ions and solubility in water

[superduper12]

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why is the sodium cation, Na+, more soluble in water than the silver cation, Ag+.

Answer- silver has a greater electronegativity than sodium.

explanation - because silver is more electronegative than sodium, we expect sodium to maintain itself as a "naked" cation (not accepting electron density from the water). This leads to a large ion-dipole interaction between the sodium and water. ...water is a polar molecule, it will dissolve polar entities. the low electronegativity of sodium makes the sodium cation a better positive charge than the silver cation.

I don't understand this because shouldn't silver which is more electronegative, pull oxygen closer and thus be more soluble in water?

 

[minhaj]

a more electronegative Ag+ is more likely than Na+ to accept an electron and lose its positive charge. Since we know that ions dissolve easily, and since Na is more likely to stay in the solution as an ion, we know that it will dissolve better than Ag+.

 

[superduper12]

so what if we change the problem to Ag2+...does the charge affect this in any way.

or let me guess. since Ag2+ is more electronegative and positive than Na+, it will attract the lone pairs on the oxygen atom further. Thus Ag2+, will lose it's charge easier and becomes less soluble in water.

is this right?