H2A (ACID) Molarity = 0.15 M Normality N1 = Molarity x Basicity of acid = 0.15x 2 = 0.3 N Volume V1 = 100 ml N1V1 = 0.3 x 100 = 30 NaOH (BASE) Molarity = 0.16 M Normality N2 = Molarity xAcidity of Base = 0.16 x 1 = 0.16 N Volume V2 = 100 ml N2V2 = 0.16X100 = 16 Since concentration of ACID is more than concentration of BASE, resulatant concentration is equal to H+ ion concentration. Normality at eqivalance point N = (N1V1 - N2V2)/ (V1+V2) = 30 - 16/(100+100) = 14/200 = 0.07 N = H+ ion concentartion Solution H2A (ACID) Molarity = 0.15 M Normality N1 = Molarity x Basicity of acid = 0.15x 2 = 0.3 N Volume V1 = 100 ml N1V1 = 0.3 x 100 = 30 NaOH (BASE) Molarity = 0.16 M Normality N2 = Molarity xAcidity of Base = 0.16 x 1 = 0.16 N Volume V2 = 100 ml N2V2 = 0.16X100 = 16 Since concentration of ACID is more than concentration of BASE, resulatant concentration is equal to H+ ion concentration. Normality at eqivalance point N = (N1V1 - N2V2)/ (V1+V2) = 30 - 16/(100+100) = 14/200 = 0.07 N = H+ ion concentartion.