The concentration in M of OH^- in 0.001 M H_2SO_4 is
For the formation of NH_3 from H_2 at 500 K, The concentration of N_2, H_2 and NH_3 at equilibrium are 1.5xx10^(-2) M , 3.0 x 10^(-2) M and 1.2 xx 10^(-2) M , respectively. The equilibrium constant for the reverse reaction is
100ml 0.1M H_(3)PO_(4) is mixed with S0ml of 0.1M NaOH. What is the pH of the resultant solution? (Successive dissociation constant of H_(3) PO_(4) "are" 10^(-3) , 10^(-8) and 10^(-12) respectively ?
H_2A is a weak diptotic acid . IF the pH of 0.1 M H_2A solution is 3 and concentration of A^(2) is 10 ^(-12) " at " 25 ^(@) C Select correct statement (s)
The first and second dissociation constants of an acid H_(2)A are 10^(-5) and 5 xx 10^(-10) respectively . Then overall dissociation constant of the acid is
Initial concentration of the reactant is 1.0 M. The concentration becomes 0.9 M, 0.8 M and 0.7 M in 2 hours, 4 hours and 6 hours respectively. Then the oerder of reaction is
The dissociation coustant of H_(2)O, H _(2)Se and H_(2) Te are 1.8 xx 10 ^(-16) , 1.4 xx 10 ^(-7) , 1.3 xx 10 ^(-4)and 2.2 xx 10 ^(-3), respectively. What do these values denote ?
At 25°C the molar conductances at infinite dilution for the strong electrolytes NaOH, NaCl and BaCl_(2) are 248 xx 10^(-4) ,126 xx 10^(-4) and 280xx10^(-4)Sm^(2)mol^(-1) respectively, lambda_(m)^(o) Ba(OH)_(2) in Sm^(2)mol^(-1) is
Hydrolysis of an ester is catalysed by H^(+) ion. Using equimolar concentrations of two acids HX and HY both being strong acids. The rate constants of the reaction are found to eb 3xx10^(-3)"min"^(-1) and 5xx10^(-3)"min"^(-1) respectively at a fixed temperature. It can be concluded that.
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
