Calculating Kb: Ph 0.3mol/l Weak Base, 10.66

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SUMMARY

The discussion focuses on calculating the base dissociation constant (Kb) for a 0.3 mol/L solution of a weak base with a pH of 10.66. Participants emphasize the importance of converting pH to pOH and subsequently determining the concentration of hydroxide ions (OH-) to find Kb. The methodology mirrors that of weak acid calculations but requires adjustments for basicity, specifically using Kb instead of Ka. Key contributors, Borek and others, provide guidance on modeling the calculations effectively.

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  • Familiarity with Kb and Ka concepts
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The Ph of 0.3mol/l of a weak base is 10.66, calculate kb.

I was thinking of using ph and calculate the concentration of H ions and then calculate poh and OH, but don't know what to do next. Any ideas?
 
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This is much like a solution of a weak acid, but now the opposite. Model the work like some of the others in this board and you'll get the answer.

OH- instead of H+;
pOH instead of pH and convert back when ready.
Kb instead of Ka.

Look at some of the guidance which Borek and I have given and make appropriate changes.
 

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