Question

How many millilitres of 0.1 M H2SO4 must be added to 50 mL of 0.1 M NaOH to give a solution that has a
concentration of 0.05 M in H2SO4?
A) 400 ml
B) 200 ml
C) 100 mL
D) None of these​

Answer 1

Answer : The correct option is, (C) 100 ml

Explanation :

The expression used will be :

$n_1M_1V_1-n_2M_2V_2=nMV$

where,

$n_1$ = basicity of an acid = 2

$n_2$ = acidity of a base = 1

$M_1$ = concentration of $H_2SO_4$ = 0.1 M

$M_2$ = concentration of NaOH = 0.1 M

$V_1$ = volume of $H_2SO_4$ = v ml

$V_2$ = volume of NaOH = 50 ml

n = basicity of an acid = 2

M = concentration of left $H_2SO_4$ = 0.05 M

V = volume of $H_2SO_4$ = (v + 50) ml

Now put all the given values in the above law, we get the volume of  $H_2SO_4$ added.

$(2\times 0.1M\times v)-(1\times 0.1M\times 50ml)=(2\times 0.05\times (v+50)ml)$

By solving the terms, we get :

$v=100ml$

Therefore, the volume of the $H_2SO_4$ added will be, 100 ml

Answer 2

Answer:

100 ML

Explanation:

HOPE I HELPS YOU