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Question
Q136) When 100 ml of (M/10) H_{2}SO_{4} is mixed with 500 ml of (M/10) NaOH then nature of resulting solution and normality ofexcess of reactant left is

SOLUTION

Reaction is H_{2}SO_{4} + 2NaOH → Na_{2}SO_{4}+ 2H_{2}O

One mole of H_{2}SO_{4} reacts with 2 moles of NaOH

Since both the solution have same concentration

100 ml of H_{2}SO_{4} will neutralize 200 mLof NaOH

Thus 300 mL of NaOH of 0.1M will remain reacted =0.03mole of NaOH

But after adding both the reactant volume of solution= 100+ 500 = 600 mL

And mixture have 0.03 mole of NaOH

âˆ´molarity of NaOH =

600mL =0.03 mole

1000 mL = N/20

∴ mixture will be basic, N/20

Answer: (b)