a 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? give your answer to 2 decimal places

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25-10-2022
Chemistry

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a 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? give your answer to 2 decimal places

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Qwbox Qwbox · Answer 1 · 2022-11-03T10:59:30-04:00

The molarity of this partially evaporated solution is 1.66 M.

The molarity of a solution is given by the number of moles divided by the volume of the solution as it is mentioned the solute particle do not evaporate so it means that the moles of sodium bicarbonate NaHCO₃ are constant.

So, we can write,

Moles = molarity x volume

Initial molarity x initial volume = final molarity x final volume.

Initial volume of bhai carbonate is 250 ml and 0.5M while the final volume is 75 ml and we have to find the final molarity,

Now, putting all the values,

0.5 x 250 = 75 x Final molarity.

Final molarity = 1.66M

So, the molarity of the solution after evaporation is 1.66 M

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