Acid/Base Chemistry Part II
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Transcript of Acid/Base Chemistry Part II
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Acid/Base Chemistry Part II
CHEM 2124 – General Chemistry II
Alfred State College
Professor Bensley
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Learning Objectives
• Write the chemical equation for a weak acid undergoing acid ionization in aqueous solution.
• Define acid dissociation constant.• Determine Ka from a solution pH.• Calculate concentrations of species in
a weak acid solution using Ka.• Write the hydrolysis reaction of an ion
to form an acidic solution.
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Learning Objectives
• Recognize common acid-base reactions.
• Predict whether a salt solution is acidic, basic, or neutral.
• Calculate concentrations of acid or base solutions through titrations.
• Define buffer.
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Learning Objectives
• Describe the pH change of a buffer solution with the addition of an acid or a base.
• Calculate the pH of a buffer from given volumes of solution.
• Calculate the pH of a buffer when a strong acid or a strong base is added.
• Learn and apply the Henderson-Hasselbalch equation.
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Acid/Base Chemistry – Part II
A. Equilibrium and Acid Dissociation Constants
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B. The relationship between [H3O+], pH, and Ka
[H3O+] = √KaC0
pH = ½ pKa – ½ log C0
Acid/Base Chemistry – Part II
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Acid/Base Chemistry – Part II
1. Neutralization reaction
C. Common Acid/Base Reactions
2. Net Ionic Reaction of Neutralization reactions:
3. Bicarbonate Base reactions
D. The Acidity and Basicity of Salt Solutions
NaCl
Na+
from NaOHstrong base
Cl−
from HClstrong acid
NaHCO3
Na+
from NaOHstrong base
HCO3−
from H2CO3
weak acid
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NH4Cl
NH4+
from NH3
weak base
Cl−
from HClstrong acid
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E. Buffers
A buffer is a solution whose pH changes very littlewhen acid or base is added.
Acid/Base Chemistry – Part II
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Acid/Base Chemistry – Part II
F. Calculating the pH of a Buffer
Henderson-Hasselbalch Equation
pH = pKa + log ([A-]/[HA])
pH = pKa + log Cs – log Ca
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