The document discusses buffers and their properties. It defines a weak acid as having less ability to produce hydrogen ions (H+), and a weak base as having less ability to accept H+. It explains that buffers resist changes in pH when small amounts of acid or base are added. Common examples of buffers include a solution of acetic acid and sodium acetate, which can accept or donate H+ to resist pH changes. Buffers have important applications in biological systems like blood and microbial cultures.

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3.  Weak Acid: An acid having less
power to produce H +
 Salt : The neutralization product of
acid and base
Weak Base: A base having less power
to Accept H +
Buffer: Hindrance/ Resistance
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4.  The salt of a weak acid (CH3COOH )is
a strong electrolyte (CH3COONa )
 The salt of a weak base (NH4OH)is a
strong electrolyte (NH4OH)
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5.  The solutions that resists change in its pH
when small quantity of acid or base is added
to it.
 They have a constant specific value of pH that
don’t change with time.
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6.  Acidic Buffers(pH less than 7)
 Basic Buffer(pH More than 7)
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7.  Acidic Buffers consist of a weak acid and its
salt with a strog base eg,
 CH3COOH (Acetic acid/ aweak acid)
 CH3COONa ( Sodium Acetate/salt of Acetic
acid)
 They are mixed
 CH3COOH ⇌H++ CH3COO−
 CH3COONa ⇌ Na++ CH3COO−
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8.  When acid H+ is added
 CH3COOH ⇌H++ CH3COO−
 CH3COONa ⇌ Na++ CH3COO−
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9.  When acid 0H- is added
 H2O
 CH3COOH ⇌ H+ + CH3COO−
CH3COONa ⇌ Na++ CH3COO−
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10.  Blood pH 7.35-8.35
 In chemical Industries
 To Grow Bacterial Cultures
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