Chemistry - Ionic Equilibrium Question with Solution | TestHub

ChemistryIonic EquilibriumBuffer solutionEasy2 minQB

ChemistryEasysingle choice

Calculate the pH of a solution containing $0.2 M HCO_{3}^{-}$ and $0.1 MCO_{3}^{2 -}$ $[K_{1} (H_{2} CO_{3}) = 4 \times 1 0^{- 7}; K_{2} (HCO_{3}^{-}) = 4 \times 1 0^{- 11}]$

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Answer:

Solution:

$pH = pK_{a_{2}} + lo g \frac{[ CO _{3}^{2 -} ]}{[ HCO _{3}^{-} ]} \Rightarrow (11 - lo g 4) + lo g (\frac{1}{2}) \Rightarrow 10.1]$

Stream:JEESubject:ChemistryTopic:Ionic EquilibriumSubtopic:Buffer solution

⏱ 2mℹ️ Source: QB

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