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 0.01M acid solution is :
If degree of dissociation is 0.01 of decimolar solution of weak acid HA then pK_(a) of acid is :
What is the ionization constant of an acid if the hydronium ion concentration of a 0.40 M solution is 1.40xx10^(-4) M?
A_(AgCl)^(oo) can be obtained:
At 25^(@) C dissociation constants of acid HA and base BOH in aqueous solution are same. The pH of 0.01 M solution of HA is 5. The pOH of 10^(-4) M solution of BOH at the same temperature is :
Units of rate constant for the first and zero order reactions in terms of molarity, M units are respectively
The enthalpy of neutralization of a Weak monoprotic acid (HA) in 1 M solution with a strong base is -55.95 KJ/mol . If the unionized acid required 1.4 KJ/mol heat for it's comptate ionzatation and enthalpy of netralization of the strong monobasic acid with a strong monoacidic base is -57.3 KJ/mol . What is the % ionzation of the weak acid in molar solution ?
The acid dissociation constant of uric acid is K_(a)=4.0xx10^(-6) M. The pH of a sample of urine is 6.0. What is the ratio of concentration of urate ion to uric acid in the urine?
The percentage degree of hydrolysis of a salt of weak acid (HA) and weak base (BOH) in its 0.1 M solution is found to be 10%. If the molarity of the solution is 0.05 M, the percentage hydrolysis of the salt should be :
The molar conductivity of a solution of a weak acid HX(0.01M) is 10 times smaller than the molar conductivity of a solution of a weak acid HY(0.10M). If lambda_(X)^@ = lambda_(Y)^@ , the difference in their pK_a values, pK_a(HX)-pK_a(HY)
