Data for CH3COOH(l) + C2H5OH(l) CH3COOC2H5(l) + H2O(l) balance were obtained at 100. The initial concentrations of the reagents
are indicated in columns 1 and 2 of the table below and the CH3COOC2H5 concentrations in equilibrium are given in column 3. Calculate H2O and determine the value of KC
1 answer:
Answer:
Kc = 3.94
Explanation:
CH₃COOH(g) + C₂H₅OH(g) → CH₃COOC₂H₅(g) + H₂O(g)
Liquids aren't included in the equilibrium constant, but at 100°C, all four compounds are a gas. So the equilibrium equation is:
Kc = [CH₃COOC₂H₅] [H₂O] / ([CH₃COOH] [C₂H₅OH])
Set up an ICE table for each row and calculate the value of Kc. Then average the results. (See picture.)
Kc ≈ (3.919 + 4.012 + 3.902) / 3
Kc ≈ 3.94
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Answer:
The pH is equal to 4.41
Explanation:
Since HClO is a weak acid, its dissociation in aqueous medium is:
HClO ⇄ ClO- + H+
start: 0.05 0 0
change -x +x +x
balance 0.05-x x x
As it is a weak acid it dissociates very little, in its ClO- and H + ions, so the change is negative, where x is a degree of dissociation.
the acidity constant when equilibrium is reached is equal to:
The 0.05-x fraction can be approximated to 0.05, because the ionized fraction (x) is very small, therefore we have:
clearing the x and calculating its value we have:
the pH can be calculated by: