The titration of a weak acid with a strong base is a common exercise in chemistr

Question

The titration of a weak acid with a strong base is a common exercise in chemistry labs. We have looked at all of the individual types of calculations needed to determine the pH at any point of a titration.

Consider the titration of 0.100 L of 0.300 M acetic acid with 1.50 NaOH.

What type of calculation will we be performing at the following points of the titration curve?

Answers can be used more than once:  -weak acid calculation -buffer calculation -conjugate base calculation -strong base calculation

1. Zero equivalents of base added
2. 0.15 equivalents of base added
3. One equivalent of base added
4. 1.75 equivalents of base added

Explanation / Answer

CH3COOH + NaOH ----> CH3COONa + H2O

1 mole CH3COOH = 1 mole NaOH

or 1 equivalent CH3COOH = 1 equivalent NaOH

1. Zero equivalents of base added    = weak acid calculation

Because before addition of base.only pure CH3COOH present.so that to determine pH. weak acid equation is used.

pH = 1/2(pka+log c)

2. 0.15 equivalents of base added   = buffer calculation

after adding base ,the solution behaves like a buffer solution up to half equivalence point.

3. One equivalent of base added = conjugate base calculation

at equivalence point solution behaves like a salt of weakacid,strongbase.

4. 1.75 equivalents of base added = strong base calculation

after equivalence point the no of equivalents of base is more.so that it behaves like strong base.

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