In the lab, you made a $2\mathrm{.}5L$ of $0\mathrm{.}95$mNaCl solution at $25C$ and $1$atm

Boiling point of water at $1$atm is $100C$

Freezing point of water at $1$atm is $0C$

Density of water at $25C$ and $1$atm is $0\mathrm{.}998\frac{g}{m}L$

Q$1$: What is the molar concentration $(M)$ of this solution?

Q$2$: In terms of intermolecular interactions, explain why would you expect this solution's vapor pressure to be lower than that of pure water.

Q$3$: What is the boiling point of this solution?

Q$4$: What is the freezing point of this solution?

Q$5$: Justify why would you rather use $1\mathrm{.}9mMgC{l}_2$ as de$-$icing salt for your icy driveway in the winter than $1\mathrm{.}9$mNaCl $?$ Show calculations to convince me$.$