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A classic experiment in equilibrium studies dating from 1862 involved the reaction in aqueous solution of...

A classic experiment in equilibrium studies dating from 1862 involved the reaction in aqueous solution of ethanol and acetic acid to produce ethyl acetate and water.

C₂H₅OH (aq) + CH₃COOH (aq) <---> CH₃COOC₂H₅ (aq) + H₂O (l)

The reaction can be followed by analyzing the equilibrium mixture for its acetic acid content using a titration with Ba(OH)₂ as shown below:

2CH₃COOH (aq) + Ba(OH)₂ (aq) ---> Ba(CH₃COO)₂ (aq) + 2H₂O (l)

In one experiment, a mixture of 1.000 moles acetic acid and 0.5000 moles ethanol is brought to equilibrium in a 1.000 L flask. A 20.00 mL sample of the equilibrium mixture requires 56.74 mL of 0.1000 M Ba(OH)₂ for its titration.

What is the concentration of the acetic acid found in the titration?

What is the mass action expression for the reaction of ethanol and acetic acid?

What is the value of the equilibrium constant for the reaction of ethanol and acetic acid?

Expert Solution

2CH3COOH (aq) + Ba(OH)2 (aq) ---> Ba(CH3COO)2 (aq) + 2H2O (l)

$nBa(OH)_{2}=0.1 M � 56.74 x10^{-3} L$

i) 0.5 1 0

eq) 0..5-X 1-X X

queen_honey_blossom answered 2 years ago

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