100 ml of 0.1 N NaOH is mixed with 100 ml of 0.1 N H2SO4.The pH of the resultant solution is??
NaOH volume = 100ml or 0.1L
Normality =0.1 N
molarity=normality= 0.1M
moles of NaOH = 0.10.1 = 0.01mol [using formula mole = C (concentration in M) V in L]
H2SO4 volume = 100ml or 0.1L
Normality= 0.1 N
number of electron change (n) for H2SO4 = 2
Thus molarity = 0.05 M ( since N = M n)
Moles of H2SO4 = 0.10.1 = 0.005 mol
0.01 mole of NaOH exactly neutralizes 0.005 mole of H2SO4 according to the reaction
NaOH + H2SO4 Na2SO4 + H2O
Thus neither NaOH is in excess nor H2SO4 therefore solution will be neutral and hence
pH= 7
Normality =0.1 N
molarity=normality= 0.1M
moles of NaOH = 0.10.1 = 0.01mol [using formula mole = C (concentration in M) V in L]
H2SO4 volume = 100ml or 0.1L
Normality= 0.1 N
number of electron change (n) for H2SO4 = 2
Thus molarity = 0.05 M ( since N = M n)
Moles of H2SO4 = 0.10.1 = 0.005 mol
0.01 mole of NaOH exactly neutralizes 0.005 mole of H2SO4 according to the reaction
NaOH + H2SO4 Na2SO4 + H2O
Thus neither NaOH is in excess nor H2SO4 therefore solution will be neutral and hence
pH= 7