Question

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 solution?

0.900 mL
1.11 mL
6.94 mL
7.20 mL

Answer 1

Hello!

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 solution?  

0.900 mL  

1.11 mL  

6.94 mL  

7.20 mL

We have the following data:

M1 (initial molarity) = 2.50 M (or mol/L)

V1 (initial volume) = 50.0 mL → 0.05 L

M2 (final molarity) = 18.0 M (or mol/L)

V2 (final volume) = ? (in mL)

Let's use the formula of dilution and molarity, so we have:

$M_{1} * V_{1} = M_{2} * V_{2}$

$2.50 * 0.05 = 18.0 * V_{2}$

$0.125 = 18.0\:V_2$

$18.0\:V_2 = 0.125$

$V_2 = \dfrac{0.125}{18.0}$

$V_2 \approx 0.00694\:L \to \boxed{\boxed{V_2 \approx 6.94\:mL}}\:\:\:\:\:\:\bf\green{\checkmark}$

Answer:

The volume is approximately 6.94 mL

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Answer 2

Answer:

C, 6.94

Explanation:

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