Question

10 g of NaOH was added to 200cc of N/2(f=1.5) H2SO4. The
volume was diluted to two litres. Predict whether the dilute
solution is acidic, basic or neutral and also calculate the
resulting molarity of the dilute solution.​

Answer 1

Answer:

hey mate

Explanation:

Given weight of NaOH= 10g

Volume of H2SO4=200cc

Normality of H2SO4= (1/5)*1.5=0.75

Number of gram equivalence of NaOH= (Weight/ Equivalent weight)= (10/40)=0.25

No. of gram equivalence of H2SO4=

(Normality* volume in Lt) = (0.75*0.2) =0.15

Hence it is basic.

Now, remaining no of gram equivalence of NaOH after it neutralises H2SO4= 0.25-0.15= 0.1

Normality of diluted remaining base=(no. of gram equivalence of remaining base)/ total diluted volume in litre

= (0.1/2)

= 0.05

Finally,

Molarity= normality/ acidity

= 0.05/1

= 0.05 M

Hence the molarity of the dilute solution is 0.05 M

I hope you got it!