The ionization constant of a weak acid is 1.6 xx 10^(-5) and the molar conductivity at infinite dilution is 380 xx 10^(-4) sm^(2) mol^(-1) . If the cell constant is 0.01m^(-1) , then conductance of 0.01M acid solution is
Derive an expression for the dissociation constant of an acid or base in terms of extent of ionisation.
Addition of sodium hydroxide solution to a weak acid (HA) results in a buffer of pH 6 . If ionisation constant of HA is 10^(-5) , the ratio of salt to acid concentration in the buffer solution will be
The first ionisation constant of oxalic acid is much greater than its second ionisation constant. Justify.
If the equlibrium constant for the reaction of weak acid HA with strong base is 10^(9) then calculate the pH of 0.1 M NaA.
Two situations are shown in fig. (a) and (b) In each case m_(1) = 3 kg and m_(2) = 4 kg . If a_(1), a_(2) are the respective accelerations of the blocks in these situations, then the values of a_(1) and a_(2) are respectively [g = 10 ms^(-2)]
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 :
At T (K ) , it the ionisation constant of ammonia in solution is 2.5 xx 10^(-5) the pH of 0.01 M ammonia solution and the ionisation constant of its conjugate acid respectively at that temperature are (log 2= 0.30)
