Chemistry - Ionic Equilibrium Question with Solution | TestHub

ChemistryIonic EquilibriumTitration Based ProblemsMedium2 minQB

ChemistryMediumnumerical

Passage / Comprehension

Following is the titration curve of two weak monoprotic acids HA and HB (5 milli-moles each) in 50 ml aqueous solution titrated against aqueous solution of strong base NaOH (0.1 M) in two different experiments :

[Given : log 2 = 0.3]

pH at equivalence point if HA is titrated by NaOH in the experiment given above :

Answer:

9.35

Solution:

$pH = pKa + lo g \frac{[ A ^{-} ]}{[ HA ]}$

$6 = pKa$

$C = \frac{0.1}{2}$

At the equivalence point:

$[H^{+}] = \frac{K _{w} \cdot K _{a}}{C}$

$[H^{+}] = \frac{1 0 ^{- 14} \times 1 0 ^{- 6}}{\frac{0.1}{2}}$

$[H^{+}] = 2 \times 1 0^{- 19}$

$pH = \frac{1}{2} (19 - lo g 2)$

$pH = \frac{1}{2} (18.7)$

$pH = 9.35$

Stream:JEESubject:ChemistryTopic:Ionic EquilibriumSubtopic:Titration Based Problems

⏱ 2mℹ️ Source: QB

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