In a school’s laboratory, students require 50.0 mL of 2.50 M H2SO4 for an experiment, but the only available stock solution of the acid has a concentration of 18.0 M. What volume of the stock solution would they use to make the required solutionA. 0.900 mL
B. 1.11 mL
C. 6.94 mL
D. 7.20 mL

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Respuesta :

Alleei Alleei · Answer 1 · 2019-12-09T05:23:40+01:00

Answer: The volume of stock solution of acid required 6.94 mL.

Explanation:

To calculate the volume of stock solution, we use the equation given by neutralization reaction:

[tex]M_1V_1=M_2V_2[/tex]

where,

[tex]M_1\text{ and }V_1[/tex] are the molarity and volume of acid which is [tex]H_2SO_4[/tex]

[tex]M_2\text{ and }V_2[/tex] are the molarity and volume of stock solution of acid.

We are given:

[tex]M_1=2.50M\\V_1=50.0mL\\M_2=18.0M\\V_2=?[/tex]

Putting values in above equation, we get:

[tex]2.50M\times 50.0mL=18.0M\times V_2\\\\V_2=6.94mL[/tex]

Hence, the volume of stock solution of acid required 6.94 mL.

william3556 william3556 · Answer 2 · 2021-01-05T08:56:26+01:00

Answer:

C) 6.94

Explanation:

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