Molar conductivity of aqueous solution of HA is 200Scm^(2)mol^(-1),pH of this solution is 4 Calculate the value of pK_(a)(HA) at 25^(@)C . Given ^^_(M)^(oo)(NaA)=100scm^(2)mol^(-1), ^^_(M)^(oo)(HCl)=425Scm^(2)mol^(-1), ^^_(M)^(oo)(NaCl)=125 Scm^(2)mol^(-1)
At 25^(@) C dissociation constants of acid HA and base BOH in aqueous solution are same. The pH of 0.01 M solution of HA is 5. The pOH of 10^(-4) M solution of BOH at the same temperature is :
Calculate pOH of 0.1 M aq. Solution of weak base BOH (K_(b)=10^(-7)) at 25^(@)C.
H_(2) A is a weak diprotic acid. If the pH of 0.1 M H_(2)A solution is 3 and concentration of A^(2-) is 10^(-12) at 25^(@)C. Select correct statement (s)
10 mL of H_(2)A (weak diprtic acid) solutio is titrated against 0.1M NaOH. pH of the solution is plotted against volume of strong base added and following obserbation is made Ip pH of the solution at first equivalence point is pH_(1) and at secnd equibalence point is pH_(2^.) Calculate the value of (pH_(2)-pH_(1)) at 25^(@)C Given for H_(2)A,pK_(a_1) =4.6 and pK_(a_2) =8, log 25=1.4
What will be the pH of an aqueous solution of 1.0 M ammonium formate? Given : pK_(a)=3.8 and pK_(b)=4.8
When 100 mL of 0.1 M NaCN solution is titrated with 0.1 M HCl solution the variation of pH of solution with volume of HCl added will be :
The compound whose 0.1 M solution is acidic :
If degree of dissociation is 0.01 of decimolar solution of weak acid HA then pK_(a) of acid is :
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
