How does the degree of ionization (assuming lt lt 1)` of a weak electroyte vary with concentration ? Give exact relationship.

If alpha is the degree of ionization, C the concentration of a weak electrolyte and K_(a) the acid ionization constant , then the correct relationship between alpha and C is

How does the value of rate constant vary with reactant concentration ?

How does the value of rate constant vary with reactant concentration ?

How does the value of rate constant vary with reactant concentration ?

How does the value of rate constant vary with reactant concentrations?

1.0 M solution of a weak base , BOH is only 0.5 % ionized . If 2 mL 1 M solution of BOH is mixed with 30 mL water , the degree of dissociation of the base in the resulting solution and H^(+) ion concentration of the solution will bee respectively

The ionization constant of acetic acid 1.74xx10^(-5) . Calculate the degree of dissociation of acetic acid in its 0.05 M solution. Calculate the concentration of acetate ion in the solution and its pH .

The degree of dissociation of a weak monoprotic acid of concentration 1.2xx10^(-3)"M having "K_(a)=1.0xx10^(-4 is

Statement-1: On increasing dilution, the specific conductance keeps on increasing. Statement-2: On increasing dilution. Degree of ionization of weak electrolyte ncreases and mobility of ions also increases.

In a 0.2 molal aqueous solution of a weak acid HX the degree of ionization is 0.3 . Taking k_(f) for water as 1.85 the freezing point of the solution will be nearest to-