Two litres of ammonia at 30^(@) C and 0.90 atmosphere pressure neutralised 134 mL of a solution of sulphuric acid . Calculate the normality of the acid .

Two litres of ammonia at 30^(@) C and 0.90 atmosphere pressure neutral

1.	Two litres of ammonia at 30^(@) C and 0.90 atmosphere pressure neutralised 134 mL of a solution of sulphuric acid . Calculate the normality of the acid .
Answer» Solution :Volume of `NH_(3)" at NTP "= (0.9 xx 273)/(303) " lit " = 1.62 ` lit . ` :. ` numbers of moles of `NH_(3)= (" volume at NTP (litres)")/(22.4)` ` = (1.622)/(22.4) = 0.0724` Number of equivalents of `NH_(3)` = number of moles `xx` factor relating mol.e wt . eq.wt . ....(Eqn. 6ii) ` = 0.0724` `{:( :."ACCORDING to the reaction "2NH_(3)+H_(2)SO_(4)to(NH_(4))_(2)SO_(4)) ,(" eq. wt of " NH_(3)"is equal to its mol.wt"):}` ` :. ` m.e of `NH_(3) ` = equivalent xx1000 ` = 0.0724 xx1000 = 72.4` Let the normality of `H_(2)SO_(4)` be N ` :. ` m.e of `H_(2)SO_(4) = N xx 134` Now m.e of `H_(2)SO_(4) ` = m.e of `NH_(3)` ...(Eqn.2) ` 134 xx N = 72.4` ` :. ` normality of `H_(2)SO_(4) = (72.4)/(134)` ` = 0.54 N `