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kotegsom [21]
3 years ago
5

A laboratory requires 2.0 L of a 1.5 M solution of hydrochloric acid (HCl), but the only available HCl is a 12.0 M stock solutio

n. How could you prepare the solution needed for the lab experiment? show all work to find your answer
Chemistry
2 answers:
ira [324]3 years ago
6 0
The amount of the solute is constant during dilution. So the mole number of HCl is 2*1.5=3 mole. The volume of HCl stock is 3/12=0.25 L. So using 0.25 L stock solution and dilute to 2.0 L.
Marat540 [252]3 years ago
5 0

<u>Answer:</u> The volume of stock HCl solution required to make laboratory solution will be 0.25L

<u>Explanation:</u>

To calculate the volume of stock solution required to make the laboratory solution, we use the equation:

M_1V_1=M_2V_2

where,

M_1\text{ and }V_1 are the molarity and volume of stock solution.

M_2\text{ and }V_2 are the molarity and volume of laboratory solution.

We are given:

M_1=12M\\V_1=?L\\M_2=1.5M\\V_2=2L

Putting values in above equation, we get:

12\times V_1=1.5\times 2\\\\V_1=0.25L

Hence, the volume of stock HCl solution required to make laboratory solution will be 0.25L

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