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nlexa [21]
3 years ago
12

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]3 years ago
3 0

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.

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In trigonal pyramidal molecule  like molecule of ammonia , the vector some of intra- molecular dipole moment is not zero because the bonds are not symmetrically oriented . In other molecules , bonds are symmetrically oriented in space so the vector sum of all the internal dipole moment  vectors cancel each other to make total dipole moment zero.

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The half life of an isotope decay is the time transcurred when the initial amount of the isotope decays to the half of its amount.

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