Question

pH of a 0.1M monobasic acid is found to be 2.Hence its osmotic pressure at a given temp T is

Answer 1

According to Arrhenius principle,
pH = - log[H⁺]
2 = -log[H⁺] ⇒[H⁺] = 10⁻² = 0.01

Assume HX is monobasic acid.
HX ⇄ H⁺ + X⁻
so, for dilute solution,
[H⁺ ] = Cα, here C is concentration of acid and α is dissociation Constant
Now, 0.01 = 0.1 × α [ ∵ concentration = 0.1M is given ]
α = 0.1

Now, A/C to van Hoff's principle,
i = 1 + α
i = 1 + 0.1 = 1.1
use Osmotic pressure, π = iCRT
= 1.1 × 0.1RT
= 0.11RT

Hence, answer is 0.11RT