In each othe following compounds, which compound is likely to be more soluable in water? Please...

In each othe following compounds, which compound is likely to be more soluable in water?

Please explain your answers.

A). CCl4 or CHCl3

B). CH3OH or C6H11OH

C). NaF or MgO

D). CaF2 or BaF2

Expert Solution

A) both will not soluble in water. but CHCl3 is slightly more soluble than CCl4 because net dipole moment is zero in CCl4

B) CH3OH will soluble in water more than C6H11OH in this both can form hydrogen bonding but second one is having higher alkyl chain it will make decrease in the solubility in water

C) NaF more soluble in water than MgO because larger the size of cation more will be the ionic natureAccording to Coulomb's law, Force is proportional to charge1 x charge2 / radius squared. Since both are ionic compounds, we will be using charges in our arrow analysis. The charge on Na and F are each 1 while on Mg and O are each 2, thus the attractive force in MgO is greater than the attractive force in NaF, hence in solution, MgO tends to dissociate less since it is more difficult to break the bonds between an ionic compound with a greater attractive force compared to sodium fluoride.

D) BaF2 is more soluble in water because Ba is larger size than Ca so more will be the ionic nature more will be the soluble in water

queen_honey_blossom answered 4 hours ago

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