calculate degree of dissociation of 0.02M acetic acid at 298K.
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Definition :
Degree of dissociation — The fraction of total number of molecules of electrolytes dissolved that ionizers at equilibrium.
It is given by:
α = √(Ka / C)
Where α = the degree of dissociation
Ka — The ionization constant of acetic acid.
C — The molarity of acetic acid.
CALCULATIONS
Ka = 1.8 × 10⁻⁵ M
C = 0.02 M
Substituting in the formula we have :
α = √{(1.8 × 10⁻⁵) / 0.02}
α = √9⁻⁴
α = 0.03
Answer :
0.03
Degree of dissociation — The fraction of total number of molecules of electrolytes dissolved that ionizers at equilibrium.
It is given by:
α = √(Ka / C)
Where α = the degree of dissociation
Ka — The ionization constant of acetic acid.
C — The molarity of acetic acid.
CALCULATIONS
Ka = 1.8 × 10⁻⁵ M
C = 0.02 M
Substituting in the formula we have :
α = √{(1.8 × 10⁻⁵) / 0.02}
α = √9⁻⁴
α = 0.03
Answer :
0.03
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