aqueous reactions pb(no 3 ) 2 (s) + h 2 o (l) leadnitrate(ii) ki (s) potassiumiodide + h 2 o (l) ...
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![Page 1: Aqueous Reactions Pb(NO 3 ) 2 (s) + H 2 O (l) leadnitrate(II) KI (s) potassiumiodide + H 2 O (l) Pb 2+ (aq) + 2 NO 3 - (aq)+ K + (aq) + I - (aq)](https://reader035.vdocument.in/reader035/viewer/2022072014/56649e7c5503460f94b7df5a/html5/thumbnails/1.jpg)
Aqueous Reactions
Pb(NO3)2 (s) + H2O (l) lead nitrate(II)
KI (s)potassium iodide
+ H2O (l)
Pb2+ (aq) + 2 NO3- (aq) + K+ (aq) + I- (aq)
yellow solid + solution
PbI2 KNO3
Pb2+ (aq) + NO3- (aq)2
K+ (aq) + I- (aq)
displacement reactionsolubility of salts
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Solubility rules1. Most NO3
- salts are soluble
2. Most salts of alkali metals (IA) and NH4+ are soluble
3. Most Cl-, Br- and I- salts are solubleExceptions: Ag+, Pb2+ and Hg2
2+ insoluble4. Most SO4
2- are soluble
Exceptions: Ca2+, Ba2+, Pb2+, Hg22+ insoluble
5. Most OH- are insolubleExceptions: IA, Ca2+, Ba2+, Sr2+ soluble
6. Most S2-, CO32-, CrO4
2-, PO43- insoluble
Exceptions: IA, NH4+ soluble
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Pb2+ (aq) + 2 NO3- (aq) + K+ (aq) + I- (aq)
yellow solid + solution
PbI2 KNO3
2. Most IA salts are soluble
PbI2 (s) + K+ (aq) + NO3- (aq)
balance the equation
start with molecular equation
3. Most Cl-, Br- and I- salts are solubleExceptions: Ag+, Pb2+ and Hg2
2+ insoluble
1. Most NO3- salts are soluble
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Pb(NO3)2 (aq) + KI (aq)
balance molecular equation
PbI2 (s) + KNO3 (aq)22
change to ionic equation
1. Most NO32- salts are soluble
Pb2+(aq)+2NO3-(aq)
2. Most Group I salts are soluble
3. Most Cl-, Br- and I- salts are soluble
except Ag+, Pb2+ and Hg22+
+2K+(aq) +2I-(aq) PbI2 (s) +2K+(aq) +2NO3- (aq)
spectator ions they can be cancelled out innet ionic equation
Pb2+(aq) + 2 I- (aq) PbI2 (s)
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Acid/Base reactionsHCl strongdissociates completely
NaOH dissociates completely strong
H+(aq) Cl- (aq)
Na+(aq) OH-(aq)
H+(aq)
H2O (l)
+Cl-(aq)+ Na+(aq)+ OH-(aq)
acid
base
+ Na+(aq) + Cl-(aq)
HCl(aq)
molecular eqn
+ NaOH(aq) H2O(l) + NaCl(aq)
ionic eqn H+ +Cl-+ Na++ OH- H2O + Na++ Cl-
net ionic eqn H+ + OH- H2O
![Page 6: Aqueous Reactions Pb(NO 3 ) 2 (s) + H 2 O (l) leadnitrate(II) KI (s) potassiumiodide + H 2 O (l) Pb 2+ (aq) + 2 NO 3 - (aq)+ K + (aq) + I - (aq)](https://reader035.vdocument.in/reader035/viewer/2022072014/56649e7c5503460f94b7df5a/html5/thumbnails/6.jpg)
Acid/Base reactionsHCl strongdissociates completely
H+(aq) Cl- (aq)
acid
Mg(OH)2 does not dissociate completely
Mg(OH)2(aq)
weak base
H++ Cl-
Mg2+(aq) + 2OH-(aq)
+ Mg(OH)2 + Mg2++ 2OH-
H2O + MgCl2molecular eqn
ionic eqn
net ionic eqn
Mg(OH)2 + HCl
H2O + Mg2+ + Cl-
22
Mg(OH)2+ 2H++ 2Cl-2 H2O + Mg2+ +2Cl-
Mg(OH)2(s) +2 H+(aq) 2 H2O(l) + Mg2+(aq)
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Acid/Base reactions
neutralization reactions products are not acidsbases
H+
OH-
equivalence point [H+] = [OH-]
mol H+
L= mol OH-
L
What volume of 0.100 M HCl is needed to neutralize 25.00 mL of 0.350 M NaOH
0.350 mol NaOHL
25.00 x 10-3 L = 8.75 x 10-3 mol NaOH
8.75 x 10-3 mol HCl0.100 mol HCl
L = 0.0875 L= 87.5 mL HCl
H2O
(x) (x)
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A 2.2 g sample of an unknown acid, HA, is dissolved in 1.0 L of water.A titration required 25.0 mL of 0.500 M NaOH to react completely. What is the molecular weight of the unknown?
g HA 2.2 g HA
mol H+= mol OH-
0.500 mol NaOH
= 0.0125 mol OH-
0.0125 mol H+ =
2.2 g0.0125 mol
= 176 g/molmol HA
mol HA = mol H+
0.025 LL
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