Calculate the value of kb for this base

Thread starter nysoprano
Start date Dec 20, 2004
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Base Value

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SUMMARY

The discussion focuses on calculating the base dissociation constant (Kb) for a 0.200 M solution of a weak base with a pH of 10.40. To determine Kb, one must use the equilibrium expression for weak bases, considering that they do not fully dissociate in hydroxide ions. The equilibrium concentration of hydroxide ions can be derived from the pH value, which is essential for solving the Kb equation.

PREREQUISITES

Understanding of weak base dissociation and equilibrium concepts
Knowledge of pH and pOH calculations
Familiarity with the Kb expression for weak bases
Basic algebra for solving equilibrium equations

NEXT STEPS

Learn how to calculate pOH from pH values
Study the equilibrium constant expressions for weak bases
Explore examples of Kb calculations for various weak bases
Review the concept of hydrolysis in weak base solutions

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Chemistry students, educators, and anyone involved in analytical chemistry or studying acid-base equilibria will benefit from this discussion.

Dec 20, 2004

nysoprano

pH help??

This is the question i need help in:
A 0.200 M solution of a weak base in water has a pH=10.40. Calculate the value of kb for this base.

I know the answer but i need help on how to get that answer. Thanks

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Dec 20, 2004

Pyrrhus

Homework Helper

If its a weak base then it doesn't diassociates completely in OH ions, so you need to use the equilibrium solution.

Dec 21, 2004

Sirus

This may help: see post #5 here.

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