We are being asked to find determine which situation where Kb for the conjugate base A– will have the largest Kb value.
HA(aq) ⇌ H3O+(aq) + A-(aq)
(weak acid) (conjugate base)
Hence, the Kb of A- can be calculated from the Ka of HA. Ka and Kb are connected by the autoionization constant of water (Kw) in the following equation:
Kw = 1.0x10-14 @ 25°C
Given a weak acid HA and the following equilibrium in water:
HA(aq) ⇌ H+(aq) + A–(aq)
which answer describes a situation where Kb for the conjugate base A– will have the largest Kb value?
A. Ka = 7.0 × 10–8 and T = 25 °C
B. Ka = 7.0 × 10–8 and T = 80 °C
C. Ka = 9.0 × 10–6 and T = 25 °C
D. Ka = 9.0 × 10–6 and T = 80 °C
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