Let us assume the conc of Ba(OH)2 is known to us and initially we have known amount of Ba(OH)2 in the flask which is completely dissociated in form of Ba2+ and OH- ions. Now H2SO4 is added. H2SO4 dissociates to form H+ and SO42- ions. H+ and OH- ions form water while Ba2+ and SO42- form insoluble BaSO4 when enough H2SO4 is added to consume the Ba(OH)2 completely the conductance of the analyte which is being monitored continuosly shows a sharp decrease and is at its lowest point. at this point H2SO4 addition is stopped and titration ends. Now you know the molarity of Ba(OH)2 ...(M1) volume of Ba(OH)2 taken initially ...(V1) and volume of H2SO4 consumed ...(V2) use M1V1 = M2V2 only unknown M2 which is molarity of H2SO4 can be calculated !! Solution Let us assume the conc of Ba(OH)2 is known to us and initially we have known amount of Ba(OH)2 in the flask which is completely dissociated in form of Ba2+ and OH- ions. Now H2SO4 is added. H2SO4 dissociates to form H+ and SO42- ions. H+ and OH- ions form water while Ba2+ and SO42- form insoluble BaSO4 when enough H2SO4 is added to consume the Ba(OH)2 completely the conductance of the analyte which is being monitored continuosly shows a sharp decrease and is at its lowest point. at this point H2SO4 addition is stopped and titration ends. Now you know the molarity of Ba(OH)2 ...(M1) volume of Ba(OH)2 taken initially ...(V1) and volume of H2SO4 consumed ...(V2) use M1V1 = M2V2 only unknown M2 which is molarity of H2SO4 can be calculated !!.

1. Let us assume the conc of Ba(OH)2 is known to us and initially we have known
amount of Ba(OH)2 in the flask which is completely dissociated in form of Ba2+ and OH- ions.
Now H2SO4 is added. H2SO4 dissociates to form H+ and SO42- ions. H+ and OH- ions form
water while Ba2+ and SO42- form insoluble BaSO4 when enough H2SO4 is added to consume
the Ba(OH)2 completely the conductance of the analyte which is being monitored continuosly
shows a sharp decrease and is at its lowest point. at this point H2SO4 addition is stopped and
titration ends. Now you know the molarity of Ba(OH)2 ...(M1) volume of Ba(OH)2 taken
initially ...(V1) and volume of H2SO4 consumed ...(V2) use M1V1 = M2V2 only unknown M2
which is molarity of H2SO4 can be calculated !!
Solution
Let us assume the conc of Ba(OH)2 is known to us and initially we have known
amount of Ba(OH)2 in the flask which is completely dissociated in form of Ba2+ and OH- ions.
Now H2SO4 is added. H2SO4 dissociates to form H+ and SO42- ions. H+ and OH- ions form
water while Ba2+ and SO42- form insoluble BaSO4 when enough H2SO4 is added to consume
the Ba(OH)2 completely the conductance of the analyte which is being monitored continuosly
shows a sharp decrease and is at its lowest point. at this point H2SO4 addition is stopped and
titration ends. Now you know the molarity of Ba(OH)2 ...(M1) volume of Ba(OH)2 taken
initially ...(V1) and volume of H2SO4 consumed ...(V2) use M1V1 = M2V2 only unknown M2
which is molarity of H2SO4 can be calculated !!