Question

Which aqueous solution has a freezing point closer to its predicted value, 0.01 m NaBr or 0.01 m MgCl₂? Explain

Answer 1

NaBr will behave more ideally and have an actual freezing point closer to its predicted (theoretical) value.

What is freezing point?

The temperature at which a liquid turns into a solid under normal air pressure is known as the freezing point.

NaBr in water dissociates to $Na^{+}$ and $Br^{-}$ (two particles) while $MgCl_{2}$​ dissociating to $Mg^{2+}$ two $Br^{-}$(three particles). There is a difference between a theoretical boiling/freezing point and an experimentally determined one and the primary cause of this phenomenon is the formation of positive ions on top of negative ones and vice versa, creating an ionic environment with a net opposite charge.

In such a setting we can conclude univalent ions will behave more ideally (bivalent ions have a 'greater' charge and are therefore affecting the solution interactions more). Also, since NaBr dissociates to only two particles, we can conclude it will behave more ideally. Finally, based on these two reasons, we can conclude that out of the two given compounds, NaBr will behave more ideally and have an actual freezing point closer to its predicted (theoretical) value.

To know more about freezing point, visit: brainly.com/question/3121416

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