Given the table of Ka values on the right below, arrange the conjugate bases in order from strongest to weakest.

Acid Ka
HClO 3.5 e-8
HClO2 1.2 e-2
HCN 6.2 e-10
H2PO4- 6.2 e-8
A. ClO2-, ClO¬-, HPO42-, CN-
B. ClO2-, HPO42-, ClO¬-, CN-
C. CN-, HPO42-, ClO-, ClO2¬-
D. CN-, ClO-, HPO42-, ClO2-

Kb = (Kw/Ka)

Calculate Kb for each acid, then arrange in order.

To determine the relative strength of conjugate bases, we need to remember that the stronger the acid, the weaker its conjugate base.

The first step is to identify the acids from the given Ka values. The acids are HClO, HClO2, HCN, and H2PO4-.

Next, we need to determine the conjugate bases of these acids. The conjugate base of an acid is formed when the acid loses a proton (H+). Therefore, the conjugate bases are ClO-, ClO2-, CN-, and HPO42-.

Now, we need to compare the Ka values to determine the relative strength of the acids. The higher the Ka value, the stronger the acid.

Given the Ka values:
- HClO has a Ka of 3.5 e-8
- HClO2 has a Ka of 1.2 e-2
- HCN has a Ka of 6.2 e-10
- H2PO4- has a Ka of 6.2 e-8

From these values, we can see that HClO2 is the strongest acid because it has the highest Ka value.

Now, we can arrange the conjugate bases in order from strongest to weakest based on the strength of their corresponding acids.

Therefore, the correct answer is:
B. ClO2-, HPO42-, ClO-, CN-