Problem: The pH of a 0.10 M solution of a weak base is 9.82. What is the Kb for this base?

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We are being asked to calculate the Kb for a 0.1 M weak base (HB).


Step 1. Equilibrium reaction:        HB(aq) + H2O(l)   BH2+(aq) + OH-(aq)


Kb=productsreactants=[BH2][OH-][HB]

Kb=xx0.1-xKb=x20.1-x

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The pH of a 0.10 M solution of a weak base is 9.82. What is the Kb for this base?