Determine the hydrogen ion concentration in `1.0 ` M solution of HCN , if its dissociation constant is `4.0 xx 10^(-10)`.

Calculate the H^+ ion concentration of a 0.01N weak monobasic acid. The value of dissociation constant is 4.0 xx 10^(-10) .

Calculate the H^(+) ion concentration of 0.01 weak monobase acid . The value of dissociation contant is 4.0 xx 10^(-10)

Calculate the H^(+) ion concentration of 0.01 weak monobase acid . The value of dissociation contant is 4.0 xx 10^(-10)

The pH of a 0.1M solution of NH_(4)Oh (having dissociation constant K_(b) = 1.0 xx 10^(-5)) is equal to

The pH of a 0.1M solution of NH_(4)OH (having dissociation constant K_(b) = 1.0 xx 10^(-5)) is equal to

The concentration of HCN and NaCN in a solution is 0.01 M each. Calculate the concentration of hydrogen and hydroxyl ions if dissociation constant of HCN is 7.2 xx 10^(-10)

Calculate the degree of hydrolysis of 0.10 M solution of KCN. Dissociation constant of HCN = 7.2 xx 10^(-10) at 25@C and K_w = 1.0 xx 10^(-14)