A 20.0 mL sample of a 0.20 M solution of the weak diprotic acid `H_(2)A` is titrated with 0.250 M NaOH. The concentration of solution at the second equivalent point is:
Decimolar weak monoprotic acid (pK_a = 4.8) is titrated with decimolar potash solution. What is the pH at equivalence point?
The pH of 0.1 M solution of weak mono protic acid is 4.0. Calculate its [H^(+)] and Ka .
A 25.0ml sample of 0.1 M HCl is titrated with 0.1 M NaOH . What is the pH of the solution at the points where 24.9 and 25.1 ml of NaOH have been added ?
10 mLof H,A (weak diprotic acid) solutions is titrated against 0.1M NaOH. pH of the solution is plotted against volume of strong base added and following observation is made. If pH of the solution at 1^(st) equivalence point is pH_(1) and at 2^(nd) equivalnee point is pH_(2) , Cal the value (pH_(2),-pH_(1)) at 25^(@) C. Given for H_(2),A, p^(Kal) =4.6 &p^(Ka2) =8
20 ml of 0.1 M NH, solution is titrated with 0.025M HCI solution. What is the pH of the reaction mixture at equivalence point at 25^(@) C ? (K_(b) "of " NH_(3) "is " 2 xx 10^(-6)) .
20 gm of sample Ba(OH)_(2) is dissolved in 10 ml of 0.5 N HCl solution, The excess of HCl was titrated with 0.2 NaOH. The volume of NaOh used was 10 mol. Calculate the % of Ba(OH)_(2) in the sample.
NARENDRA AWASTHI-IONIC EEQUILIBRIUM-Assertin-Reason Type Questions
