In the titration of `NH_(4)OH` versus `HC1`, the `pH` of the solution at equivalence point is about:

In the titration of NH_(4)OH versus HCl , the pH of the solution at equivalence point is about:

In the titration of acetic acid versus sodium hydroxide , the pH of the solution at equivalence point (whene temperature is 25^(@)C ) is :

In the titration of NH_(4)OH) with HCl, the indicator which cannot be used is :

In the titration of NH_(4)OH) with HCl, the indicator which cannot be used is :

10 mL of H_(2)A (weak diprotic acid) solution 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 first equivalence point is pH_(1) and at second equivalence 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

When 40mL of a 0.1 MN weak base, BOH is titrated with 0.01M HC1 , the pH of the solution at the end point is 5.5 . What will be the pH if 10mL of 0.10M NaOH is added to the resulting solution ?