Question

Which of the following K values represents the weakest base Kb= 1.26 × 10-6

© B. K5 = 7.41 × 10-5
O c. K5 = 1.8 × 10-5
O D. K5 = 3.8 × 10-10

Answer 1

K5​=3.8×10^−10 represents the weakest base among the given options. Hence the correct option is b.

The Kb values represent the equilibrium constants for the ionization of a base in water, with lower values indicating weaker bases. In this case, K5​ =3.8×10^−10 has the smallest numerical value among the options, signifying the weakest base.

This implies that the corresponding base has a lower tendency to accept protons in aqueous solution, making it less effective as a Brønsted-Lowry base compared to the other options. The magnitude of the equilibrium constant is indicative of the strength of the base, with smaller values corresponding to weaker bases in the context of acid-base chemistry. Hence the correct option is b.