Asked by Chris

When 23.3 mL of 0.14 M HCl are added to 50.0 mL of a 0.16 M solution of a weak monoprotic base, the pH of the solution is 10.50. What is the Kb of the weak base?


do u find moles of both and then add the moles for HB+ and then just use the B- moles for the B on the henderson hasselbach equation

and then solve for Ka and then solve for Kb?

i don't get the right answer
please help
Answered by DrBob222
Find moles of both, SUBTRACT mols acid from moles base (because base is larger), then plug into the HH equation to calculate pKa, change to pKb, then to Kb.
Answered by Kody
What do you plug into the HH equation?
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