For a weak electrolyte `alpha_(1) and alpha_(2)` are in ratio of `1:2`, for a given concentration `k_(a_(1))=2xx10^(-4)`. What will be value of `k_(a_(2))`?

The degree of dissociation of weak electrolyde is inversely proportional to the square root fo concentration. It is called Ostwald's dilution law. alpha = sqrt((K_(a))/(c)) As the tempertaure increases, degree of dissociation will increase. (alpha_(1))/(alpha_(2)) = sqrt((K_(a_(1)))/(K_(a_(2)))) if concentration is same. (alpha_(1))/(alpha_(2)) = sqrt((c_(2))/(c_(1))) if acid is same. a_(1) and a_(2) are in ratio of 1:2, K_(a_(1)) = 2xx10^(-4) . What will be K_(a_(2)) ?

The degree of dissociation of weak electrolyde is inversely proportional to the square root fo concentration. It is called Ostwald's dilution law. alpha = sqrt((K_(a))/(c)) As the tempertaure increases, degree of dissociation will increase. (alpha_(1))/(alpha_(2)) = sqrt((K_(a_(1)))/(K_(a_(2)))) if concentration is same. (alpha_(1))/(alpha_(2)) = sqrt((c_(2))/(c_(1))) if acid is same. a_(1) and a_(2) are in ratio of 1:2, K_(a_(1)) = 2xx10^(-4) . What will be K_(a_(2)) ?

Weak acids and bases are not completely ionised when dissolved in polar medium like water H rarr H^(+) +A^(-) {:(t_(0),C,O,O),(t_(eq),C-Calpha,Calpha,Calpha):} K_(a)=(C alpha^(2))/(1-alpha)=Calpha^(2),alphasqrt((K_(a))/(C)) :. (alpha_(1))/(alpha_(2))=sqrt((Ka_(1))/(Ka_(2))),(alpha_(1))/(alpha_(2))=sqrt((C_(2))/(C_(1))) ( For two acids at same conc.) (for same acid at diff conc. ) alpha and alpha are in the ratio 1:2 at same conc. Ka_(1), =2xx 10^(-4) , what will be Ka_(2) ,?

If alpha and beta are roots of the equation x^(2)-3x+1=0 and a_(n)=alpha^(n)+beta^(n)-1 then find the value of (a_(5)-a_(1))/(a_(3)-a_(1))

If alpha and beta are roots of the equation x^(2)-3x+1=0 and a_(n)=alpha^(n)+beta^(n)-1 then find the value of (a_(5)-a_(1))/(a_(3)-a_(1))

A solution contains 0.1MH_(2) and 0.3MHCl. Calculate the concentration of S^(2) and HS- ions in the solution. For H_(2)S, K_(a_(1))=1.05xx10^(-7) and K_(a_(2))=1.3xx10^(-14) .

The degree of dissociation of weak electrolyde is inversely proportional to the square root fo concentration. It is called Ostwald's dilution law. alpha = sqrt((K_(a))/(c)) As the tempertaure increases, degree of dissociation will increase. (alpha_(1))/(alpha_(2)) = sqrt((K_(a_(1)))/(K_(a_(2)))) if concentration is same. (alpha_(1))/(alpha_(2)) = sqrt((c_(2))/(c_(1))) if acid is same. pH of 0.005 M HCOOH [K_(a) = 2 xx 10^(-4)] is equal to