Question

How much volume of 3.0 M H2SO4 is required for preparation of 1.0 litre of 1.0 M solution?

Answer 1

Answer:

the answer is 333.3

V1M1=V2M2

3.x=1.1

1/3 =0.333l

333l

Explanation:

Answer 2

Answer: The volume of sulfuric acid needed is 0.333 L

Explanation:

To calculate the volume of the concentrated solution, we use the equation:

$M_1V_1=M_2V_2$

where,

$M_1\text{ and }V_1$ are the molarity and volume of the concentrated solution

$M_2\text{ and }V_2$ are the molarity and volume of diluted solution

We are given:

$M_1=3.0M\\V_1=?L\\M_2=1.0M\\V_2=1L$

Putting values in above equation, we get:

$3.0\times V_1=1\times 1\\\\V_1=0.333L$

Hence, the volume of sulfuric acid needed is 0.333 L