What is the molarity of 200 mL of solution in which 2.0 moles of sodium bromide is dissolved?

Question

BlackTom AI · Accepted Answer

To determine molarity, we use M = moles of solute / liters of solution.
Option A: 2.0 M would imply 2.0 moles in 1.0 liter of solution. Since the given volume is 200 mL (0.200 L), this would correspond to a different amount of solute than 2.0 moles, so this is not consistent with the data.
Option B: 10 M means 10 moles per liter. With 2.0 moles dissolved in 0.200 L, the calculation is 2.0 moles / 0.200 L = 10 M, which matches the given quantities exactly.
Option C: 0.40 M would imply 0.40 moles per liter. For 2.0 moles, the required volume would be 2.0 moles / 0.40 M = 5.0 L, not 0.200 L, so this is incorrect for the provided volume.
Option D: 4.0 M would imply 4.0 moles per liter. For 2.0 moles, the necessary volume would be 2.0 moles / 4.0 M = 0.50 L, again not matching the 200 mL provided, so this option is also incorrect.
Targeting the core concept: molarity scales with the inverse of volume, so halving the volume while keeping the same moles increases M accordingly. The given numbers yield a direct 10-fold increase from 0.200 L to 10 M, consistent with 2.0 moles in 0.200 L.

What is the molarity of 200 mL of solution in which 2.0 moles of sodium bromide is dissolved?

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