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Chemistry
Chemistry
Problem
During the titration of a monoprotic weak acid with a strong base, what is the numerical relationship between the solution’s pH and the acid’s
K
a
K_a
K
a
at the half-equivalence volume? a)
pH
=
1
2
p
K
a
\text{pH} = \dfrac{1}{2}\,\text{p}K_a
pH
=
2
1
p
K
a
b)
pH
=
p
K
a
\text{pH} = \text{p}K_a
pH
=
p
K
a
c)
pH
=
14
−
p
K
a
\text{pH} = 14 - \text{p}K_a
pH
=
14
−
p
K
a
d)
pH
≈
p
K
a
−
0.30
\text{pH} \approx \text{p}K_a - 0.30
pH
≈
p
K
a
−
0.30
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