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March 30, 2017

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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

  • Chemistry - ,

    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.

  • Chemistry - ,

    What do you plug into the HH equation?

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