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Review:.

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Presentation on theme: "Review:."— Presentation transcript:

1 Review:

2 Review: (b.) 5 grams of magnesium metal is dropped 20 mL of 3 M hydrochloric acid, HCl, producing hydrogen gas and magnesium chloride. If the hydrogen gas is collected under standard conditions, what volume is produced? If the experiment is performed, but only 0.5 L of H2 gas is collected at STP, what is the % yield?

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6 Net Ionic Equations: Sol’n stoich. can be tricky when aqueous ionic compounds are involved … Remember how ionic things dissociate? MgCl2 (aq)  Al(NO3)3 (aq) 

7 Pb(NO3)2 (aq) + NaI (aq)  PbI2 (s) + NaNO3 (aq)
Net Ionic Equations: Sol’n stoich. can be tricky when aqueous ionic compounds are involved … Pb(NO3)2 (aq) + NaI (aq)  PbI2 (s) + NaNO3 (aq) Reactions where 2 aqueous solutions produce an insoluble product are called precipitation reactions. Ionic equation: Net Ionic equation: DOUBLE REPLACEMENT REACTIONS: AB + CD  AD + CB

8 Remember Solubility Rules:
1). All common salts of the nitrate ion (NO3-) are soluble in water. 2). All common salts of the Na+, K+, and NH4+ cations are soluble in water. 3). Most common salts of the Cl-, Br-, and I- anions are soluble in water EXCEPT when the accompanying cation is Ag+, Pb2+, and Hg22+. 4). All common salts of the sulfate ion (SO42-) are soluble in water EXCEPT when the accompanying cation is Ba2+, Sr2+, and Pb2+. 5). Salts of the S2- ion are insoluble in water EXCEPT when the accompanying cation is Na+, K+, NH4+, Ba2+, and Ca2+. 6). Most of the transition metal cations (Ag+, Cu2+, Ni2+, etc.) form complexes with aqueous ammonia. Sometimes, ammonia is used to "dissolve" otherwise insoluble precipitates of these metal cations. ***The new AP Chemistry Guidelines suggest that you don’t really have to know most of these, just the common ones that are most useful.

9 Net Ionic Equations: Sol’n stoich. can be tricky when aqueous ionic compounds are involved … Predict the products and write the net ionic equation for the following precipitation reaction: Na2SO4 (aq) + BaCl2 (aq) 

10 Single Replacement Reactions:
A + BC --> BA + C (single anion replaces anion in compound) or A + BC --> AC + B (single cation replaces cation in compound)  *Free metal “A” needs t be above combined metal “B” Metal Activity Series

11 Net Ionic Equations: Sol’n stoich. can be tricky when aqueous ionic compounds are involved … Predict the products and write the net ionic equation for the following aqueous reaction: Zn (s) + HCl (aq) 

12 Net Ionic Equations: Practice by writing complete net ionic equations for each of the following: AgNO3(aq) + K2CO3(aq)  Al(s) + HCl (aq)  Ca (s) + H2O (l)  Ca(OH)2 + H2

13 2Ag+ (aq) + CO3-2 (aq)  Ag2CO3 (s)
Net Ionic Equations: Practice by writing complete net ionic equations for each of the following: 2Ag+ (aq) + CO3-2 (aq)  Ag2CO3 (s) AgNO3(aq) + K2CO3(aq)  Al(s) + HCl (aq)  Ca (s) + H2O (l)  Ca(OH)2 + H2

14 2Ag+ (aq) + CO3-2 (aq)  Ag2CO3 (s)
Net Ionic Equations: Practice by writing complete net ionic equations for each of the following: 2Ag+ (aq) + CO3-2 (aq)  Ag2CO3 (s) AgNO3(aq) + K2CO3(aq)  Al(s) + HCl (aq)  Ca (s) + H2O (l)  Ca(OH)2 + H2 2Al (s) H+ (aq)  2Al+3 (aq) H2 (g)

15 2Ag+ (aq) + CO3-2 (aq)  Ag2CO3 (s)
Net Ionic Equations: Practice by writing complete net ionic equations for each of the following: 2Ag+ (aq) + CO3-2 (aq)  Ag2CO3 (s) AgNO3(aq) + K2CO3(aq)  Al(s) + HCl (aq)  Ca (s) + H2O (l)  Ca(OH)2 + H2 2Al (s) H+ (aq)  2Al+3 (aq) H2 (g) Ca (s) H2O (l)  Ca(OH)2 (s) H2 (g)


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