A weak acid HA of concentration 0.001 mile/litre have conductance 2x`10^(-5)Scm^(-1)` and molar conductivity at infinite dilution is 190 `Scm^2"mole"^(-1)` then value of `K_a` of weak acids id [X] x `10^(-6)`, then value of x in nearest integer is:

The dissociation constant of a weak acid is 1.6xx10^(-5) and the molar conductivity at infinite dilution is 380xx10^(-4) S m^2mol^(-1) . If the cell constant is 0.01 m^(-1) then conductace of 0.1M acid solution is :

The conductivity of a weak acid HA of concentration 0.001 mol L^(-1) is 2.0 xx 10^(-5)S cm^(-1) . If Lambda_(m)^(0)(H A) = 190 S cm^(2) mol^(-1) , the ionization constant (K_(a)) of HA is equal to ________ xx 10^(-6) . (Round off to the Nearest Integer)

Molar conductivity of a weak acid HA at infinite dilution is 345.8 cm^(2) mol^(-) calculate molar conductivity of 0.05 M HA solution

The molar conductivity of 0.05 M solution of weak acid is 16.6Omega^(-1)cm^(-2)mol^(-1). Its molar conductivity at infinite dilution is 390.7Omega^(-1)cm^(-2)mol^(-1) . The degree of dissociation of weak acid is

The dissociation constant of n-butyric acid is 1.6 xx 10^(-5) and the molar conductivity at infinite dilution is 380 xx 10^(-4) Sm^(2) mol^(-1) . The specific conductance of the 0.01M acid solution is

Molar conductance of 0.1 M acetic acid is 7 ohm^(-1) cm^(2) "mol"^(-1) . If the molar conductance of acetic acid at infinite dilution is 280 ohm^(-1) cm^(2) "mol"^(-1) , the value of dissoication constant will be:

The molecular conductivity of acetic acid at infinite dilution is 390 S cm^(2) "mole"^(-1) and for 0.1 acetic and solution is 5.8 cm^(3) "mole"^(-1) .The hydrogen ion concentration of the solution is