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3 years ago

What volume of concentrated hydrochloric acid (12.0 M HCl) is required to make 2.0 liters of a 3.0 M HCl solution?

Chemistry

2 answers:

Allushta [10]3 years ago

7 0

Given:

12.0 M HCl

2.0 liters of a 3.0 M HCl

Required:

volume of concentrated hydrochloric acid

Solution:

M1V1 = M2V2

(12.0 M HCl)V1 = (3.0 M HCl)( 2.0 liters)

V1 = (3.0 M HCl)( 2.0 liters)/ (12.0 M HCl)

V1 = 0.5 liters

valentina_108 [34]3 years ago

6 0

Answer: The volume of concentrated HCl solution is 0.5 L

Explanation:

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

$M_1V_1=M_2V_2$

where,

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

$M_2\text{ and }V_2$ = Molarity and volume of the diluted HCl solution

We are given:

$M_1=12M\\V_1=?L\\M_2=3M\\V_2=2L$

Putting values in above equation:

$12M\times V_1=3M\times 2L\\\\V_1=0.5L$

Hence, the volume of concentrated HCl solution is 0.5 L

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in the laboratory a student dilute 13.3 ml of a 10.8 m hcl solution to a total of 300.0 ml what is the concentration of the dilu

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Answer: The concentration of the diluted solution is 0.4788M

Explanation:

To calculate the concentration of the diluted solution, we use the following equation:

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