Home
Class 12
CHEMISTRY
K(a) for HA is 4.9 xx 10^(-8). After mak...

`K_(a)` for `HA` is `4.9 xx 10^(-8)`. After making the necessary approximation, calculate for its decimolar solution,
a. `%` dissociation b. `overset(Θ)OH` concentration
c. `pH`

Text Solution

Verified by Experts

`{:(HA,hArr,H^(+),+,A^(-)),(C,,0,,0),(C(1-alpha),,alpha,,alpha):}`
`K_(a) = ([H^(+)][A^(-)])/([HA]) rArr K_(a) = (Calpha .Calpha)/(C(1-alpha)) = (Calpha^(2))/((1-alpha))approx Calpha^(2)`
(i) ` :. alpha = sqrt((K_(a))/C) = sqrt((4.9 xx10^(-8))/(1//10)) (C=1//10 M)`
` = 7 xx10^(-4) = 0.07 % `
(ii) `[H^(+)] = Calpha = 1/10 xx 7 xx10^(-4) = 7 xx10^(-5) ` mol/L
(iii) `[H^(+)] [OH^(-)] = 1xx10^(-14)`
` :. [OH^(-)] = (10^(-14))/(7xx10^(-5)) = 1.43 xx10^(-10) ` mol/L
Promotional Banner

Topper's Solved these Questions

  • IONIC EQUILIBRIUM

    FIITJEE|Exercise SOLVED PROBLEM (SUBJECTIVE)|15 Videos

  • IONIC EQUILIBRIUM

    FIITJEE|Exercise SOLVED PROBLEM (OBJECTIVE )|19 Videos

  • HYDROCARBONS

    FIITJEE|Exercise SINGLE INTEGER ANSWER TYPE QUESTION|9 Videos

  • LIQUID SOLUTION

    FIITJEE|Exercise Single Integer Answer Type Question|10 Videos

Similar Questions

Explore conceptually related problems

The dissociation constant of a weak acid HA si 4.9 xx 10^(-8) . After making the necessary approximations, calculate i. Percentage ionisation ii. pH iii. overset(Theta)OH concentration in a decimolar solution of the acid. Water has a pH of 7 .

The dissociation constant of weak acid HA is 4.9xx10^(-8) . After making the necessary approximations, calculate pH in 0.1 M acid.

K_(a) for an acid HA is 4.9 xx 10^(-8) . Calculate percentage dissocitation H^(+) ion concentration for its 0.1 M aqueous solution.

The dissociation constant of a weak acid HA is 4.9 xx 10^(-8) . Calculate for a decimolar solution of acid:. % of ionisation

The dissociation constant of a weak acid HA is 4.9 xx 10^(-8) . Calculate for a decimolar solution of acid:. OH^(-) concentration

Calculate the pH of a solution which has a hydronium-ion concentration of 6 xx 10^(-8) M

The ionisation constant of HF is 3.2 xx 10^(-4) . a. Calculate the dergee of dissociation of aall species present M solution. b. Calculate the concentration of all species present (H_(3)O^(o+),F^(Θ) and HF ) in the solution. c. Calculate method:

The dissociation constant of a weak monobasic acid in 0.01 M solution is 10^(-8) . What is its [OH^(-)] concentration?

Calculate the pH of 0.10 M solution of Nh_(4)Cl. The dissociation constant (K_(b)) of NH_(3) is 1.8xx10^(-5)