Ask Question
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)
  1. 29 August, 17:37
    0
    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.
  2. 29 August, 19:44
    0
    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.
Know the Answer?
Not Sure About the Answer?
Get an answer to your question ✅ “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 ...” in 📙 Chemistry if there is no answer or all answers are wrong, use a search bar and try to find the answer among similar questions.
Search for Other Answers