Any help? The Kb for hydroxylamine, HONH2, is 1.1 x 10 -8
. What would be the pH of a solution
prepared by placing 1.34 g of HONH2 in 0.500 L of water?

pH = 9.475

Explanation:

Hello there!

In this case, according to the basic ionization of the hydroxylamine:

The resulting equilibrium expression would be:

Thus, we first need to compute the initial concentration of this base by considering its molar mass (33.03 g/mol):

Now, we introduce as the reaction extent which provides the concentration of the hydroxyl ions to subsequently compute the pOH:

However, since Kb<<<<1, it is possible to solve for by easily neglecting it on the bottom to obtain:

Thus, the pOH is:

And the pH:

Regards!