g chemist accidentally leaves an open beaker containing 250.0 mL of a 0.500 M NaHCO3(aq) solution on a lab bench. They return a

Question

3 years ago

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g chemist accidentally leaves an open beaker containing 250.0 mL of a 0.500 M NaHCO3(aq) solution on a lab bench. They return a

few weeks later to find that the volume of the solution has decreased to 75.0 mL. What is the molarity of this partially evaporated solution, assuming the solute does not evaporate

Chemistry

1 answer:

aleksklad [387] · Answer 1 · 2022-07-25T23:02:02+03:00

Answer:

1.67 M

Explanation:

The following data were obtained from the question:

Initial volume (V1) of solution = 250 mL

Initial Molarity (M1) of solution = 0.5 M

Final volume (V2) of solution = 75 mL

Final Molarity (M2) of solution =?

Thus, we can obtain the final molarity of the solution by using the following formula:

M1V1 = M2V2

0.5 × 250 = M2 × 75

125 = M2 × 75

Divide both side by 75

M2 = 125 /75

M2 = 1.67 M

Thus, the new Molarity of the solution is 1.67 M.