Asked by Anonymous
A buffer contains the weak acid HA abd its conjugated base A-. The weak acid has a Ka of 1.51 x10^-5 and the buffer has a pH of 4.25. Which statement is true about the relative concentrations of HA and A- in the buffer?
A) [HA]>[A-]
B) [HA]<[A-]
C) [HA] = [A-]
A) [HA]>[A-]
B) [HA]<[A-]
C) [HA] = [A-]
Answers
Answered by
DrBob222
pH = pKa + log base/acid
pH = 4.26
pKa = 4.82
So log A/HA must be negative. Which (A or B) will make it negative?
pH = 4.26
pKa = 4.82
So log A/HA must be negative. Which (A or B) will make it negative?
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