Monoacidic weak base MOH has the dissociation constant as 1.8 × 1 0 − 5 . What would be the concentration of OH − ion in its 0.1 M solution

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Monoacidic weak base MOH has the dissociation constant as $1.8 \times 1 0^{- 5}$ . What would be the concentration of $OH^{-}$ ion in its 0.1 M solution

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Solution:

For a Monoacidic weak base MOH , the relationship between the hydroxide concentration the base, the base concentration C and dissociation constant is

$[OH^{-}] = K_{b} \times C$

$= 1.8 \times 1 0^{- 5} \times 0.1$

$= 1.34 \times 1 0^{- 3} M$

Stream:JEESubject:ChemistryTopic:Thermodynamics - ISubtopic:Miscellaneous/Mixed

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