Question

How much volume of water need to be added to 50 ml 0.1M sodium hydroxide to make it's concentration 0.01M​

Answer 1

Normality of H
2
​
SO
4
​
=M
1
​
=0.05M
Normality of NaOH=M
2
​
=0.1M
Vol. of NaOH =V
2
​
=50ml
Vol. of H
2
​
SO
4
​
=V
1
​
=?
Now M
1
​
V
1
​
=M
2
​
V
2
​

V
1
​
=
M
1
​

M
2
​
V
2
​

​

=
0.05
0.1×50
​

Vol. of H
2
​
SO
4
​
=V
1
​
=100ml

HOPE ITS HELPFUL

Answer 2

Given:

50 ml 0.1M sodium hydroxide is diluted to make its concentration 0.01M​

To find:

The volume of water

Solution:

The initial volume of sodium hydroxide before dilution = 50 ml

The molarity of NaOH before dilution = 0.1 M

The molarity of the solution after dilution = 0.01 M

Let's assume, "V₂" represents the final volume of the solution after dilution

We know the formula of molarity is given as:

$\boxed{\bold{M_1V_1 = M_2V_2}}$

where

M₁ = Molarity before dilution

V₁ = Volume before dilution

M₂ = Molarity after dilution

V₂ = Volume after dilution

So, by substituting the values in the formula, we get

$0.1 \times 50 = 0.01 \times V_2$

$\implies 5 = 0.01 \times V_2$

$\implies V_2 = \frac{5}{0.01}$

$\implies \bold{V_2 = 500\: ml}$ ← the volume of the solution after dilution

Also, we know that ⇒ $V_2 = V_1 + V_w_a_t_e_r\:_a_d_d_e_d_$

Therefore,

The required volume of water added is,

= $V_w_a_t_e_r\:_a_d_d_e_d_$

= [Volume of the solution after dilution] - [Initial volume of NaOH before dilution]

= $V_2 - V_1$

= $500 - 50$

= $\bold{450\:ml}$

Thus, the volume of water needs to be added to 50 ml 0.1M sodium hydroxide to make its concentration 0.01M​ is → 450 ml.

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