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VLD [36.1K]
3 years ago
8

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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The concentration of the HCl solution is 0.72 M.

<h3>How do we calculate the concentration?</h3>

Concentration of the required solution by the use of the known concentration solution will be determine by using the below equation as:

M₁V₁ = M₂V₂, where

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