Chemistry - Ionic Equilibrium Question with Solution | TestHub

ChemistryIonic EquilibriumMiscellaneous/MixedEasy2 minPYQ_2020

ChemistryEasynumerical

The average concentration of SO₂in the atmosphere over a city on a certain day is 10 ppm, when the average temperature is 298 K. Given that average solubility of SO₂at 298 K is 1.3653 M atm^-1and pK_aof H₂SO₃is 1.92, estimate the pH of rain on that day.

Answer:

4.86

Solution:

Partial pressure of SO₂in air = 10^{- 5}atm

[SO₂] = 1.3653 x 10^{- 5}M

[H₂SO₃] = 1.3653 x 10^{- 5}M

$H_{2} {SO}_{3} ⇌ H^{+} + {HSO}_{3}^{-}$

H₂SO₃at low concentration is fully ionised.

[H⁺] = 1.3653 x 10^{- 5}

pH = - log 1.3653 x 10^{- 5}

= 5 - log 1.36

= 4.86

Stream:NTA_ABHYASSubject:ChemistryTopic:Ionic EquilibriumSubtopic:Miscellaneous/Mixed

⏱ 2mℹ️ Source: PYQ_2020

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