When 100 ml of M/10 H2SO4 is mixed with 500 ml of M/10 NaOH then nature of resulting solution and normality of excess of reactant left is______?
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As NaOH is an excess reagent it is not totally consumed during the reaction..... so some (300ml) NaOH is left out.
Therefore, the resulting soln is basic in nature.
Then,
molarity of Na2SO4 = 0.0045/0.6=0.0 075
also molarity× n-factor = normality
so normality of the Na2SO4=0.0075× 2=0.015
Therefore, the resulting soln is basic in nature.
Then,
molarity of Na2SO4 = 0.0045/0.6=0.0 075
also molarity× n-factor = normality
so normality of the Na2SO4=0.0075× 2=0.015
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RevanthNaidu:
normality=1/2×1/10=1/20
see 300ml is left out
300ml = approx 0.01mole
so molarity is 0.01/0.6 =1/60
& nfactor of NaOH is 1
so its 1/60
not n factor it is no of moles
what is no of moles....??
How is not factor 1/2
It's n factor
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