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Unit 1 – reactions in aqueous solutions Lesson 2
Chemistry 40S Unit 1 – reactions in aqueous solutions Lesson 2
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Learning outcomes C : Perform a laboratory activity to develop a set of solubility rules C : Use a table of solubility rules to predict the formation of a precipitate
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Solubility rules Solubility rules allow people to predict if a precipitate will form, and if one does---what it is! Solubility rules rely on standard known solubilities for ions at STP (standard temperature and pressure: 0C and kPa) In order to use the solubility rules to your advantage when predicting the product of the combination of two ionic solutions you must be able to write a net ionic equation
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Writing net ionic equations
Step 1: Predict the products of the reaction and ensure that the equation is balanced Think double-displacement reaction Example: Reaction between BaCl2 and Na2SO4 BaCl2 + Na2SO4 BaSO4 + NaCl
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Writing net ionic equations
Step 2: Balance the equation BaCl2 + Na2SO4 BaSO4 + 2NaCl
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Writing net ionic equations
Step 3: Use a table of solubility rules to identify which ionic substances will precipitate from aqueous solutions Precipitate is a solid give it an ‘s’ subscript and the rest an ‘aq’ subscript BaCl2(aq) + Na2SO4(aq) BaSO4(s) + 2NaCl(aq) This is known as a balanced molecular equation
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Writing net ionic equations
Step 4: Separate the aqueous solutions into their ions Ba2+ (aq) + 2Cl- (aq) + 2Na+(aq) + SO42-(aq) BaSO4(s) + 2Na+(aq) + 2Cl-(aq) This is known as an ionic equation
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Writing net ionic equations
Step 5: Cancel out spectator ions Ba2+ (aq) + 2Cl- (aq) + 2Na+(aq) + SO42-(aq) BaSO4(s) + 2Na+(aq) + 2Cl-(aq) Ba2+ (aq) + SO42-(aq) BaSO4(s) This is a net ionic equation
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Solubility rules A set of rules to help you predict if and what precipitate will form when combining ionic solutions.
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