The pH of an aqueous solution of a 0.1M solution of a weak monoprotic acid which is 1% ionised is:

An aqueous solution whose pH= 0 is

pH of a 0.001 M solution of hydrochloric acid will be

calculate [H^(o+)] and [overset(Θ)OH] in a 0.1M solution of weak monoacitic base which is 2.0% ionised. What is the pH of solution.

The pH value of 0.001M aqueous solution of NaCl is

The dissociation constant of a weak monoprotic acid, which is 0.01 % ioniosed in 1 .00M solution , is

In aqueous solution , ethanoic acid is _______ ionised .

The specific conductivity of an aqueous solution of a weak monoprotic acid is 0.00033 ohm^(-1) cm^(-1) at a concentration 0.02 M. If at this concentration the degree of dissociation is 0.043, then calculate the value of lambda_(0) ("in" ohm^(-1)cm^(2)//eqt) :

The pH of 0.005 molar aqueous solution of sulphuric acid is approximately

pH of 0.1 M aqueous solution of weak monoprotic acid HA is 2. Calculate osmotic pressure of this solution at 27^(@)C . Take solution constant R="0.082 L atm/K-mol"

The pK_a of a weak acid (HA) is 4.5 The pOH of an aqueous buffered solution of HA in which 50% of it is ionised is