HA is a weak acid . No. of moles = 0.001, `K_a` = 2x`10^(-6)`, HCl is added with molarity 0.01 and the solution is made 1 litre. calculate degree of dissociation of HA

HA is a weak acid. The pH of 0.1 M HA solution is 2. What is the degree of dissociation (alpha) of HA ?

The pH of a 0.1 M aqueous solution of a weak acid (HA) is 3. What is its degree of dissociation ?

A monoprotic acid in 0.1 M solution has K_(a)=1.0xx10^(-5) . The degree of dissociation for acid is

0.01 moles of a weak acid HA ( K_(a) = 2.0 xx 10^(-6) ) is dissolved in 1.0 L of 0.1 M HCl solution. The degree of dissociation of HA is "____________" xx 10^(-5) ( Round off to the Nearest Integer). [ Neglect volume change on adding HA. Assume degree of dissocaition lt lt 1 ]

1 cm^(3) of 0.01 N HCl solution is added to one litre of sodium chloride solution . Calculate the pH of the resulting solution.