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3 years ago

What volume of a 3.0 M stock solution of H2SO4 is needed to prepare 2.8 L of a 1.6 M H2SO4 solution?

Chemistry

2 answers:

DiKsa [7]3 years ago

5 0

<u>Answer:</u> The volume of stock solution needed is 1.5 L

<u>Explanation:</u>

To calculate the molarity of the diluted 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 stock solution

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

We are given:

$M_1=3M\\V_1=?L\\M_2=1.6M\\V_2=2.8L$

Putting values in above equation, we get:

$3\times V_1=1.6\times 2.8\\\\V_1=1.5L$

Hence, the volume of stock solution needed is 1.5 L

Georgia [21]3 years ago

4 0

Use M1V1 = M2V2 to solve
3(V1) = 2.8 * 1.6
3(V1) = 4.48
V1 = 1.493 L of stock solution

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