What is the degree of dissociation of weak acid HA having concentration =0.1 M in the presence of strong acid HB having concentration =0.1 M. Given Ka for weak acid =10-6

Question

What is the degree of dissociation of weak acid HA having concentration =0.1 M in the presence of strong acid HB having concentration =0.1 M. Given Ka for weak acid =10-6 (A) 10-5 (B) 10-6 (C) 10-4 (D) 10-3

Tardigrade Admin · Accepted Answer

For weak acid,

K a =(( H +)( A -)/( HA ))

( H +) in the solution =0.1 M (∵ of strong acid ) K, will remain constant ∴ 10-6=((0.1)( C α)/( C - C α)) 10-6=(0.1 C α/ C (1-α)) 10-6=(0.1 × α/1-α) 1-α ≈ 1 10-6=0.1 × α 10-6=10-1 × α α=10-5

Q. What is the degree of dissociation of weak acid $H A$ having concentration $= 0.1 M$ in the presence of strong acid HB having concentration $= 0.1 M$ . Given $K_{a}$ for weak acid $= 1 0^{- 6}$

$1 0^{- 5}$

$1 0^{- 6}$

$1 0^{- 4}$

$1 0^{- 3}$

Q. What is the degree of dissociation of weak acid HA having concentration =0.1M in the presence of strong acid HB having concentration =0.1M. Given Ka​ for weak acid =10−6

10−5

10−6

10−4

10−3

For weak acid, Ka​=(HA)(H+)(A−)​ (H+) in the solution =0.1M(∵ of strong acid ) K, will remain constant ∴10−6=(C−Cα)(0.1)(Cα)​ 10−6=C(1−α)0.1Cα​ 10−6=1−α0.1×α​ 1−α≈1 10−6=0.1×α 10−6=10−1×α α=10−5

Q. What is the degree of dissociation of weak acid $H A$ having concentration $= 0.1 M$ in the presence of strong acid HB having concentration $= 0.1 M$ . Given $K_{a}$ for weak acid $= 1 0^{- 6}$

$1 0^{- 5}$

$1 0^{- 6}$

$1 0^{- 4}$

$1 0^{- 3}$