. All sulfates are soluble except those of Ba+, Sr+2, Pb+2, Ca+2,
Ag+, Hg+1.
5. Carbonates, hydroxides, oxides, sulfides, phosphates, chromates and dichromates are soluble; ONLY when bonded with those in rule 1.
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Basic Solubility Rules (View 2)
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Using the Solubility rules:*Assuming the reactants will dissolve… 1. Predict the products of the reaction 2. Check RULES to see if each product will ppt
NaCl(aq) + KBr(aq)
NaCl (s) Na+ (aq) + Cl- (aq)
KBr (s) K+ (aq) + Br - (aq)
NaBr(aq) + KCl(aq)
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Indicate if any of the product form a precipitate (ppt).
KOH (aq) + AgNO3 (aq)
Calcium nitrate + sodium carbonate
KNO3 (aq) + AgOH (aq)
Ca(NO3)2 + Na2CO3 CaCO3 + NaNO3
ppt
ppt2
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Indicate if any of the product form a precipitate (ppt).
Na2SO4 (aq) + KCl (aq)
Iron (III) chloride + lead (II) nitrate
2 NaCl (aq) + K2SO4 (aq) 2
FeCl3 + Pb(NO3)2 3 2 Fe(NO3)3 + 3 PbCl2 2ppt
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AgNO3(aq) + NaCl(aq) → AgCl(s) + NaNO3(aq)
The complete ionic equation shows all ions in their dissociated form.
Ag+(aq) + NO3
−(aq) + Na+
(aq) + Cl−(aq) → AgCl(s) + Na+
(aq) + NO3−
(aq)
The net ionic equation shows the actual reaction that occurs – no spectators:
Ag+(aq) + Cl−
(aq) → AgCl(s)
Spectator ions
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Write the molecular equation and the net ionic equation for the reaction between aqueous lead (II) nitrate and aqueous potassium iodide.
Pb(NO3)2(aq) + 2 KI(aq) → PbI2(s) + 2 KNO3(aq)
Pb2+(aq) + 2 I−
(aq) → PbI2(s)
Spectator ions
K+ NO3−
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CAN YOU / HAVE YOU?
• Explain examples of solubility and precipitation at both the particle and symbolic levels.
• Use a table of solubility rules to predict the
formation of a precipitate.
Additional KEY Termsppt spectator ion