Chemistry - Ionic Equilibrium Question with Solution | TestHub

ChemistryIonic EquilibriumBuffer solutionMedium2 minQB

ChemistryMediumsingle choice

How many moles of HCl must be added to 1.0 L of $0.1 M NH_{3}$ to prepare a solution of $pH = 9$ . (Given that $K_{b} (NH_{3}) = 1.8 \times 1 0^{- 5})$

Options:

Answer:

Solution:

$n (H Cl)_{a dd e d} = n (N H_{4} Cl)_{f or m e d}$

Therefore, $[O H^{-}] = K_{b} \frac{[ N H _{3} ]}{[ N H _{4} Cl ]}$ (Basic Buffer)

$1 0^{- 5} = 1.8 \times 1 0^{- 5} [\frac{0.1 - x}{x}]$

$x = 0.643$ .

Stream:JEESubject:ChemistryTopic:Ionic EquilibriumSubtopic:Buffer solution

⏱ 2mℹ️ Source: QB

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