1 Chapter 12 Electrochemistry 12.1 Daniel / Galvanic Cell versus Electrolytic Cell • Zn is lower than Cu on the Electrochemical Series • Zn + Cu 2+ Zn 2+ + Cu E° = 0.76 + 0.34 = 1.1 V > 0 • Natural process • -ive terminal to Zn and +ive terminal to Cu • Zn 2+ + Cu Zn + Cu 2+ • E° = - 0.76 - 0.34 = - 1.1 V < 0 • Artificial process • If Zn 2+ solution is dilute, than trace H + from H 2 O becomes H 2 (cathodic reduction) • If Cu 2+ solution is dilute, than trace OH - from H 2 O becomes O 2 (anodic oxidation)
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1
Chapter 12
Electrochemistry
12.1 Daniel / Galvanic Cell versus Electrolytic Cell
• Zn is lower than Cu on the
Electrochemical Series
• Zn + Cu2+
� Zn2+
+ Cu
E° = 0.76 + 0.34 = 1.1 V > 0
• Natural process
• -ive terminal to Zn and +ive terminal to Cu
• Zn2+
+ Cu � Zn + Cu2+
• E° = - 0.76 - 0.34 = - 1.1 V < 0
• Artificial process
• If Zn2+
solution is dilute, than trace H+ from H2O becomes H2
(cathodic reduction)
• If Cu2+
solution is dilute, than trace OH- from H2O becomes O2
(anodic oxidation)
2
12.2 Charge Based Calculations
• Q = It = nF
12.3 Acid / Base Dissociation
• NaOH � Na+ + OH
- Kb = [Na
+][OH
-] / [NaOH]
pKb = -log ([Na+] / [NaOH]) + pOH
pOH = pKb + log ([Na+] / [NaOH])
Since pH + pOH = 14 = pKw (for water and all aqueous solutions),
14 - pH = pKb + log ([Na+] / [NaOH])
pH = 14 - pKb - log ([Na+] / [NaOH])
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• Strong acid / base calculation:
• Weak acid / base calculation:
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• Acid / base strength
- C2H5 etc also electron donating (increasing ion stability)
- C6H5 , halogens, OH etc are electron withdrawing (decreasing ion stability)
(in this case, more electron drawing power decreases ion stability and
therefore decreases base strength)
**So how about for ethanoic acid dissociation in water?
Where R is CH3
(in this case, more electron drawing power INcreases ion
stability and therefore INcreases base strength)
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12.4 Titration Indicators are Weak Acids / Bases
• Most indicators change colour across a pH range of 2 or concentration
range of 102
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12.5 Titration Curves
• Equivalence point shift
pH = 14 - pKb - log ([Na+] / [NaOH])
(Curve can actually be plotted)
• Titrating sodium carbonate (use which indicator?)
HCl + Na2CO3 � NaCl + NaHCO3
HCl + NaHCO3 � NaCl + H2O + CO2
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• Titrating phosphoric acid H3PO4 (again, use which indicator?)
12.6 Buffer Solutions
• Weak acid or weak base buffer solutions (must have salt present)
•
pH = 14 - pKb - log ([Na+] / [NH4OH])
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• If asked to calculate pH change when more acid or base is added, just
plug in new [acid] or [base] into the equation for calculation. This is to
determine buffer capacity i.e. how much more acid or base to upset the
buffered pH.
pH = 14 - pKb - log ([Na+] / [NH4OH])
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• Biological importance
• If asked to calculate pH change when more acid or base is added, just
plug in new [acid] or [base] into the equation for calculation. This is to
determine buffer capacity i.e. how much more acid or base to upset the