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A 5.00 mL aliquot of a 0.20 M HCl solution is diluted to a final volume of 25.00 mL. What is the molarity of this first dilution solution? Then a second dilution was made by taking 2.00 mL of the first dilution and diluting it to 50.00 mL.g What is the molarity of this second dilution?

Respuesta :

Answer:  The molarity of this second dilution is [tex]1.6\times 10^{-3}[/tex]

Explanation:

Molarity of a solution is defined as the number of moles of solute dissolved per Liter of the solution.

According to the neutralization law,

[tex]M_1V_1=M_2V_2[/tex]

where,

[tex]M_1[/tex] = molarity of stock  solution = 0.20 M

[tex]V_1[/tex] = volume of stock  solution = 5.00 ml

[tex]M_2[/tex] = molarity of dilute  solution = ?

[tex]V_2[/tex] =  volume of dilute solution = 25.00 ml

[tex]0.20\times 5.00=M_2\times 25.00[/tex]

[tex]M_2=0.04[/tex]

The molarity of this first dilution solution is 0.04 M

[tex]M_1V_1=M_2V_2[/tex]

where,

[tex]M_1[/tex] = molarity of stock  solution = 0.04 M

[tex]V_1[/tex] = volume of stock  solution = 2.00 ml

[tex]M_2[/tex] = molarity of dilute  solution = ?

[tex]V_2[/tex] =  volume of dilute solution = 50.00 ml

[tex]0.04\times 2.00=M_2\times 50.00[/tex]

[tex]M_2=1.6\times 10^{-3}[/tex]

The molarity of this second dilution is [tex]1.6\times 10^{-3}M[/tex]

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