The dissociation constant of a weak acid is 10^(-6) . Then the P^(H) of 0.01 Nof that acid is
The degree of ionization of a 0.1M bromoacetic acid solution is 0.132 . Calculate the pH of the solution and the pK_(a) of bromoacetic acid.
The degree of dissociation of 0.1 M weak acid is 10^(-2) and the degree of dissociation of the same acid in 0.025M concentration is '*', then find 100x. __________ ?
The degree of dissociation of an acid HA in 0.1 M solution is 0.1%. Its dissociation constant is
The ionization constant of acetic acid is 1.74xx10^(-5) . Calculate the degree of dissociation of acetic acid in its 0.05M solution. Calculate the concentration of acetate ion in the solution and its pH .
The percentage degree of hydrolysis of a salt of weak acid (HA) and weak base (BOH) in its 0.1 M solutions is found to be 10% If the molarity of the solution is 0.05M , the percentage hydrolysis of the salt should be :
Calcultae the degree of ionization of 0.05M acetic acid if its pK_(a) value is 4.74 . How is the degree of dissociation affected when its solution also contains (a)0.01M (b) 0.1M in HCl ?
HF is a weak acid but HCl is a strong acid because
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
