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A mono protic acid in 1M solution is 0.01% ionized the dissociation constant of this acid is
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The dissociation constant (K_(a)) of a certain weak monoprotic acid at 298 K is 1 times 10^(-5) . The % dissociation of this acid in its decimolar aqueous solution at 298 K is
0.2 molal aqueous solution of acid HX is 20% ionised. K_f="1.86 K molal"^(-1) . The freezing point of the solution is very close to:
The 'p^H' of '0.1 M' solution of cyanic acid (HCNO) is 2.34. Calculate the ionization constant of the acid and its degree of ionization in the solution.
The molar conductivity of acetic acid solution at infinite dilution is 390.7 Omega^-1 cm^2 mol^-1 . Calculate the molar conductivity of 0.01 M acetic acid solution, given that the dissociation constant of acetic acid is 1.8 xx 10^-5
The dissociation constant of a weak monoprotic acid at 298 K is found to be numerically equal to the dissociation constant of its conjugate base. The pH of a decimolar aq. Solution of this acid at 298 K is
BRILLIANT PUBLICATION-CHEMICAL AND IONIC EQUILIBRIUM-Level - III (Linked Comprehension Type Questions)
