The first and second dissociation constants of an acid H 2 A a r e 1.0 × 10 - 5 a n d 5.0 × 10 - 10 respectively. The overall dissociation constant of the acid will be

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Chemistry - Ionic Equilibrium Question with Solution | TestHub

ChemistryIonic EquilibriumpH of Strong and Weak Acids and BasesEasy2 minPYQ_2020

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The first and second dissociation constants of an acid $H_{2} A a r e 1.0 \times 10^{- 5} a n d 5.0 \times 10^{- 10}$ respectively. The overall dissociation constant of the acid will be

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Solution:

Given $K_{1} = 1.0 \times 10^{- 5}$ , $K_{2} = 1.0 \times 10^{- 5}$

so overall dissociation constant of the acid will be $K = K_{1} \times K_{2}$

$= 1.8 \times 10^{- 5} \times 5.0 \times 10^{- 10}$

$= 10 \times 10^{- 15}$

Stream:NTA_ABHYAS_NEETSubject:ChemistryTopic:Ionic EquilibriumSubtopic:pH of Strong and Weak Acids and Bases

⏱ 2mℹ️ Source: PYQ_2020

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