A chemistry teacher adds 50.0 mL of 1.50 M H2SO4 solution to 200 mL of water. What is the concentration of the final solution? A) 0.300 M B) 0.375 M. C) 6.00 M. D) 7.50 M.

Question

Chemistry

Kaylee Dorsey

29 August, 16:37

A chemistry teacher adds 50.0 mL of 1.50 M H2SO4 solution to 200 mL of water. What is the concentration of the final solution? A) 0.300 M B) 0.375 M. C) 6.00 M. D) 7.50 M.

+3

Answers (2)

Know the Answer?

Jared Aguilar · Answer 1

To solve this we use the expression,

M1V1 = M2V2

where M1 is the concentration of the stock solution, V1 is the volume of the stock solution, M2 is the concentration of the new solution and V2 is its volume.

1.50 M (50.0 mL) = M2 (200 mL)

M2 = 0.375 M H2SO4 solution

Therefore, the correct answer from the choices listed above is option B.

Michelle Lowe · Answer 2

To solve this question first calculate the number of moles of H2SO4 present.

C=n/v

n=c•v

n = (1.50 mol/l) (0.05 l)

n = 0.075 moles of H2SO4.

Then divide by the volume of water, to find the concentration.

C=n/v; C=0.075 mol/l / 0.2 l; C = 0.375 M

I believe it's B. 0.375M.